A sample of NaOH(s) was added to water in a calorimeter. The temperature was monitored as the NaOH dissolved to give the data below. Determine the heat released during the solution process. (Assume the solution specific heat is 4⋅18J⋅g−1⋅K−1Mass of water100.00 gMass of NaOH(s)10.00 gInitial Temperature of water24.0° CFinal Temperature of solution48.2° C

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Q.

A sample of $NaOH (s)$ was added to water in a calorimeter. The temperature was monitored as the $NaOH$ dissolved to give the data below. Determine the heat released during the solution process. (Assume the solution specific heat is $4 \cdot 18 J \cdot g^{- 1} \cdot K^{- 1})$

Mass of water	100.00 g
Mass of NaOH(s)	10.00 g
Initial Temperature of water	24.0° C
Final Temperature of solution	48.2° C

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a

$1.01 \times 10^{4} Joules$

b

$1.11 \times 10^{4} Joules$

c

$1.01 \times 10^{3} Joules$

d

$2.66 \times 10^{3} Joules$

answer is D.

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Detailed Solution

Heat obtained in the process,

$110 \times 4.18 \times (48.2 - 24.0) = 1.11 \times 10^{4} J$

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A sample of NaOH(s) was added to water in a calorimeter. The temperature was monitored as the NaOH dissolved to give the data below. Determine the heat released during the solution process. (Assume the solution specific heat is 4⋅18J⋅g−1⋅K−1Mass of water100.00 gMass of NaOH(s)10.00 gInitial Temperature of water24.0° CFinal Temperature of solution48.2° C