What is the pressure in a 10.00 liter container of methane, CH4(molarmass=16.05 g/mol) that contains 4.00 g of the gas at 25.0•c?

Question

A. 0.610atm

B. 0.305atm

C. 1.07atm

D. 10.7 atm

Answer 1

Hi Aliyah,

 

you can use the ideal gas equation PV = nRT
 
where:  P is pressure, V is volume in Liters, T is temperature in Kelvin, n is the number of moles, and R is a constant

 

which depends on the unit for pressure: use 0.0821 atm.L/mol.K if given in atm, or 8.31 kPa.L/mol.K if given kPa, or

 

62.4 mmHg.L/mol.K if given mmHg.

 

Thus to find P, solve the equation

              P = nRT/V

n = 4.00 g/16.05g/mol ( divide the given mass by the molar mass),

 

T = 25.0 + 273 (to covert the temperature to kelvin), V = 10.00 L, and use R =0.0821 atm.L/mol.K.

 

I will let you to complete the calculation.