A mixture of CO(g) and O2(g) in a 1.00-L container is heated to 1010 K, where it

Question

A mixture of CO(g) and O2(g) in a 1.00-L container is heated to 1010 K, where it reaches a
total pressure of 2.20 atm. The temperature is held constant at 1010 K, and the pressure begins to
fall slowly because some of the CO and O2 react to form CO2(g). Find the mass of CO2 present in
the container when the total pressure has fallen to 1.95 atm. (HINT: Think about why the
pressure is falling, realizing that T and V are both constant. Then try to relate the change in
pressure to the amount of CO2 that has formed. Keep in mind that there is a chemical reaction
taking place.)

Explanation / Answer

Supposing the reaction did not begin until the temperature reached 1010K.
2 CO + O2 ? 2 CO2
Notice that 3 moles of reactants produce 2 moles of product.
So rhe formation of 2 moles of CO2 results in the net loss of 1 mole of gases in total.

(2.20 atm - 1.95 atm) = 0.25 atm net loss = 0.50 atm CO2 produced

n = PV / RT = (0.50 atm) x (1.00 L) / ((0.08205746 L?atm/K?mol) x (1010 K)) =
0.00603 mol CO2

(0.00603 mol CO2) x (44.00964 g CO2/mol) = 0.265 g CO2

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