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3 years ago

What is the volume, in liters, of 1.40 mol of oxygen gas at 20.0°C and 0.974 atm?

Chemistry

1 answer:

topjm [15]3 years ago

4 0

Answer:

V = 34.55 L

Explanation:

Given that,

No of moles, n = 1.4

Temperature, T = 20°C = 20 + 273 = 293 K

Pressure, P = 0.974 atm

We need to find the volume of the gas. It can be calculated using Ideal gas equation which is :

PV=nRT

R is gas constant, $R=0.08206\ L-atm/mol-K$

Finding for V,

$V=\dfrac{nRT}{P}\\\\V=\dfrac{1.4\times 0.08206\times 293}{0.974 }\\\\V=34.55\ L$

So, the volume of the gas is 34.55 L.

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(b) 2.56 mol.L⁻¹.h⁻¹

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$\frac{\Delta[NO_{2}]}{\Delta t} = 7.11 \cdot 10^{-4} M/s*\frac{3600 s}{1 h} = 2.56 mol.L^{-1}.h{-1}$

Hence, the number of moles of NO₂(g) produced per hour per liter of air is 2.56 mol.L⁻¹.h⁻¹

I hope it helps you!

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