One mole of oxygen gas is at a pressure of 5.90 atm and a temperature of 22.5°C.
(a) If the gas is heated at constant volume until the pressure
triples, what is the final temperature?
°C
(b) If the gas is heated so that both the pressure and volume are
doubled, what is the final temperature?
°C
A) Given pressure p1=5.90atm, temperature T1=22.5°c=22.5+273=295.5°K
Volume v1= constant, pressure p2=3p1, temperature T2=?, volume v2= v1(since v1 is constant)
Now by ideal gas law
P1×v1/T1=P2×v2/T2
Substituting all the values
P1×v1/T1=3p1×v1/T2
T2=3p1×v1×T1/p1v1
T2=3T1=3×295.5=886.5 °K
T2=886.5–273=613.5°c
B) Given pressure p1=5.90atm , pressure p2=2p1, volume v1
Volume v2=2v1, temperature T1= 22.5°c=22.5+273=295.5°K
Temperature T2=?
Now again by ideal gas law
P1×v1/T1=P2×v2/T2
Substituting all the value
P1×v1/T1=2p1×2v1/T2
T2=4×P1×v1×T1/P1×v1
T2=4T1
T2=4×295.5=1182°K
T2=1182–273=909°c
One mole of oxygen gas is at a pressure of 5.90 atm and a temperature of...
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