Calculate the change internal energy (δe) for a system that is giving off 65.0 kj of heat and is performing 855 j of work on the surroundings. calculate the change internal energy (δe) for a system that is giving off 65.0 kj of heat and is performing 855 j of work on the surroundings. 9.00 x 102 kj 64.1 kj -9.00 x 102 kj -64.1 kj -65.9 kj

A system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings has a change in the internal energy of -65.9 kJ.

According to the First Law of Thermodynamics, we can calculate the change in the internal energy (ΔE) of the system using the following expression.

A system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings has a change in the internal energy of -65.9 kJ.

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 -64.1 kJ.  

Explanation:

According to first law of thermodynamics:

=Change in internal energy

q = heat absorbed or released

w = work done or by the system

w = work done by the system=  {Work is done by the system is negative as the final volume is greater than initial volume}

w = -855 Joules = 0.855 kJ     (1kJ=1000J)

q = -65.0 kJ  {Heat released by the system is negative}

Thus the change internal energy (ΔE) for a system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings is -64.1 kJ.  

the mass of the cathode increases because ions from the solution get reduced to atoms and become part of the cathode.

explanation:

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c. heat could easily travel through the molecules in the air and escape/enter the flask. removing the air slows down the heat transfer.