Question

A 8.65-L container holds a mixture of two gases at 11 °C. The partial pressures of gas A and gas B, respectively, are 0.205 atm and 0.658 atm. If 0.200 mol of a third gas is added with no change in volume or temperature, what will the total pressure become?

Answer 1

The total pressure = 1.402 atm

calculation

Total pressure = partial pressure of gas A + partial pressure of gas B + partial pressure of third gas

partial pressure of gas A= 0.205 atm

Partial pressure of gas B =0.658 atm

partial pressure for third gas is calculated using ideal gas equation

that is PV=nRT where,

p(pressure)=? atm

V(volume) = 8.65 L

n(moles)= 0.200 moles

R(gas constant)=0.0821 L.atm/mol.k

T(temperature) = 11°c into kelvin =11+273 =284 k

make p the subject of the formula by diving both side by V

p =nRT/v

p = [(0.200 moles x 0.0821 L.atm/mol.K x 284 K)/8.65L)] =0.539 atm

Total pressure is therefore = 0.205 atm +0.658 atm +0.539 atm

=1.402 atm