What is the entropy change in the environment when 5.0 MJ of energy is transferred thermally from a reservoir at 1000 K to one at 500 K

The entropy change in the environment is 3.62x10²⁶.

Explanation:

The entropy change can be calculated using the following equation:

Where:

Q: is the energy transferred = 5.0 MJ

: is the Boltzmann constant = 1.38x10⁻²³ J/K  

: is the initial temperature = 1000 K

: is the final temperature = 500 K

Hence, the entropy change is:

Therefore, the entropy change in the environment is 3.62x10²⁶.

I hope it helps you!          

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"

1. they vary with a higher number because boiling is way hotter than melting