Question

1a. What happens to the pressure of an ideal gas if you double its temperature in a closed volume? And what happens to the pressure of an ideal gas if you double its volume at a fixed temperature?Please explain your answer using the combine gas law.

1b. Based upon the standard molar volume, what volume would 0.500 moles of an ideal gas occupy at STP? And based upon the standard molar volume, what volume would be occupied by 1.00 mol of an ideal gas at a temperature of 819.45 K and a pressure of 760.0 mmHg?Please explain your answer.

Answer 1

1a. What happens to the pressure of an ideal gas if you double its temperature in a closed volume?

PV=n RT

V1 =CONSTANT	V2= CONSTANT
T1=X	T2=2X
P1 =P	P2 =?

P1 /T1= P2 /T2

P2 = P1 x T2 /T1

= P1 x 2x /x

=pressure doubles.-----------answer

And what happens to the pressure of an ideal gas if you double its volume at a fixed temperature?

V1 =x	V2= 2x
T1= CONSTANT	T2= CONSTANT
P1 =P	P2 =?

P1V1= P2V2

P2= P1V1/ V2

P2= P x / 2x

= pressure halved (P/2) -----------answer

===============

b. Based upon the standard molar volume, what volume would 0.500 moles of an ideal gas occupy at STP?

1mole-------------22.4 litre

0.500 moles------------11.2 litres--------answer

And based upon the standard molar volume,

what volume would be occupied by 1.00 mol of an ideal gas at a temperature of 819.45 K and a pressure of 760.0 mmHg

PV=n RT

V/T= V/T

22.4/273= V/819.45 K

V=819.45 K X 22.4 /273=67.23 LITRES