The volume of a gas is 27.5 ml at 22*C and 0.974 atm. What will be the volume if the temperature decreases to 15*C and the pressure increases to 0.993 atm?

26.33mL

Explanation:

In solving this question, we apply the general gas equation

(P1*V1) / T1 = (P2*V2) / T2

P1 = initial pressure of the gas=0.974atm

V1 = intial volume the gas occupies = 27.5mL

T1=initial temperature of the gas = 22°C = 22+273K=295K

P2 = Final pressure of the gas = 0.993atm

V2 = final volume of the gas = ?

T2 = final temperature of the gas = 15°C = 15+273=288K

From (P1*V1) / T1 = (P2*V2) / T2, we make V2 subject of formula

V2 = (P1*V1*T2) / (P2*T2)

We substitute the given values

V2 = (0.974*27.5*288) / (0.993*295)

V2=7714.08/292.935

V2=26.33mL