What is the volume of 0.153 grams of hydrogen gas at 23.0°C and 88.5 kPa?

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Answer 1 · 2016-10-11T00:25:09

Use the universal gas law $PV = nRT$

Answer $V = 2.07 L$

We are given $P = 88.5 kPa$

Convert the given amount to moles:

$0.153 g H_2(1 molH_2)/(2 gH_2) =0.076mol$

Convert the given temperature to Kelvin

$T =23°C + 273°C$

$T = 296°K$

Use the universal gas constant:

$R = 8.134 (L)(kPa)(K^(-1))(mol^(-1))$

The universal gas law:

$PV = nRT$

$V = (nRT)/P$

$V = ((0.076 mol)(8.134 (L)(kPa)(K^(-1))(mol^(-1)))(296°K))/(88.5 kPa)$

$V = 2.07 L$