Question #203977

A sample of helium occupies 535 ml at 988 torr and 25°C. If the sample is transferred to a 1.05 L flask at 25°C, what will be the gas pressure in the flask?

Expert's answer

We know that ideal gas equation is PV = nRT

Where;

T = Temperature = 25.5 oC = 25.5+273 = 298.5 K

P = pressure = 988 mm Hg = 988/760 atm = 1.3 atm

n = No . of moles = ?

R = gas constant = 0.0821 L atm / mol - K

V= Volume of the gas = 535 mL = 0.535 L

Plug the values we get n = (PV) / (RT)

= 0.0284 moles

So the number of moles of He gas is 0.0284 moles

Now we have to calculate the pressure when it is transferred to 1.05 L

We know that ideal gas equation is PV = nRT

Where

T = Temperature = 25.5 oC = 25.5+273 = 298.5 K

P = pressure = ?

n = No . of moles = 0.0284 mol

R = gas constant = 0.0821 L atm / mol - K

V= Volume of the gas = 1.05 L

Plug the values we get P = (nRT) / V

= ( 0.0284x0.0821x298.5) / 1.05

= 0.662 atm

= 0.662x760 mm Hg

since 1atm = 760 mm Hg

= 503.4 mm Hg

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