A 0.772 gram sample of hydrogen gas has a volume of 856 milliliters at a pressure of 2.79 atm. The temperature of the H2 gas sample is °C.
Molar mass of H2 = 2.016 g/mol
mass(H2)= 0.772 g
use:
number of mol of H2,
n = mass of H2/molar mass of H2
=(0.772 g)/(2.016 g/mol)
= 0.3829 mol
Given:
P = 2.79 atm
V = 856.0 mL
= (856.0/1000) L
= 0.856 L
n = 0.3829 mol
use:
P * V = n*R*T
2.79 atm * 0.856 L = 0.3829 mol* 0.08206 atm.L/mol.K * T
T = 76.0 K
= (76 - 273) oC
= -197 oC
Answer: -197 oC
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