Question

A system does 1.80×10^{8}J of work while 7.50×10^{8}J of heat transfer occurs to the environment. What is the change in internal energy of the system assuming no other changes (such as in temperature or by the addition of fuel)? (answer in ×10^{8}J)

Answer 1

Answer:

ΔU = -9.30  x 10⁸ J

Explanation:

given,                                                

Work done of the system (W)= 1.8 x 10⁸ J

heat transfer to the environment (ΔQ)= 7.50 × 10⁸ J

Using first law of thermodynamics

ΔQ = ΔU + ΔW                                          

In the case heat is given to the system  so the heat transfer is negative.

-7.50 × 10⁸ = ΔU + 1.8 x 10⁸                

ΔU = -7.50 × 10⁸ - 1.8 x 10⁸              

ΔU = -9.30  x 10⁸ J                                  

Hence, the change in internal energy is equal to -9.30 x 10⁸ J