0.34mol of argon gas is admitted to an evacuated 80cm^3 container at 10 degrees Celsius. The gas then undergoes an isochoric heating to a temperature of 500 degrees Celsius. Whats the final pressure of the gas?
I tried to use PV=nRT and got 2700 kPa but it was incorrect. Please help!
I tried to use PV=nRT and got 2700 kPa but it was incorrect. Please help!
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Volumne Iis kept the same
T/Pbefore =T/P after
P=nRT/V before
V/nR=T/P
nRT/V=P
The new temp and the old volumne which is constant
27300427.5 pascal
27300 Kilopascal
Maybe you converted the cm^3 wrong
80 cm^3 1 m^3/ 100^3 m^3
8x10^5 m^3
T/Pbefore =T/P after
P=nRT/V before
V/nR=T/P
nRT/V=P
The new temp and the old volumne which is constant
27300427.5 pascal
27300 Kilopascal
Maybe you converted the cm^3 wrong
80 cm^3 1 m^3/ 100^3 m^3
8x10^5 m^3
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How exactly did you use PV = nRT? "Isochoric" means "constant volume".
P = nRT/V. Just plug in n, R, T and V in appropriate units. Don't forget T needs to be in Kelvin, not Celsius.
P = nRT/V. Just plug in n, R, T and V in appropriate units. Don't forget T needs to be in Kelvin, not Celsius.
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I think it is 270 atm.
P = nrt/v
.34*.0821*(500+273.15) / .08
269.77
P = nrt/v
.34*.0821*(500+273.15) / .08
269.77