ammonia reacts with oxygen to produce nitrogen monoxide and water
The balanced form of the given equation is. What mass of oxygen gas is consumed by the reaction of 2.7g of ammonia? Explanation: A Computer Science portal for geeks. Assume all gases are at the same temperature and pressure. b). In a closed system, equal amounts of ammonia and oxygen react to produce nitrogen monoxide and water. (c) Give the amount of the excess reac, Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3NO2(g)+H2O(l)?2HNO3(l)+NO(g) Suppose that 4.0 mol NO2 and 0.50 mol H2O combine and react comp. If 7.35 L of nitrogen gas and 26.04 L of hydrogen gas were allowed to react, how many liters of ammonia gas could form? 4NH3 + 5O2 4NO + 6H2O The reaction above can mean: 4 molecules of NH 3 reacts with 5 molecules of O 2 to produce 4 molecules of NO and 6 molecules of H 2O. But you have only 100 g of oxygen. Methane is a hydrocarbon, which means it reacts with oxygen to produce carbon dioxide and water only as follows: methane + oxygen carbon dioxide + water. How many liter of NO are produced when 2.0 liters of oxygen reacts with ammonia? Ammonia gas reacts with molecular oxygen gas to form nitrogen monoxide gas and liquid water. All replies Expert Answer 2 months ago The chemical reaction is as follows - Ammonia is produced by the reaction of hydrogen and nitrogen. Identify the excess reagent, as well as how many grams of the excess reagent will remain when the reaction reaches completion. The balanced chemical equation for this reaction along with all the correct symbols for all the reactant and the products is given below - 4N H3(aq)+3O2(g) 2N 2(g)+6H2O(l) Suggest Corrections 9 Similar questions Nitrogen dioxide is a chemical compound with the formula NO 2.It is one of several nitrogen oxides. Ammonia {eq}(NH_3) Urea (NH_2)_2CO is prepared by reacting ammonia with carbon dioxide. But you have only 100 g of oxygen. How can a chemical equation be made more informative? Write the balanced equation for the reaction of nitrogen gas with hydrogen gas to form ammonia gas. In the first step of nitric acid manufacturing, nitric oxide (NO) is formed by reaction of NH 3 and O 2 in 850 - 1000 0 C temperature. Nitric acid is a component of acid rain that forms when gaseous nitrogen dioxide pollutant reacts with gaseous oxygen and liquid water to form aqueous nitric acid. Ammonia is formed by reacting nitrogen and hydrogen gases. In this example, let's start with ammonia:
\r\n![\"image2.jpg\"](\"https://www.dummies.com/wp-content/uploads/476717.image2.jpg\")
\r\nThe calculation reveals that you'd need 235 g of oxygen gas to completely react with 100 g of ammonia. 8.7 mol C. 4.4 mol D. 5. How many liters of ammonia at STP are produced when 10 g of hydrogen is combined with nitrogen? Dummies helps everyone be more knowledgeable and confident in applying what they know. Ammonia gas is obtained by the reaction of hydrogen gas and nitrogen gas. b. You'll discover one of two things: either you have an excess of the first reagent, or you have an excess of the second reagent. {/eq}. The reactant that is used up is the limiting reagent.\r\n\r\nChemists need to know which reactant will run out first, because that information allows them to deduce how much product and excess reagent they can expect, based on how much of the limiting reagent they've put into the reaction.\r\n
In any chemical reaction, you can simply pick one reagent as a candidate for the limiting reagent, calculate how many moles of that reagent you have, and then calculate how many grams of the other reagent you'd need to react both to completion. Selective non-catalytic reduction reduces NOx up to 70%. Question: Ammonia gas and oxygen gas react to form water vapor and nitrogen monoxide gas. NH + O = NO + HO Balanced Equation Ammonia,Oxygen equal to Nitrogen Monoxide+Water Balanced EquationRELATED SEARCHESammonia oxygen nitrogen monoxide water. Chemistry Stoichiometry Stoichiometry. (b) Find the theoretical yield of water, in grams. Ammonia burns in oxygen according to the following equation: 4NH_3 + 3O_2 \rightarrow 2N_2 + 6H_2O How many moles of nitrogen gas are generated by the complete reaction of 6.65 moles of ammonia? Ammonia and oxygen react to form nitrogen and water, like this: 4NH_3(g) + 3O_2(g) => 2N_2(g) + 6H_2O(g). Given the balanced chemical equation. If 6.42 g of each reactant are used, what is the theoretical mass, in grams, of ammonia that will be produced? Chemists need to know which reactant will run out first, because that information allows them to deduce how much product and excess reagent they can expect, based on how much of the limiting reagent they've put into the reaction. You'll run out of oxygen before you run out of ammonia, so oxygen is the limiting reagent.
\r\n\r\n \tIdentify the excess reagent, as well as how many grams of the excess reagent will remain when the reaction reaches completion.
\r\nTo calculate how many grams of ammonia will be left at the end of the reaction, assume that all 100 g of oxygen react:
\r\n![\"image3.jpg\"](\"https://www.dummies.com/wp-content/uploads/476718.image3.jpg\")
\r\nThis calculation shows that 42.5 g of the original 100 g of ammonia will react before the limiting reagent is expended. Solid iron (III) oxide reacts with hydro gen gas to form solid iron and liquid water. When ammonia gas is burned in oxygen the products formed are water and nitrogen monoxide gas. Nitrogen monoxide gas is formed by the reaction of oxygen gas and nitrogen gas. You'll run out of oxygen before you run out of ammonia, so oxygen is the limiting reagent.
\r\nIdentify the excess reagent, as well as how many grams of the excess reagent will remain when the reaction reaches completion.
\r\nTo calculate how many grams of ammonia will be left at the end of the reaction, assume that all 100 g of oxygen react:
\r\n\r\nThis calculation shows that 42.5 g of the original 100 g of ammonia will react before the limiting reagent is expended. A. NO 2 dissolves very well in water react with water to give nitrous acid and nitric acid. Dummies has always stood for taking on complex concepts and making them easy to understand. Write and balance the chemical equation. A chemical equation has two sides separated by the arrow which is called the reaction arrow. {/eq} to produce nitrogen monoxide (NO) and water {eq}(H_2O) Nitric acid is a component of acid rain that forms when gaseous nitrogen dioxide pollutant reacts with gaseous oxygen and liquid water to form aqueous nitric acid. Merely said, the ammonia reacts with oxygen to produce nitrogen monoxide and water is universally compatible in imitation of any devices to read. (Assume an, (a) Write the balanced chemical equation that represents the reaction described by words, and then perform calculations to answer parts (b) and (c). When 36.3 L of ammonia and 39.0 L of oxygen gas at STP burn, nitrogen monoxide and water are produced. Given the balanced chemical equation. 4 NH_3 + 5 O_2 to 4 NO + 6 H. Given the reaction between ammonia and oxygen as 4NH3 + 5O2 \rightarrow 4NO + 6H2O: Calculate the amount of nitrogen monoxide (in grams) produced if 0.5 g of ammonia is reacted with 0.5 g of oxygen. If the reaction uses up 9.43*10^5 g of ammonia, how many kilograms of nitrogen monoxide will be formed? NO + 3/2H2O ---> NH3 + 5/4O2. When 6 liter of nitrogen gas reacts with 18 liters of hydrogen gas at constant temperature and pressure, how many liters of ammonia gas will be produced? When 8.5 g of ammonia is allowed to react with an excess of O_2, the reaction produces 12.0 g of nitrogen monoxide. Nitrogen monoxide can be prepared by the oxidation of ammonia by the following equation: 4NH3 (g) + 5O2 (g) > 4NO (g) + 6H2O (g). Besides, specific value-added products can be produced by an appropriate . Ammonia is often produced by reacting nitrogen gas with hydrogen gas. Write a balanced equation for this reaction. If 11.2 g of. Which reagent is the limiting reagent. Determine how much ammonia would be produced if 100.0 g of hydrogen reacts. Ammonia is produced by synthesizing nitrogen and hydrogen gas, if i have 2 moles of nitrogen gas and 5 moles of hydrogen gas. 2NH 3 (g). Ammonia reacts with oxygen gas to form nitrogen monoxide and water. Ammonia and oxygen without catalyst | NH 3 + O 2 N 2 + H 2 O. Gaseous sulfur trioxide and gaseous nitrogen monoxide form when gaseous sulfur dioxide and gaseous nitrogen dioxide react. Ammonia and oxygen combine to form nitrogen monoxide and water by the chemical reaction: 4 N H 3 ( g ) + 5 O 2 ( g ) 4 N O ( g ) + 6 H 2 O ( l ) If 100 grams of ammonia are reacted with 100 grams of oxygen, a. `One way to make ammonia is to synthesize it directly from elemental nitrogen and hydrogen (though this isn't that easy). Ammonia (NH_3) reacts with oxygen (O_2) to produce nitrogen monoxide (NO) and water (H_2O). Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3NO_2(g)+H_2O(l) to 2HNO_3(l)+NO(g) Suppose that 4.3 mol NO_2 and 0.80 mol H_2O combine and react completely. N29g)+3H2 (g) --> 2nh3 (g) Ammonia and oxygen produce nitrogen dioxide and water. 8NH3 + 3Cl 2 N2 + 6NH4Cl. Balance the equation for the reaction. Write the unbalanced chemical equation for this process. In a chemical reaction between nitrogen and hydrogen, 5.0 moles of hydrogen are reacted with excess nitrogen. This problem has been solved! This allows you to see which reactant runs out first. Round your answer to 2 significant digits. How many liters of NO are produced when 2.0 liters of oxygen reacts, Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation: N_2(g) + 3H_2(g) rightarrow 2NH_3(g) 1. When ammonia gas is burned in oxygen the products formed are water and nitrogen monoxide gas. Ammonia may be oxidized to nitrogen monoxide in the presence of catalysts according to the equation 4NH_3 + 5O_2 gives 4NO and 6H_2O. What mass of ammonia is consumed by the reaction pf 6.1g of oxygen gas? What is the balanced equation for nitrogen, water, and oxygen, which are all produced by the decomposition of ammonium nitrate? Createyouraccount. Hydrogen gas, H_2, reacts with nitrogen gas, N_2, to form ammonia gas, NH_3, according to the equation 3H_2 (g) + N_2 (g) to 2 NH_3 (g) How many moles of NH_3 can be produced from 13.5 mol of H_2 and excess N_2? Construct your own balanced equation to determine the amount of NO and H2O that would form when 2.08 mol of NH3 6.32 mol of O2 react Expert's answer 4NH 3 +5O 2 ---->4NO+6H 2 O In this example, let's start with ammonia:
\r\n\r\nThe calculation reveals that you'd need 235 g of oxygen gas to completely react with 100 g of ammonia. Calculate the number of grams of ammonia needed to form 40.12 moles of nitrogen monoxide. Given the reaction between ammonia and oxygen as 4NH3 + 5O2 \rightarrow 4NO + 6H2O: Calculate the amount of nitrogen monoxide (in grams) produced if 0.5 g of ammonia is reacted with 0.5 g of oxygen. Write the chemical equation for the following reaction. How many liters of ammonia gas can be formed from the complete reaction of 150 l of hydrogen gas with excess nitrogen gas at 25 degree C and 1 atm? Ammonia is allowed to react with diatomic oxygen to form nitric oxide and water. in the presence of catalyst according to the equation 4 NH3 + 5 O2 gives 4 NO and 6 H2O. Write and balance the chemical equation. You start with 100 g of each, which corresponds to some number of moles of each. In India on the occasion of marriages the fireworks class 12 chemistry JEE_Main, The alkaline earth metals Ba Sr Ca and Mg may be arranged class 12 chemistry JEE_Main, Which of the following has the highest electrode potential class 12 chemistry JEE_Main, Which of the following is a true peroxide A rmSrmOrm2 class 12 chemistry JEE_Main, Which element possesses the biggest atomic radii A class 11 chemistry JEE_Main, Phosphine is obtained from the following ore A Calcium class 12 chemistry JEE_Main, Differentiate between the Western and the Eastern class 9 social science CBSE, NEET Repeater 2023 - Aakrosh 1 Year Course, CBSE Previous Year Question Paper for Class 10, CBSE Previous Year Question Paper for Class 12. The . be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. How many liters of nitrogen will be produced at STP? 637.2 g of ammonia are reacted with 787.3 g of carbon dioxide. 4. Balanced Equation: Ammonia reacts with oxygen to produce nitrogen oxide and water. B. 3H2 + N2 arrow 2NH3; Delta H = -96 kJ Write the balanced chemical equation for a reaction involving these substances with a Delta H = 192 kJ change in. Ammonia reacts with oxygen to form nitrogen monoxide, NO, & water. Nitrogen of ammonia is oxidized to nitrogen gas from -3 oxidation state to 0 oxidation state. Ammonia (NH3) reacts with oxygen (O2) to form air pollutant nitrogen oxide (NO) and water. Peter J. Mikulecky, PhD, teaches biology and chemistry at Fusion Learning Center and Fusion Academy. Otherwise, we can say, NO 2 is one of the strong acidic gas in chemistry. How many liters of NO are. Nitrogen gas combines with hydrogen gas to produce ammonia. What is the limiting reactant and how many grams of ammonia is formed? Which reactant is in excess? The one you have in excess is the excess reagent. The one that isn't in excess is the limiting reagent.
\r\nHere's an example. Say you are conducting an experiment where ammonia reacts with oxygen to produce nitrogen monoxide and liquid water:\r\n\r\n![\"image0.jpg\"](\"https://www.dummies.com/wp-content/uploads/476715.image0.jpg\")
\r\n\r\nIn order to find the limiting reagents, excess reagents, and products in this reaction, you need to do the following:\r\n- \r\n \t
- \r\n
Balance the equation.
\r\n \r\n \t - \r\n
Determine the limiting reagent if 100 g of each reagent are present at the beginning of the reaction.
\r\n \r\n \t - \r\n
Identify the excess reagent, as well as how many grams of the excess reagent will remain when the reaction reaches completion.
\r\n \r\n \t - \r\n
Calculate how many grams of each product will be produced if the reaction goes to completion.
\r\n \r\n
- \r\n \t
- \r\n
Balance the equation.
\r\nBefore doing anything else, you must have a balanced reaction equation. How can I balance this equation? II. After the products return to STP, how many grams of nitrogen monoxide are present? 1. Round your answer to significant digits. Be sure to include the state of, A) Nitrogen gas and chlorine gas will react to form nitrogen monochloride gas. Ammonia NH_{3} chemically reacts with oxygen gas O_{2} to produce nitric oxide NO and water H_{2}O What mass of nitric oxide is produced by the reaction of 7.0''g'' of ammonia? The balanced chemical reaction for the formation of ammonia from its elements is N2(g)+3H2(g)---2NH3(g).What is DeltarxnG for this reaction? 4NH_3 + 5O_2 to 4NO. How many moles of nitrogen gas are produced when 20 grams of ammonia react with 25 grams of oxygen gas? (a) Write a balanced chemical equation for this reaction. The fuel, typically coal or biomass, is reacted with oxygen or air to produce a 'synthesis gas' (syngas) composed of carbon monoxide, carbon dioxide and hydrogen. Solid ammonium nitrite decomposes to produce gaseous nitrogen and water vapor. If 6.42g of water is produced, how many grams of oxygen gas reacted? Nitrogen monoxide can be formed according to the equation: N2(g) + 2O2(g) -> 2NO2(g) If 8.0 L of nitrogen is reacted at STP (this is important), exactly how many liters of oxygen at STP would be needed to allow complete reaction? The reactant that is used up is the limiting reagent.\r\n\r\nChemists need to know which reactant will run out first, because that information allows them to deduce how much product and excess reagent they can expect, based on how much of the limiting reagent they've put into the reaction.\r\n
In any chemical reaction, you can simply pick one reagent as a candidate for the limiting reagent, calculate how many moles of that reagent you have, and then calculate how many grams of the other reagent you'd need to react both to completion. Calculate the number of moles of hydrogen required to react with 0.0767 moles of nitrogen, and the number of moles of ammonia that will. Write the chemical equation for the detonation reaction of this explosive. Calculate the number of grams of ammonia needed to form 40.12 moles of nitrogen monoxide. If 45.7 g of NH3 and excess of O2 react together, how many grams of NO must be produced to have an 85% yield? How many moles of oxygen gas are needed to react with 23 moles of ammonia? Scale it down to 2 L O2. Phase symbols are optional. Balance each equation in the mechanism showing formation of ozone (O_3) in the upper atmosphere. With supply of heat, ammonia reacts with oxygen and produce nitrogen gas and water as products. Write the equation that represents "nitrogen and oxygen react to form nitrogen dioxide. Given the equation N2(g) + 3H2(g) = 2NH3(g) determine how many moles of NH3 are produced when 1.4 mol of H2 reacts?Ammonia is produced by the reaction of hydrogen and nitrogen. Don't waste time or good thought on an unbalanced equation. ________ mol NO 3.68 To determine the grams of nitrogen monoxide that are generated by the complete reaction of oxygen, start with the assumption that all 100 g of the oxygen react:
\r\n![\"image4.jpg\"](\"https://www.dummies.com/wp-content/uploads/476719.image4.jpg\")
\r\nSo, 75 g of nitrogen monoxide will be produced.
\r\nAgain, assume that all 100 g of the oxygen react in order to determine how many grams of water are produced:
\r\n![\"image5.jpg\"](\"https://www.dummies.com/wp-content/uploads/476720.image5.jpg\")
\r\nYou find that 67.5g of water will be produced.
\r\n \r\n
Christopher Hren is a high school chemistry teacher and former track and football coach. Urea is used as a fertilizer because it can react with water to release ammonia, which provides nitrogen to plants. d. Gaseous ammonia (NH3) reacts with gaseous oxygen to form gaseous nitrogen monoxide and gaseous water. What volume of nitrogen monoxide would be produced by this reaction if 4.7 mL of ammonia were consumed? The balanced reaction of ammonia and oxygen is shown below. N_2 + O_2 rightarrow NO (b) Then. For the CO if you were to use it up completely you would use up 12.7 mols of CO. You need twice as much H2 as CO since their stoichiometric ratio is 1:2. a). Nitrogen, N_2, combines with hydrogen, H_2, to form ammonia, NH_3. If the total pressure of the gas at the end of the rea. Use this chemical equation to answer the following questions: 1) Write a balanced equation, including physical state for the reverse reaction. The ammonia used to make fertilizers is made by reacting nitrogen of the air with hydrogen. 6134 views Use atomic masses: N: 14.01; H: 1.01; O: 16.00; Ca: 40.08 CaO (s) + NH4Cl (s) \rightarrow NH3 (g) + H2O (g) + CaCl2 (s) a. Give the balanced equation for this reaction. Chemistry. (a) First, nitrogen and oxygen gas react to form nitrogen oxide. Gaseous ammonia chemically reacts with oxygen O2 gas to produce nitrogen monoxide gas and water vapor. Ammonia is formed by reacting nitrogen and hydrogen gases. What mass of ammonia is consumed by the reaction of 6.48 grams of oxygen gas? Which of the two. How can I know the relative number of moles of each substance with chemical equations? The density of nitrogen monoxide at 25 degrees Celsius is 1.23 g/L. Write a balanced chemical equation for this reaction. Determine the mass in grams of ammonia formed when 1.34 moles of N2 react. Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 grams of ammonia is reacted with 12.0 grams of oxygen at 25 degrees Celsius. ", Virtually all the nitric acid manufactured commercially is obtained by the ammonia oxidization process. Calculate the number of moles of hydrogen required to react with 0.0767 moles of nitrogen, and the number of moles of ammonia that will, 1) Nitrogen dioxide reacts with water to form nitric acid 1) Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3NO2(g)+H2O(l)-->2HNO3(l)+NO(g) S, Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO_2 (g)+ H_2O (l) to 2HNO_3 (l) + NO (g). Nitrogen dioxide reacts with water to produce oxygen and ammonia: 4NO2 (g)+6H2O (g)7O2 (g)+4NH3 (g) How many grams of NH3 can be produced when 4.10 L of NO2 reacts at 385 C and 735 mmHg ? Ammonia reacts with oxygen to produce nitrogen oxide and water. 2HNO_3(l) + NO(g) Part A Suppose that 4 8 mol NO_2 and 1.1 mol H_2O combin. Our experts can answer your tough homework and study questions. If 15.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced at STP? This species plays an important role in the atmosphere and as a reactive oxygen . Nitrogen atoms donate four electrons to form N4+ ions and oxygen atoms gain two electrons to form O2 ions when nitrogen and oxygen form an ionic bond. Suppose you were tasked with producing some nitrogen monoxide. The balanced form of the given equation is
\r\n![\"image1.jpg\"](\"https://www.dummies.com/wp-content/uploads/476716.image1.jpg\")
\r\nTwo candidates, NH3 and O2, vie for the status of limiting reagent. b. To determine the grams of nitrogen monoxide that are generated by the complete reaction of oxygen, start with the assumption that all 100 g of the oxygen react: So, 75 g of nitrogen monoxide will be produced. Write a balanced chemical equation of this reaction. Change the grams of NH3 to moles of NH3. For the reaction represented by the equation N_2 + 3H_2 to 2NH_3, how many moles of nitrogen are required to produce 18 mol of ammonia? Stoichiometry : the numerical relationship between chemical quantities in a balanced chemical equation. Round your answer to 2 significant d. Ammonia (NH_3) is formed industrially by reacting nitrogen and hydrogen gases. The balanced equation for this reaction is: 4NH3 (g) + 502 (g) 4NO (g) + 6H2O (g) Suppose 16.7 moles of ammonia react. The one you have in excess is the excess reagent. For this calculation, you must begin with the limiting reactant. b. If 112 grams of nitrogen gas is allowed to react wit. Our experts can answer your tough homework and study questions. In order to find the limiting reagents, excess reagents, and products in this reaction, you need to do the following: Determine the limiting reagent if 100 g of each reagent are present at the beginning of the reaction. The one you have in excess is the excess reagent. The one that isn't in excess is the limiting reagent.
\r\nHere's an example. Say you are conducting an experiment where ammonia reacts with oxygen to produce nitrogen monoxide and liquid water:\r\n\r\n\r\n\r\nIn order to find the limiting reagents, excess reagents, and products in this reaction, you need to do the following:\r\n- \r\n \t
- \r\n
Balance the equation.
\r\n \r\n \t - \r\n
Determine the limiting reagent if 100 g of each reagent are present at the beginning of the reaction.
\r\n \r\n \t - \r\n
Identify the excess reagent, as well as how many grams of the excess reagent will remain when the reaction reaches completion.
\r\n \r\n \t - \r\n
Calculate how many grams of each product will be produced if the reaction goes to completion.
\r\n \r\n
- \r\n \t
- \r\n
Balance the equation.
\r\nBefore doing anything else, you must have a balanced reaction equation. 2S (s)+3O2 (g) --> 2SO3 (g) 1.09 1024 molecules oxygen Reacting 3.00 mol nitrogen gas with 3.59 mol hydrogen gas will produce how many moles of ammonia according to the following balanced chemical equation? 4NH3 + O2 = 6NO + 6H2O a. how many grams of oxygen are needed to react with 0.15 moles of ammonia? Who is the Limiting Reactio? When ammonia (NH_3^(2-)) reacts with dinitrogen oxide (N_2O), the products of the reaction are H_2O(l) and nitrogen gas. Write a balanced chemical equation for this reaction. Except where otherwise noted, data are given for materials in their standard state (at 25 C [77 F], 100 kPa). Ammonia chemically reacts with oxygen gas to produce nitric oxide and water. How many grams of oxygen do you need to react with 21.4 g ammonia? Ammonia chemically reacts with oxygen gas to produce nitric oxide and water . ","hasArticle":false,"_links":{"self":"https://dummies-api.dummies.com/v2/authors/9161"}},{"authorId":9160,"name":"Chris Hren","slug":"chris-hren","description":"
Christopher Hren is a high school chemistry teacher and former track and football coach. ","noIndex":0,"noFollow":0},"content":"In real-life (substances present at the start of a chemical reaction) convert into product. ","hasArticle":false,"_links":{"self":"https://dummies-api.dummies.com/v2/authors/9160"}}],"primaryCategoryTaxonomy":{"categoryId":33762,"title":"Chemistry","slug":"chemistry","_links":{"self":"https://dummies-api.dummies.com/v2/categories/33762"}},"secondaryCategoryTaxonomy":{"categoryId":0,"title":null,"slug":null,"_links":null},"tertiaryCategoryTaxonomy":{"categoryId":0,"title":null,"slug":null,"_links":null},"trendingArticles":null,"inThisArticle":[],"relatedArticles":{"fromBook":[{"articleId":253707,"title":"How to Make Unit Conversions","slug":"make-unit-conversions","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"https://dummies-api.dummies.com/v2/articles/253707"}},{"articleId":251836,"title":"How to Convert between Units Using Conversion Factors","slug":"convert-units-using-conversion-factors","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"https://dummies-api.dummies.com/v2/articles/251836"}},{"articleId":251010,"title":"How to Build Derived Units from Base Units","slug":"build-derived-units-base-units","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"https://dummies-api.dummies.com/v2/articles/251010"}},{"articleId":251005,"title":"How to Do Arithmetic with Significant Figures","slug":"arithmetic-significant-figures","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"https://dummies-api.dummies.com/v2/articles/251005"}},{"articleId":250992,"title":"How to Add and Subtract with Exponential Notation","slug":"add-subtract-exponential-notation","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"https://dummies-api.dummies.com/v2/articles/250992"}}],"fromCategory":[{"articleId":253707,"title":"How to Make Unit Conversions","slug":"make-unit-conversions","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"https://dummies-api.dummies.com/v2/articles/253707"}},{"articleId":251836,"title":"How to Convert between Units Using Conversion Factors","slug":"convert-units-using-conversion-factors","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"https://dummies-api.dummies.com/v2/articles/251836"}},{"articleId":251010,"title":"How to Build Derived Units from Base Units","slug":"build-derived-units-base-units","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"https://dummies-api.dummies.com/v2/articles/251010"}},{"articleId":251005,"title":"How to Do Arithmetic with Significant Figures","slug":"arithmetic-significant-figures","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"https://dummies-api.dummies.com/v2/articles/251005"}},{"articleId":250992,"title":"How to Add and Subtract with Exponential Notation","slug":"add-subtract-exponential-notation","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"https://dummies-api.dummies.com/v2/articles/250992"}}]},"hasRelatedBookFromSearch":false,"relatedBook":{"bookId":282070,"slug":"chemistry-workbook-for-dummies-with-online-practice-3rd-edition","isbn":"9781119357452","categoryList":["academics-the-arts","science","chemistry"],"amazon":{"default":"https://www.amazon.com/gp/product/1119357454/ref=as_li_tl?ie=UTF8&tag=wiley01-20","ca":"https://www.amazon.ca/gp/product/1119357454/ref=as_li_tl?ie=UTF8&tag=wiley01-20","indigo_ca":"http://www.tkqlhce.com/click-9208661-13710633?url=https://www.chapters.indigo.ca/en-ca/books/product/1119357454-item.html&cjsku=978111945484","gb":"https://www.amazon.co.uk/gp/product/1119357454/ref=as_li_tl?ie=UTF8&tag=wiley01-20","de":"https://www.amazon.de/gp/product/1119357454/ref=as_li_tl?ie=UTF8&tag=wiley01-20"},"image":{"src":"https://www.dummies.com/wp-content/uploads/chemistry-workbook-for-dummies-3rd-edition-cover-9781119357452-204x255.jpg","width":204,"height":255},"title":"Chemistry Workbook For Dummies with Online Practice","testBankPinActivationLink":"","bookOutOfPrint":false,"authorsInfo":"
Christopher Hren is a high school chemistry teacher and former track and football coach.
