An endothermic reaction occurs in a cylinder with initial volume of 1 L. 5 kJ of heat is transferred and the internal energy change (∆E) is -5 kJ. The only work occurring the expansion or contraction of the cylinder against an external pressure of 1 atm. What is the final Volume of the cylinder? Can anyone help?

critical Nov 2, 2018

#3**+1 **

Hmmm...I think I am stuck...

if you add 5kj (or subtract) from a volume...it will change ...according to the gas laws...but if it is 6000 degrees it will change less than if it was 200 degrees.....so I think I need an initial temp.......I could be wrong....was STP stated?

ElectricPavlov Nov 3, 2018

#4**+3 **

Solution:

\( \small \text {Translate Joules to Liter-atmospheres}\\ w = -5000J * \dfrac{ 1L * atm} {101.325J} =-49.35L*atm \,| \small \text { Negative (-) means energy entered system.}\\ w = −P*\Delta V\\ \small \text {Change in volume }\\ \Delta V = -\dfrac {w}{P} = -\dfrac {-49.35L*atm }{1 atm}=+ 49.35L \,| \small \text { Positive (+) means gas expanded.}\\ \text { }\,\\ \text {Final Volume of the cylinder } 49.35L\)

GA

GingerAle Nov 4, 2018