Question

A reaction between liquid reactants takes place at 30.0 °C in a sealed, evacuated vessel with a measured volume of 20.0 L. Measurements show that the reaction produced 17. g of carbon monoxide gas. Calculate the pressure of carbon monoxide gas in the reaction vessel after the reaction.

Answer 1

Answer:

The correct answer is 0.75 atm

Explanation:

We have carbon monoxide gas (CO) at the following conditions:

T= 30ºC = 303 K

V= 20.0 L

m = 17 g

The molecular weight of CO (MM CO) is the following:

MM CO= molar mass of C + molar mass of O = 12 g/mol + 16 g/mol = 28 g/mol

We calculate the number of moles (n) as follows:

n= m/MM CO = 17 g/28 g/mol = 0.61 mol

Finally we use the ideal gases equation to calculate the pressure (P):

P x V = n x R x T

P = (n x R x T)/V

P= (0.61 mol x 0.082 L.atm/K.mol x 303 K)/20.0 L

P= 0.75 atm

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