A chemist carefully measures the amount of heat needed to raise the temperature of a 278.0g sample of C5H12S from 0.8degree celsius to 15.9 degree celsius. The experiment shows that 8.46X10^3J of heat are needed. What can the chemist report for the molar heat capacity of C5H12S? Be sure your answer has the correct number of significant digits.

Question

Jean

Chemistry

28 July, 20:49

A chemist carefully measures the amount of heat needed to raise the temperature of a 278.0g sample of C5H12S from 0.8degree celsius to 15.9 degree celsius. The experiment shows that 8.46X10^3J of heat are needed. What can the chemist report for the molar heat capacity of C5H12S? Be sure your answer has the correct number of significant digits.

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Answers (1)

Know the Answer?

Wolf · Answer 1

The answer to your question is C = 2.01 J/g°C

Explanation:

Data

mass = m = 278 g

Temperature 1 = T1 = 0.8°C

Temperature 2 = T2 = 15.9 °C

Heat = Q = 8.46 x 10³ J

Heat capacity = C = ?

Process

1. - Write the formula to calculate the heat

Q = mC (T2 - T1)

2. - Solve for C

C = Q / m (T2 - T1)

3. - Substitution

C = 8.46 x 10³ / 278 (15.9 - 0.8)

4. - Simplification

C = 8.46 x 10³ / 4197.8

5. - Result

C = 2.01 J/g°C