A 35.6 g sample of ethanol () is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0^oC to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of ? The molar mass of ethanol is 46.07 g/mol.

answer

watching

214

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Brian HingpitLv10

27 Jan 2021

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

A sample of ethanol (C₂H₅OH) was burned completely in a bomb calorimeter whose total heat capacity is 30.75 kJ/^oC. The temperature of the calorimeter plus the contents increased from 25.6^oC to 32.7^oC.

Knowing that ethanol's heat of combustion is -3330 kJ/mol, calculate the mass of the sample (in g).

At constant volume, the heat of combustion of a particular compound is â3936.0 kJ/mol. When 1.107 g of this compound (molar mass = 111.78 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 8.299 Â°C. What is the heat capacity (calorimeter constant) of the calorimeter?