Question

What is the molar heat of combustion of methanol, CH3OH, if combustion of 1.00g of methanol...

What is the molar heat of combustion of methanol, CH3OH, if combustion of 1.00g of methanol causes a temperature of 3.68 degrees Celsius in a bomb calorimeter that has a heat capacity of 6.43kJ/degrees Celsius?

Homework Answers

Answer #1

if 1g of methanol causes a 3.68 degree change, then find molar mass of methanol. 1 mole methanol = 32.05g, so 32.05 times as much energy will be released by a mole and the temp will change 32.05 times as much. 32.05 x 3.68 = 117.944 degree C change per mole of methanol.

If it takes 6.43 Kj to raise it one degree C, and the temp rose 117.944 degrees C, just multiply 6.43 by 117.944. The answer is 758.37992 Kj, and since it is exothermic and 3 sig figs, the answer is
-758Kj/mol

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A 3.250g sample of methanol, CH3OH, is combusted un a bomb calorimeter. The temperature of the...
A 3.250g sample of methanol, CH3OH, is combusted un a bomb calorimeter. The temperature of the calorimeter increases by 12.55 degrees celsius. If the heat capacity of the bomb is 850.0 J/degrees celsius and it contains 1.200kg of water, what is the heat envolved per mole of ethanol combusted? The specific heat capaacity of water is 4.184 J/g degrees celsius and the molar mass of methanol is 32.04g/mol.
A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently,...
A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature rose by 5.56°C. If the heat capacity of the bomb plus water was 8.09 kJ / °C, calculate the molar heat of combustion of methanol.
A 1.00g sample of the rocket fuel hydrazine N2H4 is burned in a bomb calorimeter containing...
A 1.00g sample of the rocket fuel hydrazine N2H4 is burned in a bomb calorimeter containing 12.00g of water. The temperature of the water and bomb calorimeter rises from 24.62 degrees Celsius to 28.16 degrees Celsius. Assuming the heat capacity of the empty bomb calorimeter is 837J/degrees Celsius, calculate the heat of combustion of 1 mol of hydrazine in the bomb calorimeter. (The specific heat capacity of water is 4.184 J/g*degree Celsius .
Under constant-volume conditions the heat of combustion of benzoic acid (HC7H5O2) is 26.38 kJ/g. A 1.670...
Under constant-volume conditions the heat of combustion of benzoic acid (HC7H5O2) is 26.38 kJ/g. A 1.670 g sample of benzoic acid is burned in a bomb calorimeter. The temperature of the calorimeter increases from 22.45 degrees Celsius to 27.60 degrees Celsius. A) what is the total heat capacity of the calorimeter? B) 1.390 g sample of new sample organic substance is combusted in the same calorimeter. The temperature of the calorimeter increases from 22.14 degrees Celsius to 26.82 degrees Celsius....
The molar heat of combustion of liquid ethyl alcohol is -1336.91 kcal/mole. If 300 mg of...
The molar heat of combustion of liquid ethyl alcohol is -1336.91 kcal/mole. If 300 mg of ethyl alcohol is burned in a calorimeter causes a rise in temperature of 2.225oC. What is the total heat capacity of the calorimeter?
At constant volume, the heat of combustion of a particular compound is –3146.0 kJ/mol. When 1.159...
At constant volume, the heat of combustion of a particular compound is –3146.0 kJ/mol. When 1.159 g of this compound (molar mass = 157.13 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.565 °C. What is the heat capacity (calorimeter constant) of the calorimeter?
a 25.0g piece of aluminum (molar heat capacity of 24.03 J/g degrees Celsius) is heated to...
a 25.0g piece of aluminum (molar heat capacity of 24.03 J/g degrees Celsius) is heated to 82.4 degrees Celsius and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g degrees Celsius) initially at 22.3 degrees Celsius. The final temperature of the water is 24.98 degrees Celsius. Calculate the mass of water in the calorimeter.
An electrical heater is used to add 18.25 kJ of heat to a constant-volume calorimeter. The...
An electrical heater is used to add 18.25 kJ of heat to a constant-volume calorimeter. The temperature of the calorimeter increases by 3.12°C. When 1.75 g of methanol (CH3OH) is burned in the same calorimeter, the temperature increases by 6.78°C. Calculate the molar heat of combustion for methanol (enter in kJ).
1. At constant volume, the heat of combustion of a particular compound, compound A, is –3409.0...
1. At constant volume, the heat of combustion of a particular compound, compound A, is –3409.0 kJ/mol. When 1.277 g of compound A (molar mass = 117.77 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.891 °C. Using this data, what is the heat capacity (calorimeter constant) of the calorimeter? 2. Suppose a 3.107 g sample of a second compound, compound B, was combusted in the same calorimeter, and the temperature...
1. When 1.550 g of liquid hexane (C6H14) undergoes combustion in a bomb calorimeter, the temperature...
1. When 1.550 g of liquid hexane (C6H14) undergoes combustion in a bomb calorimeter, the temperature rises from 25.87∘C to 38.13∘C. Find ΔErxn for the reaction in kJ/mol hexane. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.73 kJ/∘C. Express your answer in kilojoules per mole to three significant figures. 2. The combustion of toluene has a ΔErxn of –3.91×103 kJ/mol. When 1.55 g of toluene (C7H8) undergoes combustion in a bomb calorimeter, the temperature...