Question

1. 3.000 grams of Ca is burned in a bomb calorimeter. The water’s temperature rose from...

1. 3.000 grams of Ca is burned in a bomb calorimeter. The water’s temperature rose from 20.0 degrees centigrade to 21.79 degrees centigrade. The heat capacity of the calorimeter is 26.60 kJ/C. What is the enthalpy change for this reaction as written. The thermochemical equation is:
2Ca (s) + O2 (g) —> 2CaO (s)

2. 1.30 grams of C7H6O2 is combusted in a bomb calorimeter. The water’s temperature rose from 20.00 degrees centigrade to 21.58 degrees centigrade. The heat capacity of the calorimeter is 10.90 kJ/C. What is the enthalpy change for this reaction. The thermochemical reaction is:
2C7H6O2 + 15O2 —> 14CO2 + 6H2O

3. 0.560 grams of C6H6 is burned in a bomb calorimeter. The water rises in temperature from 22.0 degrees centigrade to 29.90 degrees centigrade. The heat capacity of the calorimeter (bomb plus water) is 2.96 kJ/C. What is the enthalpy change for the combustion of one mole of C6H6? The thermochemical equation is:
C6H6 (l) + 15/2O2 —> 6CO2 (g) + 3H2O (l)

Homework Answers

Answer #1

1):

Moles of Ca = Mass of Ca/ atomic mass of Ca = 3.000 g/(40.078 g/mol) = 0.07485 mol

Heat of calorimeter (qcal) = heat capacity of calorimeter x temperature change

                                        = (26.60 kJ/oC) x (21.79 oC - 20.0 oC)

                                        = 47.61 kJ

Enthalpy change of the reaction = - qcal /mol Ca = - 47.61 kJ/0.07485 mol = - 636 kJ/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
When 2.25mg of anthracene was combusted in a constant volume bomb calorimeter, the temperature rose by...
When 2.25mg of anthracene was combusted in a constant volume bomb calorimeter, the temperature rose by 1.35K. Given that the standard molar enthalpy of combustion of anthracene at 298K is -7061 kJ/mol, calculate the heat capacity of the calorimeter.
A 1.000 g sample of octane (C8H18) is burned in a bomb calorimeter containing 1200 grams...
A 1.000 g sample of octane (C8H18) is burned in a bomb calorimeter containing 1200 grams of water at an initial temperature of 25.00ºC. After the reaction, the final temperature of the water is 33.20ºC. The heat capacity of the calorimeter (also known as the “calorimeter constant”) is 837 J/ºC. The specific heat of water is 4.184 J/g ºC. Calculate the heat of combustion of octane in kJ/mol.
A 0.373-g sample of naphthalene (C10H8) is burned in a bomb calorimeter and the temperature increases...
A 0.373-g sample of naphthalene (C10H8) is burned in a bomb calorimeter and the temperature increases from 24.90 °C to 27.80 °C. The calorimeter contains 1.05E3 g of water and the bomb has a heat capacity of 836 J/°C. Based on this experiment, calculate ΔE for the combustion reaction per mole of naphthalene burned (kJ/mol).
A 0.287-g sample of bianthracene (C28H18) is burned in a bomb calorimeter and the temperature increases...
A 0.287-g sample of bianthracene (C28H18) is burned in a bomb calorimeter and the temperature increases from 25.30 °C to 27.50 °C. The calorimeter contains 1.03E3 g of water and the bomb has a heat capacity of 856 J/°C. Based on this experiment, calculate ΔE for the combustion reaction per mole of bianthracene burned (kJ/mol).
A 0.553-g sample of diphenyl phthalate (C20H14O4) is burned in a bomb calorimeter and the temperature...
A 0.553-g sample of diphenyl phthalate (C20H14O4) is burned in a bomb calorimeter and the temperature increases from 24.40 °C to 27.57 °C. The calorimeter contains 1.08×103 g of water and the bomb has a heat capacity of 877 J/°C. The heat capacity of water is 4.184 J g-1°C-1. Based on this experiment, calculate ΔE for the combustion reaction per mole of diphenyl phthalate burned. ______ kJ/mol
. A 0.500 g sample of naphthalene (C10H8) is burned in a bomb calorimeter containing 650...
. A 0.500 g sample of naphthalene (C10H8) is burned in a bomb calorimeter containing 650 grams of water at an initial temperature of 20.00 oC. After the reaction, the final temperature of the water is 26.4ºC. The heat capacity of the calorimeter is 420 J/oC. Using these data, calculate the heat of combustion of naphthalene in kJ/mol.
A 1.000g sample of benzene (C6H6) is burned in a bomb calorimeter whose total heat capacity...
A 1.000g sample of benzene (C6H6) is burned in a bomb calorimeter whose total heat capacity is 4.957 kJ/ oC. If the temperature of the calorimeter increases from 25.30 to 33.74 oC , what is the heat of combustion of the benzene per mole. Explanation please.
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 2.50 mol sample of benzene (C6H6, 78.11 g/mol) was burned in a bomb calorimeter with...
A 2.50 mol sample of benzene (C6H6, 78.11 g/mol) was burned in a bomb calorimeter with a heat capacity of 800 J/°C. The calorimeter contained 100g of water (4.18J/g°C) and the temperature increased by 4°C. What is the molar enthalpy of combustion for this compound?
Sulfur (2.56 g) is burned in a bomb calorimeter with excess O2(g). The temperature increases from...
Sulfur (2.56 g) is burned in a bomb calorimeter with excess O2(g). The temperature increases from 21.25 °C to 26.72 °C. The bomb has a heat capacity of 923 J/K, and the calorimeter contains 815 g of water. Calculate the heat evolved, per mole of SO2 formed, in the course of the reaction: S8(s) + 8 O2(g) --> 8 SO2(g) Answer is in kJ. A. 301.2 B. 3410 C. 296.3 D. 145.1
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT