Question

At what temperature (in °C) would one liter of phosphine gas, PH3, have a mass of 1.725 g, if the gas pressure is 0.9910 atm? Assume that the gas behaves ideally.

Answer 1

Answer:  Temperature of one liter of phosphine gas with a mass of 1.725 g and gas pressure of 0.9910 atm is $-36^0C$

Explanation:

According to the ideal gas equation:

PV=nRT

P = Pressure of the gas = 0.9910 atm

V= Volume of the gas= 1.0 L

T= Temperature of the gas in kelvin = ?

R= Gas constant =$0.0821Latm/Kmol$

n=  moles of gas= $\frac{\text {given mass}}{\text {molar mass}}=\frac{1.725g}{34g/mol}=0.051ol$

$0.9910atm\times 1.0=0.051\times 0.0821\times T$

$T=236.7K=(236.7-273)^0C=-36.3^0C$

Thus the temperature (in °C) of one liter of phosphine gas with a mass of 1.725 g and gas pressure of 0.9910 atm is $-36.3^0C$