Question

The combustion of 1.835 g of carbon disulfide, CS2(l), in a bomb calorimeter with a heat capacity of 4.00 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.04 °C to 33.7 °C. What is the internal energy change, ΔU, for the combustion of 1.835 g of carbon disulfide? ΔU = kJ. Calculate the enthalpy of combustion, ΔHc, for the combustion of carbon disulfide in kilojoules per mole. ΔHc =

Name: the combustion of 1835 g of carbon disulfide cs2l in a bomb calorimeter with a heat capacity of 400 kjc results in an increase in the temperature of the calorimeter and its contents from 220 23025
Uploaded: 2022-06-06T14:59:11-08:00
Duration: 4 min 2 s
Channel: Madhur L
Description: the combustion of 1835 g of carbon disulfide cs2l in a bomb calorimeter with a heat capacity of 400 kjc results in an increase in the temperature of the calorimeter and its contents from 220 23025

          The combustion of 1.835 g of carbon disulfide, CS2(l), in a bomb calorimeter with a heat capacity of 4.00 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.04 °C to 33.7 °C. What is the internal energy change, ΔU, for the combustion of 1.835 g of carbon disulfide? ΔU = kJ. Calculate the enthalpy of combustion, ΔHc, for the combustion of carbon disulfide in kilojoules per mole. ΔHc =

Added by Vincent V.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

06/06/2022

Step 1

\[ \Delta T = T_{\text{final}} - T_{\text{initial}} = 33.7 \, ^\circ\text{C} - 22.04 \, ^\circ\text{C} = 11.66 \, ^\circ\text{C} \] Show more…

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The combustion of 1.835 g of carbon disulfide, CS2(l), in a bomb calorimeter with a heat capacity of 4.00 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.04 °C to 33.7 °C. What is the internal energy change, ΔU, for the combustion of 1.835 g of carbon disulfide? ΔU = kJ. Calculate the enthalpy of combustion, ΔHc, for the combustion of carbon disulfide in kilojoules per mole. ΔHc =