Question

When 120 mg of naphthalene (C10H8; ΔcH = -5157 kJ mol-1) was burned in a constant...

When 120 mg of naphthalene (C10H8; ΔcH = -5157 kJ mol-1) was burned in a constant volume calorimeter, the temperature rose by 3.05 K. What is the effective heat capacity of the calorimeter? When 10.0 mg of phenol (C6H5OH) was burned in the calorimeter, the temperature increased by 2.05 K. What is the ΔcH for phenol?

Homework Answers

Answer #1

Step1

Knowinhg Delta Hc for Naphthalene (standard) calculate the effective heat capacity of the calorimeter

Step 2

Using this value of effective heat capacity of the calorimeter, calculate Delta Hc for Phenol

---------------------------------------------------------------------------------------------------------------------------------------

Calculatuon of  effective heat capacity of the calorimeter:

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 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 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).
Mothballs are composed primarily of the hydrocarbon naphthalene (C10H8). When 1.025 g of naphthalene is burned...
Mothballs are composed primarily of the hydrocarbon naphthalene (C10H8). When 1.025 g of naphthalene is burned in a bomb calorimeter, the temperature rises from 24.25 ∘C to 32.33 ∘C.Find ΔErxn for the combustion of naphthalene. The heat capacity of the calorimeter, determined in a separate experiment, is 5.11kJ/∘C. Express the change in energy in kilojoules per mole to three significant figure
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?
When 1.799 g of naphtalene (C10H8) is burned in a constant-volume bomb calorimeter at 298 K,...
When 1.799 g of naphtalene (C10H8) is burned in a constant-volume bomb calorimeter at 298 K, 72.31 kJ of heat is evolved. Calculate U and w for the reaction on a molar basis.
0.9410 g of phenol (C6H5OH) are burned in a bomb calorimeter with a heat capacity of...
0.9410 g of phenol (C6H5OH) are burned in a bomb calorimeter with a heat capacity of 4.630 kJ/C . The temperature of the calorimeter increases by 6.590C. What is the heat of combustion (Hrxn for the process of burning) of phenol? a. -30.51 kJ/C b. -267.5 kJ/C c. -3051 kJ/mol d. none of these
Find ΔErxn for the combustion of C10H8 in kJ/mol. The heat capacity of the bomb calorimeter,...
Find ΔErxn for the combustion of C10H8 in kJ/mol. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 4.947 kJ/∘C . When 1.318 g of C10H8 undergoes combustion in a bomb calorimeter, the temperature rises from 26.04 ∘C to 49.29 ∘C.
The heat of combustion of benzoic acid (C6H5COOH) is -3226 kJ/mol. When 0.841 g of benzoic...
The heat of combustion of benzoic acid (C6H5COOH) is -3226 kJ/mol. When 0.841 g of benzoic acid was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose from 23.50 °C to 27.05 °C. What is the heat capacity (calorimeter constant) of the calorimeter? A.6.25 kJ/°C B.22.2 kJ/°C C.79.0 kJ/°C D.0.439 kJ/°C E.908 kJ/°C
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...
A sample of solid azulene (C10H8) that weighs 0.4925 g is burned in an excess of...
A sample of solid azulene (C10H8) that weighs 0.4925 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.150 °C. The heat capacity of the calorimeter and its contents is known to be 9.455×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT