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.
Consider the reaction C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l) in which 10.0 g of sucrose, C12H22O11, was burned in a bomb...
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...
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...
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...
part a. The air in an inflated balloon (defined as the system) is warmed over a toaster and absorbs 110 J of heat. As it expands, it does 79 kJ of work. What is the change in internal energy for the system? Express the energy in kilojoules to two significant figures. part b. When fuel is burned in a cylinder equipped with a piston, the volume expands from 0.235 L to 1.350 L against an external pressure of 1.02 atm...
ReviewI Constants1 Periodic Table Part A A calorimeter is an insulated device in which a chemical reaction is contained By measuring the temperature change. ΔΤ, we can calculate the heat released or absorbed during the reaction using the following equation: A calorimeter contains 35.0 mL of water at 13.5 °C . when 1.20 g of X (a substance with a molar mass of 61.0 g/mol) is added, it dissolves via the reaction X+20)-X(ag) and the temperature of the solution increases...
The combustion of 1.010 g sucrose C12H22O11 in a bomb calorimeter causes the temperature to rise from 24.92 to 28.33 oC. The heat capacity of the calorimeter assembly is 4.90 kJ/ oC. What is the heat of combustion of sucrose in kJ per mole of sucrose?
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.
<P 8 Calorimetry < 7 of 29 > A calonmeter is an insulated device in which a chemical reacton is contained. By measuring the temperature change, A7, we can calculate the heat released or absorbed during the reaction using the following equation: Review Constants Periodic Table A calorimeter contains 18.0 mL of water at 11.5 °C. When 2.30 g of X (a substance with a molar mass of 46.0 g/mol) is added, it dissolves via the reaction X(s) + II,...
A 1.800-g sample of solid phenol (C6H5OH(s)) was burned in a bomb calorimeter, which has a total heat capacity of 11.66 kJ/∘C. The temperature of the calorimeter plus its contents increased from 21.36∘C to 26.37∘C. A. Write a balanced chemical equation for the reaction that takes place in the bomb calorimeter. Express you answer as a chemical equation including phases. B. What is the heat of combustion per gram of phenol? Express the heat in kilojoules per gram to three...