Consider the following reaction in a closed reaction flask. If 1.00 atm of gas A
ID: 794821 • Letter: C
Question
Consider the following reaction in a closed reaction flask. If 1.00 atm of gas A is allowed to react with 1.00 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?
6A(g) + 2B(g) ? 2A3B(g)
A. (1.00 atm of A3B produced) + (0.333 atm of A remaining) = 1.33 atm total pressure B. (0.667 atm of A3B produced) + (0.333 atm of B remaining) = 1.00 atm total pressure C. (0.333 atm of A3B produced) + (0.167 atm of A remaining) = 0.500 atm total pressure D. (0.333 atm of A3B produced) + (0.667 atm of B remaining) = 1.00 atm total pressureExplanation / Answer
Since temperature and volume are kept constant, pressure is directly proportional to the number of moles of the gas.
Initially, since both the gases have same partial pressures, we assume both of them have equal number of moles present. (say 1 mole each for that matter)
Since the reaction goes to completion, A would be totally consumed up.
6A + 2B ------> 2A3B
For each 1 mole of B used, 3 moles of A are used.
So, if one mole of A is consumed, 1/3 = 0.333 moles of B are consumed and 0.333 moles of A3B are formed
Thus, 0.667 moles of B remain which is equivalent to 0.667 atm pressure
And 0.333 moles of A3B formed which is same as 0.333 atm pressure
Thus, Option (D) is the correct choice.
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