Question

In a constant-pressure calorimeter, 0.961 g of ammonium nitrate is dissolved in 100.0 g of water. The water decreases in temperature from 21.11 to 20.39. Based on this information, and estimating the solution's heat capacity as 4.18 J g-' °C-, what is the amount of heat, in joules, transferred in this reaction?

Answer 1

The amount of heat transferred in this reaction is -314.32 J.

Step-by-step explanation:

To calculate the amount of heat transferred in this reaction, we can use the formula Q = m × Cs × ΔT, where Q is the amount of heat, m is the mass of the solution, Cs is the heat capacity of the solution, and ΔT is the change in temperature.

First, we need to calculate the mass of the solution, which is the sum of the mass of the ammonium nitrate and the mass of the water.

Given that the mass of the ammonium nitrate is 0.961 g and the mass of the water is 100.0 g, the total mass of the solution is 100.961 g.

Next, we can calculate ΔT by subtracting the final temperature (20.39 °C) from the initial temperature (21.11 °C), which gives us a change in temperature of -0.72 °C.

Using the given heat capacity of 4.18 J/g-°C,

we can now calculate the amount of heat transferred:

Q = (100.961 g) × (4.18 J/g-°C) × (-0.72 °C)

= -314.32 J