A chemical reaction was run in 210.0 mL of H2O. During the reaction, the temperature of the H2O changes from 27.2 oC to 57.6 oC. How much heat (in kJ) did the chemical reaction produce? For H2O, Cp = 4.184 J / (g · oC). Assume the mass of the solution is 210.0 g. Enter your answer as a positive decimal number.

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Chemistry

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6 August, 04:14

A chemical reaction was run in 210.0 mL of H2O. During the reaction, the temperature of the H2O changes from 27.2 oC to 57.6 oC. How much heat (in kJ) did the chemical reaction produce? For H2O, Cp = 4.184 J / (g · oC). Assume the mass of the solution is 210.0 g. Enter your answer as a positive decimal number.

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Answers (1)

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Kaylyn Boyer · Answer 1

Answer: The quantity of heat produced by the reaction is + 26710.656J

Explanation:

Quantity of Heat, Q = mass * specific heat capacity * temperature change

Q = mCpTc, where m = mass, Cp = specific heat capacity, Tc is temperature change

m = 210.0g, Cp=4.184J / (g · oC), Tc = 57.6 - 27.2 = 30.4 oC

Q = 210.0g * 4.184J / (g · oC) * 30.4 oC

Q = + 26710.656J

Therefore, the quantity of heat produced by the reaction is + 26710.656J.

Note: Even though heat is given out by the system and is normally written as a negative value to indicate that heat is lost, the answer is written as a positive decimal number according to instruction.