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A balloon containing 0.500 mol Ar at 0.00°C and 65.0 kPa pressure is expanded by adding more argon. How many moles of argon are added to bring the sample to a final volume of 60.0 L at 30.0°C and 45.0 kPa?

What is the original volume of the gas?
______K

Respuesta :

Edufirst
Use the ideal gas equation.

PV = nRT

1) Volume of the original gas

V = nRT/P = [0.5mol * 0.082 atm-l/mol-K * 273.15K] / 0.6415 atm] = 17.45 l

2) # of mols to bring to the new state

n = PV/RT = [0.444 atm * 60 l] / [0.082 atm-l/k-mol *303.15k] = 1.07 mol

Then, 1.07 mol - 0.5mol = 0.57 mol were added.
leahk0876

1. What is the original volume of the gas?

17.5 L

2. How many moles of argon exist in the new conditions?

1.07 mol

3. How many moles of argon were added?

0.570 mol

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