Determine the number of moles of gas particles produced when the following amounts of each chemical are decomposed. Use the balanced chemical equations to explain how these values were determined. Table 3. Number of moles of gas produced by decomposition #moles gas Substance sodium azide (NaN3) 1 mole 2 moles ammonium nitrate (NH4NO3) 1 mole 2 moles nitroglycerin (C₂H5N309) 1 mole 2 moles particles produced 1.5 3 3 6 7.25 14.5 2 NaN3 (s) → 2 Na (s) + 3 N2 (g) 1 NH4NO3 (s) →1 N20 (g)+ 2 H2O (g) 4 C3H5N309 (1)→ 12 CO2 (g) + 10 H20 (1) +6 N2 (g) + 02 (g)

Determine the number of moles of gas particles produced when the following amounts of each chemical are decomposed. Use the balanced chemical equations to explain how these values were determined. Table 3. Number of moles of gas produced by decomposition #moles gas Substance sodium azide (NaN3) 1 mole 2 moles ammonium nitrate (NH4NO3) 1 mole 2 moles nitroglycerin (C₂H5N309) 1 mole 2 moles particles produced 1.5 3 3 6 7.25 14.5 2 NaN3 (s) → 2 Na (s) + 3 N2 (g) 1 NH4NO3 (s) →1 N20 (g)+ 2 H2O (g) 4 C3H5N309 (1)→ 12 CO2 (g) + 10 H20 (1) +6 N2 (g) + 02 (g)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 113AE: Gold is produced electrochemically from an aqueous solution of Au(CN)2 containing an excess of CN....

See similar textbooks

Similar questions

Carbon dioxide from the atmosphere weathers, or dissolves, limestone (CaCO3) by the reaction CaCO3(s)+CO2(g)+H2O(l)Ca2(aq)+2HCO3(aq) Obtain H for this reaction. See Table 6.2 for the data.
The nitrogen content of organic compounds can be determined by the Dumas method. The compound in question is first reacted by passage over hot CuO(s): CompoundCuO(s)HotN2(g)+CO2(g)+H2O(g) The product gas is then passed through a concentrated solution of KOH to remove the CO2. After passage through the KOH solution, the gas contains N2 and is saturated with water vapor. In a given experiment a 0.253-g sample of a compound produced 31.8 mL N2 saturated with water vapor at 25C and 726 torr. What is the mass percent of nitrogen in the compound? (The vapor pressure of water at 25C is 23.8 torr.)
Gold is produced electrochemically from an aqueous solution of Au(CN)2 containing an excess of CN. Gold metal and oxygen gas are produced at the electrodes. What amount (moles) of O2 will be produced during the production of 1.00 mole of gold?
Without consulting your textbook, list and explain the main postulates of the kinetic molecular theory for gases. How do these postulates help us account for the following bulk properties of a gas: the pressure of the gas and why the pressure of the gas increases with increased temperature; the fact that a gas tills its entire container; and the fact that the volume of a given sample of gas increases as its temperature is increased.
34. For each of the following solutions, the number of moles of solute is given, followed by the total volume of the solution prepared. Calculate the molarity of each solution. a. 0.754 mol KNO; 225 mL b. 0.0105 in of CaCl; 10.2 mL c. 3.15 mol NaCl; 5.00 L d. 0.499 mol NaBr; 100. mL
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Write a balanced equation for the reaction between (a) dihydrogen sulfide and sulfur dioxide gases to form sulfur solid and steam. (b) methane, ammonia, and oxygen gases to form hydrogen cyanide gas and steam. (c) iron(lll) oxide and hydrogen gas to form molten iron and steam. (d) uranium(IV) oxide and hydrogen fluoride gas to form uranium(IV) fluoride and steam. (e) the combustion of ethyl alcohol (C2H5OH) to give carbon dioxide and water.