Question

What would the volume of 40g of butane be under a pressure of 1000 Torr and a temperature of 18°C?

Answer 1

From the calculation, the volume of the gas is 12.6 L

What is the pressure of the gas?

We can define the pressure of a gas as the force that the gas exerts per unit area of the container. Now we knw that we can be able to obtain the volume  of the gas by the use of the ideal gas equation.

Now;

Number of moles =  40g/58 g/mol = 0.69 moles

1 mole of butane occupies 22.4 L

0.69 moles of butane occupies  0.69 moles  *  22.4 L/ 1mole

= 15.5 L

Now;

P1 =760 Torr

V1 =  15.5 L

T1 = 273 K

P2 =  1000 Torr

V2 = ?

T2 =  18°C + 273 = 291 K

P1V1/T1 = P2V2/T2

P1V1T2 = P2V2T1

V2 = P1V1T2/P2T1

V2 = 760 Torr * 15.5 L * 291 K/1000 Torr * 273 K

V2 =12.6 L

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