Question

The bomb calorimeter in Exercise 102 is filled with 987g water. The initial temperature of the calorimeter contents is 23.32. A 1.056g sample of benzoic acid is combusted in the calorimeter. What is the final temperature of the calorimeter contents

Answer 1

To find the final temperature of the calorimeter contents, we need to calculate the heat released by the combustion of benzoic acid and use the heat capacity of the calorimeter. Using the given values, we can calculate that the final temperature is approximately 23.313 °C.

Step-by-step explanation:

In order to determine the final temperature of the calorimeter contents, we need to use the heat released by the combustion of benzoic acid and the heat capacity of the calorimeter. From the given information, the mass of benzoic acid is 1.056 g and its enthalpy of combustion is -26.38 kJ/g. The initial temperature of the calorimeter contents is 23.32 °C.

To find the final temperature, we can use the equation:

q = m × C × ΔT

Where:
q is the heat released by the combustion of benzoic acid
m is the mass of benzoic acid
C is the heat capacity of the calorimeter
ΔT is the change in temperature
Let's calculate it:

q = (1.056 g) × (-26.38 kJ/g)
q = -27.86 kJ

Using the equation, we can rearrange it to solve for ΔT:

ΔT = q / (m × C)

ΔT = (-27.86 kJ) / (987 g × 4.18 J/g°C)

ΔT ≈ -0.007 °C

Therefore, the final temperature of the calorimeter contents would be approximately 23.32 °C - 0.007 °C, which is approximately 23.313 °C.

Answer 2

The bomb calorimeter in Exercise 102 is filled with 987g water, the final temperature is 50.45°C.

Step-by-step explanation:

To determine the final temperature of the calorimeter contents, we can use the equation:

q = mCΔT

where

q is the heat gained or lost

m is the mass of the substance

C is the specific heat capacity

ΔT is the change in temperature.

In this case, the heat gained by the water can be calculated using the equation:

q = (mwater)(Cwater)(ΔT)

Substituting the known values, we get:

q = (987g)(4.18 J/g°C)(ΔT)

Similarly, the heat gained by the benzoic acid can be calculated using the equation:

q = (macid)(Cacid)(ΔT)

Substituting the known values, we get:

q = (1.056g)(26.38 kJ/g)(ΔT)

Since the total heat gained by the water and the benzoic acid is zero (assuming no heat is lost to the surroundings), we can set the two equations equal to each other and solve for ΔT:

(987g)(4.18 J/g°C)(ΔT) = (1.056g)(26.38 kJ/g)(ΔT)

Solving for ΔT, we find 50.45°C.

Therefore the final temperature of the calorimeter contents is 50.45°C.