Question

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.

Answer 1

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

Step-by-step 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