Question

322 L of hydrogen occupies a volume of 197 L at STP. If the initial temperature of the hydrogen was 37°C, what was the initial pressure?

Answer 1

Answer:

Ideal Gas Law rearranged:

P = nRT / V

Density of Hydrogen gas = 0.000089 g/ml

Mass of Hydrogen gas = Volume x Density = 322000 x 0.000089 = 28.658 g

Moles of Hydrogen gas = Mass / Molecular Mass = 28.658 / 2 = 14.32 moles

Substitute value into the equation:

P = [ (14.32) (0.08206 L atm mol¯1 K¯1) (310 K) ] / 197 L

P = 1.84 atm

P = 1.84 atm x 760.0 mmHg atm¯1 = 1405.34 mmHg

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Explanation:

Answer 2

Initial pressure was determined as 1405.34 mmHg

Explanation:

We know that the Ideal gas equation is PV=nRT

Ideal Gas Law can be rearranged as :

P = nRT / V

Given that, 322 L of hydrogen occupies a volume of 197 L at STP

Density of Hydrogen gas = 0.000089 g/ml

The initial temperature of the hydrogen given  37°C

Mass of Hydrogen gas = Volume x Density = 322000 x 0.000089 = 28.658 g

Moles of Hydrogen gas = Mass / Molecular Mass = 28.658 / 2 = 14.32 moles

we substitute value into the equation:

P = [ (14.32) (0.08206 L atm mol¯1 K¯1) (310 K) ] / 197 L

P = 1.84 atm

P = 1.84 atm x 760.0 mmHg atm¯1 = 1405.34 mmHg

Initial pressure was determied as 1405.34 mmHg

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