Question

2 attempts left Check my work At 82.7°C and 799 torr, calculate the number of moles and mass of 4.42 L of CH, gas. mol

Answer 1

Temperature(T) = 82.7 ^oC + 273.15 = 355.85 ^oC

Pressure(P) = 799 Torr x ( 1 atm/760 Torr) = 1.05 atm

Volume(V) of methane gas = 4.42 L

The ideal gas law equation is as follows:

PV = nRT

Here, Pressure is P, Volume is V, Number of moles is n, Gas constant is R, and Temperature is T.

The value of Gas constant(R) is 0.08206 L.atm/mol.K

Rearrange the formula for number of moles(n) as follows:

n = PV/RT

Substitute the known values in the rearranged formula and determine the value of n as follows:

n = (1.05 atm x 4.42 L)/(0.08206 L.atm/mol.K x 355.85 ^oC)

n = 0.159 mol CH₄

Use the moles of CH₄ and the molar mass of CH₄ to determine the mass of methane as follows:

The molar mass of methane(CH₄) = 16.04 g/mol

=0.159 mol CH₄ x ( 16.04 g CH₄ / 1 mol CH₄)

= 2.55 g CH₄