Define 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 as well as the reaction goes to completion at constant temperature and volume, explain what is the total pressure in the reaction flask at the end of the reaction? Define what are the partial pressures of the gases in the flask?
6A(g) + 2B(g) ? 2A3B(g)
A. 0.500 atm of A3B is produced and since no other gases remain, 0.500 atm is the total pressure
B. (0.500 atm of A3B produced) + (0.500 atm of A remaining) = 1.00 atm total pressure
C. (0.500 atm of A3B produced) + (1.00 atm of A remaining) = 1.50 atm total pressure
D. (0.250 atm of A3B produced) + (0.500 atm of A remaining) = 0.750 atm total pressure