Consider the following reaction in a closed reaction flask. If 1.50 atm of gas A
ID: 794842 • 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. (0.333 atm A2B3 produced) + (0.500 atm A remaining) = 0.833 atm total pressure B. (1.50 atm A2B3 produced) + (0.167 atm A remaining) = 1.67 atm total pressure C. (0.750 atm A2B3 produced) + (0.25 atm B remaining) = 1.00 atm total pressure D. (0.167 atm A2B3 produced) + (1.17 atm A remaining) = 1.34 atm total pressureExplanation / Answer
6 B reacts with 4 A to give 2A2B3
hence 1 B reacts with ( 4/6 = 2/3) A to give ( 2/6 = 1/3) A2B3
hence 0.5 atm B react with ( 2/3) x 0.5 = 0.333 atm A to give ( 1/3) x 0.5 = 0.167 A2B3
hence A left = 1.5-0.333 = 1.17 atm
total pressure = sum of partial presurres = 1.17+0.167 = 3.34
hence option D is right answer