An unknown compound (A) is decomposed according to the reaction given below. One of the gas identities is also unknown and represented as Y. The gases are collected over water at 290K. The final volume of the gas sample is 1565mL and the pressure is 765torr. At 290K the vapor pressure of water is 14.53torr. 2A(l) + O2 (g) → 4Y(g) + O2 (g) + 3H2(g) a. Calculate the total number of moles of gas that were produced in the reaction. b. Calculate the partial pressures of each of the gases, in atm. c. The density of the gas sample (without the water included) is 3.16 g/L. What is the molar mass, in g/mol, of the unknown gas, Y? d. How many moles of A were consumed in the reaction?
An unknown compound (A) is decomposed according to the reaction given below. One of the gas identities is also unknown and represented as Y. The gases are collected over water at 290K. The final volume of the gas sample is 1565mL and the pressure is 765torr. At 290K the vapor pressure of water is 14.53torr. 2A(l) + O2 (g) → 4Y(g) + O2 (g) + 3H2(g) a. Calculate the total number of moles of gas that were produced in the reaction. b. Calculate the partial pressures of each of the gases, in atm. c. The density of the gas sample (without the water included) is 3.16 g/L. What is the molar mass, in g/mol, of the unknown gas, Y? d. How many moles of A were consumed in the reaction?
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...
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An unknown compound (A) is decomposed according to the reaction given below. One of the gas identities is also unknown and represented as Y. The gases are collected over water at 290K. The final volume of the gas sample is 1565mL and the pressure is 765torr. At 290K the vapor pressure of water is 14.53torr. 2A(l) + O2 (g) → 4Y(g) + O2 (g) + 3H2(g)
a. Calculate the total number of moles of gas that were produced in the reaction.
b. Calculate the partial pressures of each of the gases, in atm.
c. The density of the gas sample (without the water included) is 3.16 g/L. What is the molar mass, in g/mol, of the unknown gas, Y?
d. How many moles of A were consumed in the reaction?
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