Question

A 6.55 g sample of aniline (C₆H₅NH₂, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter with a heat capacity of 14.25 kj/°c. if the initial temperature was 32.9°c, use the information below to determine the value of the final temperature of the calorimeter. 4C₆H₅NH₂(l)+35O₂(g)→24CO₂(g)+14H₂O(g)+4NO₂(g)

Answer 1

The calculation of the final temperature of a bomb calorimeter after the combustion of aniline requires the heat of combustion per mole of aniline, which is not provided. Thus, an accurate final temperature cannot be determined from the given information.

Step-by-step explanation:

The question involves calculating the change in temperature of a bomb calorimeter after the combustion of aniline. To determine the final temperature of the calorimeter, we first need to calculate the heat released by the combustion of aniline and then apply it to the heat capacity of the bomb calorimeter.

First, we calculate the number of moles of aniline combusted:

moles = mass / molar mass = 6.55 g / 93.13 g/mol = 0.0703 mol

We need to know the heat released by this amount of aniline; however, this information is not directly given. If we knew the heat of combustion per mole of aniline, we could proceed with the calculation using the following equation:

q = moles × ΔH_comb

Then, we calculate the change in temperature using the heat capacity of the bomb calorimeter:

ΔT = q / C_bomb

If we assume the heat of combustion to be similar to that of benzene or another known standard, like benzoic acid, we could make an estimation. However, without the exact value for the heat of combustion of aniline, an accurate final temperature cannot be determined from the information provided.