2 Sodium azide, NaN, is used in automotive air bags. Upon decomposition, it produces sodium and nitrop gas: 2NAN,(s) → Na(s) + 3N,(g). The nitrogen gas liberated in this reaction inflates the air bag. moles of N, are produced by the decomposition of 2.50 moles of NaN,? How many a. b. How many grams of NaN, are required to form 10 g of nitrogen gas? c. How many grams of NaN, are require to produce 20 L of nitrogen gas gas leium hvdrovide and hydrogen gas if the has a density of 1.25

2 Sodium azide, NaN, is used in automotive air bags. Upon decomposition, it produces sodium and nitrop gas: 2NAN,(s) → Na(s) + 3N,(g). The nitrogen gas liberated in this reaction inflates the air bag. moles of N, are produced by the decomposition of 2.50 moles of NaN,? How many a. b. How many grams of NaN, are required to form 10 g of nitrogen gas? c. How many grams of NaN, are require to produce 20 L of nitrogen gas gas leium hvdrovide and hydrogen gas if the has a density of 1.25

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Fe2O3(s) + 2Al(s) → 2Fe(l) + Al2O3(s) a. What mass of Fe(l) will be produced if 15.0 g of Fe2O3 is used? b. What is the mass of Al need to completely react with 15.0 g of Fe2O3?
Automotive airbags a inflate when sodium azide decomposers exclusively to its constituent elements 2NaN3(s)---->2Na(s)+3N2(g) how many moles of N2 are produced by the decomposition of 1.88 more of sodium azide
21. Tungsten reacts with Cl2 to form WCl6 according to the following balanced equation: W + 3 Cl2 ==> WCl6 Determine the mass of WCl6 that forms when 231.80 g of W completely react. Molar Mass, g/mol W 183.91 Cl2 70.91 WCl6 396.56
What mass of H2S will form when 200 g aluminum sulfide react with 144 g water, how many atoms of the excess group VI (O or S in the respective compound) are in excess, given the unbalanced reaction… Al2S3 + H2O à Al(OH)3 + H2S
Dimethylnitrosamine, (CH3)N2O , is a carcinogenic (cancer-causing)substance that may be formed in foods, beverages, or gastricjuices from the reaction of nitrite ion (used as a food preservative) with other substances.a.What is the molar mass of dimethylnitrosamine?b. How many moles of (CH3) N2O molecules are present in 250 mgdimethylnitrosamine?c. What is the mass of 0.050 mole of ciimethylnitrosamine?d. How many atoms of hydrogen arein 1.0 mole of dimethylnitrosamine?e. What is the mass of 1.0 x 106 molecules of dimethylnitrosamine?f. What is the mass in grams of one molecule of dimethylnitrosamine?
2. Octane (a common organic solvent, and a major component of gasoline, mol formula: C8H18) burns in the presence of oxygen. The combustion produces carbon dioxide, water, and heat. If we burn 325.2 g of octane, determine: a. The balanced chemical equation for the combustion reaction (you can omit heat) b. The mass of oxygen consumed in the reaction
76)A mixture of hydrazine (N2H4) and hydrogen peroxide (H2O2) is used as a fuel for rocket engines. These two substances react as shown by the equation: N2H4 + 2H2O2 N2 + 4H2O. What mass of N2H4, in grams, is needed to react completely with 35.0 g of H2O2?
A student weighs out 8.00g of fertilizer. After performing the experiment, the student obtains 5.85 g of product. a. What is the actual % P?
8. Use the following equation for the following: ni 916 2siuosiom ynsm woll Mg3N2 + H₂O → Mg(OH)2 + NH3 20000.0 6 a. Balance the equation. IX IX. b. How many moles of NH3 are produced when 0.0425 moles of Mg3N2 are reacted? c. How many grams of H₂O are needed to form 6.31 x 10-5 moles of Mg(OH)2 ? d. How many molecules of H₂O are needed to react with 0.525 lbs Mg3N₂? e. How many kilograms of Mg(OH)2 are produced when 7.23 x 1027 molecules of NH3 are also produced? f. How many grams of Mg3N2 are needed to make 4.18 lb Mg(OH)2 ?
3. Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO₂), a dark brown gas. In one experiment 0.87 mol of NO is mixed with 0.50 mol of O₂. a. Determine the limiting reagent. b. Calculate the number of moles of NO₂ produced.
3. Consider the following balanced reaction: 2 Fe + 3 Cl₂ → 2 FeCl3 Given 60.0 g of Fe and excess Cl₂ (as much as we need), calculate: a. The theoretical yield of FeCl3, in grams. b. The theoretical amount of Cl₂ consumed, in grams.
The combustion of propane (C3H8) produces CO2 and H20: C3H8 (g) + 502 (g) – 3C02 (g) + 4H20 (g)The reaction of 2.5 mol of 02 (molar mass: 32:00 g/mol) with 4.6 mol of C3H8 (molar mass: 44.10 g/mol) will produce. mol of H20 (molar mass: 18.01 g/mol). Select one: a.3,68 b.2.76 c.2.0 d.1.5 e.36.02