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#