When a sample of aqueous hydrochloric acid was neutralized with aqueous sodium hydroxide in a calorimeter,the temperature of 100.0 g of water surrounding the reaction increased from 25.0°C to 31.5°C.If the specific heat of water is 1.00 cal/(g•°C),calculate the quantity of energy in calories involved in this neutralization reaction.

Question

Quizplus · Accepted Answer

650 cal.The energy involved in the reaction can be calculated using the formula $q = m \cdot c \cdot \Delta T$, where $q$ is the heat absorbed or released, $m$ is the mass of the water, $c$ is the specific heat capacity of water, and $\Delta T$ is the change in temperature. Here, $m = 100.0 \, \text{g}$, $c = 1.00 \, \text{cal/(g•°C)}$, and $\Delta T = 31.5°C - 25.0°C = 6.5°C$. Thus, $q = 100.0 \, \text{g} \times 1.00 \, \text{cal/(g•°C)} \times 6.5°C = 650 \, \text{cal}$.

When a Sample of Aqueous Hydrochloric Acid Was Neutralized with Aqueous