Consider the following reaction in a closed reaction flask. If 1.50 atm of gas A
ID: 840979 • Letter: C
Question
Consider the following reaction in a closed reaction flask. If 1.50 atm of gas A is allowed to react with 0.500 atm of gas B and the reaction goes to completion at constant temperature and volume, what is the total pressure in the reaction flask at the end of the reaction? What are the partial pressures of the gases in the flask?
4A(g) + 6B(g) ? 2A2B3(g)
A. (0.750 atm A2B3 produced) + (0.25 atm B remaining) = 1.00 atm total pressure B. (0.167 atm A2B3 produced) + (1.17 atm A remaining) = 1.34 atm total pressure C. (1.50 atm A2B3 produced) + (0.167 atm A remaining) = 1.67 atm total pressure D. (0.333 atm A2B3 produced) + (0.500 atm A remaining) = 0.833 atm total pressureExplanation / Answer
B. (0.167 atm A2B3 produced) + (1.17 atm A remaining) = 1.34 atm total pressure
4 moles A =6 mole B = 2 Mole A2B3
Limiting reagent is B
partial pressure of A = 0.5*4/6 = 0.333333333
A remaiming after reaction = 1.5-0.333333333 = 1.16666667 atm
A2B3 produced = 0.5*2/6 = 0.166666667 atm
Total pressure = 1.1666667 + 0.16667 = 1.34 atm