The pressure in the container is 761.4 mmHg and the temperature is 36.6C and the volume reads a total of 25.2(cm^3). The temperature rises to 65.6 C and the pressure changes to 9.07 atm. Convert pressure to mmHg and determine the new volume?

1 Answer
anor277
May 12, 2018

You do not use #mm*Hg# for pressures OVER #1*atm#..

Explanation:

We know that #1*atm-=760*mm*Hg#... i.e. one atmosphere will support a column of mercury that is #760*mm*Hg# high. And so we can use a mercury column to measure pressures at about #1*atm# or BELOW this pressure...

For a given quantity of gas we use the combined Gas Law...

#(P_1V_1)/T_1-=(P_2V_2)/T_2#....temperature is quoted on the #"absolute scale..."#

We want #V_2=(P_1V_1)/T_1xxT_2/P_2=#

#((761.4*mm*Hg)/(760*mm*Hg*atm^-1)xx25.2*cm^3xx338.75*K)/(309.75*Kxx9.07*atm)=??*cm^3#

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