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GaryK [48]
3 years ago
8

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?
Chemistry
1 answer:
Digiron [165]3 years ago
8 0

Answer:

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

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Answer:

  • The first picture attached is the diagram that accompanies the question.

  • The<u> second picture attached</u> is the diagram with the answer.

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A 0.10MCaCl₂ (aq) solution will have half the number of CaCl₂ units as the number of NaCl units in a 0.20M NaCl (aq) solution.

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Molar mass:-

\\ \tt\longmapsto 14+3(1)=17g/mol

Now

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