What is the final temperature of a 93.9 g block of copper (whose specific heat is .385 J/g0C) that starts at a temperature of 45.0 degrees Celsius and absorbs 1,450.3 J of energy?

7.01 hope this is right !

Explanation:

This problem can be summarized thusly:

qlost by copper = qgained by water + qgained by calorimeter

2) Therefore:

(610. g) (95.3 °C − x) (0.387 J g¯1 K¯1) = (45.0 g) (x − 36.5 °C) (4.184 J g¯1 °C¯1) + [(10.0 J/K) (x − 36.5 °C)]

Comment: The K and the °C cancel because the °C in this problem is a temperature difference (not one single specific value) and the "size" of one K = one °C.

22497.471 − 236.07x = 198.28x − 7237.22

424.35x = 29734.691

x = 70.1 °C

- decrease the number of plants and animals living in the water.