1a) Consider the reaction:
C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l) in which 10.0 g of sucrose,
C12H22O11, was burned in a bomb calorimeter with a heat capacity of
7.50 kJ/∘C. The temperature increase inside the calorimeter was
found to be 22.0 ∘C. What is the heat of this reaction per mole of
sucrose?
1b) One tablespoon of peanut butter has a mass of 17.0 g. It is
combusted in a calorimeter whose heat capacity is 110 kJ/°C. The
temperature of the calorimeter rises from 21.6 ∘C to 25.8 ∘C . What
is the caloric content of peanut butter in Cal/g?
1c)When a 3.50 g sample of liquid octane (C8H18) is burned in a
bomb calorimeter, the temperature of the calorimeter rises by 26.7
∘C. The heat capacity of the calorimeter, measured in a separate
experiment, is 6.10 kJ/∘C . The calorimeter also contains 3.00 kg
of water, specific heat capacity of 4.18 J/g°C. Determine ΔErxn for
the combustion of octane in units of kJ/mol octane.
a) Heat capacity = c = 7.50 kJ/oC
Change in temperature = t = 22.0 oC
Heat generated = ct = 7.50*22.0 = 165 kJ
Mass of sucrose = 10.0 g
Molar mass of sucrose = 342 g/mol
number of moles of sucrose = mass/molar mass = 10.0/342 = 0.029 mol
Heat generated per mole = heat generated/number of moles = 165/0.029 = 5690 kJ/mol
Heat of the reaction per mole of sucrose = 5690 kJ/mol
b) Heat capacity = c = 110 kJ/oC
Change in temperature = t = 25.8-21.6 oC = 4.2 oC
Heat generated = ct = 110*4.2 = 462 kJ
Convert kJ into cal
1 kcal = 4.2 kJ
So, 462 kJ = (462/4.2) kcal = 110.42 kcal
Mass of butter = 17.0 g
caloric content of peanut butter = heat generated/mass = 110.42/17.0 = 6.470 kcal/g = 6495 cal/g
caloric content of peanut butter = 6495 cal/g
c) Heat capacity = c = 6.10 kJ/oC
Change in temperature = t = 26.7 oC
Heat generated = ct = 6.10*26.7 = 162.87 kJ
Mass of octane = 3.50 g
Molar mass of octane = 114 g/mol
number of moles of octane = mass/molar mass = 3.50/114 = 0.0307 mol
Heat generated per mole = heat generated/number of moles = 162.87/0.031 = 5304.9 kJ/mol
Heat of the reaction per mole of octane = 5304.9 kJ/mol
1a) Consider the reaction: C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l) in which 10.0 g of sucrose, C12H22O11, was burned in a...
Consider the reaction C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l) in which 10.0 g of sucrose, C12H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/∘C. The temperature increase inside the calorimeter was found to be 22.0 ∘C. Calculate the change in internal energy, ΔE, for this reaction per mole of sucrose. Express the change in internal energy in kilojoules per mole to three significant figures.
Determine the heat of combustion of sucrose (C12H22O11) in kJ/mol if 2.00g of sucrose is burned in a bomb calorimeter, and the temperature of the calorimeter rose from 25.33C to 28.17C. The heat capacity of the calorimeter is 11.6kJ/C.
One tablespoon of peanut butter has a mass of 16.0 g. When it is combusted in a bomb calorimeter with a heat capacity of 103.3 kJ/ C, submerged in 4.0 L of water. The temperature of the water rises from 22.2 C to 25.4 C. Find the food caloric content of peanut butter in Cal/g. Assume density of water is 1.0 g/mL. The specific heat of water is 4.184 J/gC
1) A calorimeter contains 28.0 mL of water at 11.5 ?C . When 2.20 g of X (a substance with a molar mass of 51.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)?X(aq) and the temperature of the solution increases to 30.0 ?C . Calculate the enthalpy change, ?H, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g??C)], that density of water is...
One tablespoon of peanut butter has a mass of 17 g. It is combusted in a calorimeter whose heat capacity is 110 kJ/degrees C. The temperature of the calorimeter rises from 22.0 degrees C to 25.2 degrees C. Find the food caloric content of peanut butter. Express your answer using two significant figures.
When a 3.08 g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 26.9 oC. The heat capacity of the calorimeter, measured in a separate experiment, is 6.22 kJ/∘C . The calorimeter also contains 3.00 kg of water, specific heat capacity of 4.18 J/g°C. Determine the heat of combustion of octane in units of kJ/mol octane.
Part A: A calorimeter contains 26.0 mL of water at 13.0 ∘C . When 2.10 g of X (a substance with a molar mass of 49.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 25.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water...
Part A A calorimeter contains 34.0 mL of water at 12.5 ∘C . When 1.50 g of X (a substance with a molar mass of 75.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 25.5 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water...
The temperature rises from 25.00°C to 29.00°C in a bomb calorimeter when 3.50 g of sucrose undergoes combustion in a bomb calorimeter. Calculate ΔErxn for the combustion of sucrose in kJ/mol sucrose. The heat capacity of the calorimeter is 4.90 kJ/°C. The molar mass of sugar is 342.3 g/mol
The temperature rises from 25.00°C to 29.00°C in a bomb calorimeter when 3.50 g of sucrose undergoes combustion in a bomb calorimeter. Calculate ΔErxn for the combustion of sucrose in kJ/mol sucrose. The heat capacity of the calorimeter is 4.90 kJ/°C. The molar mass of sugar is 342.3 g/mol