A gas bottle contains 0. 350 mol of gas at 0.973 bar pressure. If the final pressure is 1.165 bar, how many moles of gas were added to the bottle?

Question

Quizplus · Accepted Answer

Using the combined gas law, we can calculate the initial volume of the gas in the bottle:

P1V1/T1 = P2V2/T2

V1 = (P2V2*T1)/(P1*T2) = (1.165*V2*273)/(0.973*298) = 1.45V2

Next, we can use the ideal gas law to calculate the initial number of moles of gas in the bottle:

PV = nRT

n = PV/RT = (0.973*1.45V2)/(0.0821*298) = 0.0536V2

Finally, we can subtract the initial number of moles of gas from the final number to find the added amount:

0.350 + added = n2

added = n2 - 0.350 = [(P2*V2)/(RT)] - 0.350 = [(1.165*V2)/(0.0821*273)] - 0.350 = 0.0691 mol.

A Gas Bottle Contains 0