Answer:
The total pressure of the mixture is 2.5 atm.
Explanation:
According to Dalton´s law of partial pressures, the total pressure of the mixture is the sum of the partial pressures of each gas.
From the chemical equation, we know that 1 mol of A reacts with 1 mol of B to produce 1 mol of AB. We have only 0.04 mol of gas A, then, only 0.04 mol of AB will be produced when reacting with 0.04 mol of B. 0.06 mol of B will remain without reacting.
After the reaction, there will be 0.04 mol of AB and 0.06 mol of B.
The pressure of AB can be calculated as follows:
PAB = n*R*T / V
Where:
PAB = partial pressure of gas AB.
n = number of mole of AB.
R = gas constant = 0.082 l atm / K mol
T = temperature
V = volume
Then:
PAB = 0.04 mol * 0.082 (l atm / K mol) * 300 K / 1 l = 0.98 atm.
In the same way, the partial pressure of B can be calculated:
PB = 0.06 mol * 0.082 (l atm / K mol) * 300 K / 1 l = 1.5 atm.
The total pressure (Pt) is then:
Pt = PAB + PB = 0.98 atm + 1.5 atm = <u>2.5 atm</u>
