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 significant digits.
C. What is the enthalpy per mole of phenol?
Express the enthalpy in kilojoules per mole to three significant digits.
A.
C6H5OH(s) + 7O2(g) -----------------> 6CO2(g) + 3H2O(l)
B. Total heat capacity of 11.66 kJ/∘C
T = T2-T1
= 26.37-21.36 = 5.010C
The heat of combustion = Total heat capacity * T
= 11.66KJ/0C*5.010C = 58.4166KJ
the heat of combustion per gram of phenol = 58.4166KJ/1.8g = 32.5KJ/g
C.
no of moles of C6H5OH = W/G.M.Wt
= 1.8/94.11 = 0.01913moles
the enthalpy per mole of phenol = 58.4166/0.01913 = -3054 = -3.05*10^3 KJ/mole
A 1.800-g sample of solid phenol (C6H5OH(s)) was burned in a bomb calorimeter, which has a...
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 1.Write a balanced chemical equation for the reaction that takes place in the bomb calorimeter.(Identify all phases) 2.What is the heat of combustion per gram of phenol? 3.What is the enthalpy per mole of phenol?
A 2.300 −g sample of quinone (C6H4O2) is burned in a bomb calorimeter whose total heat capacity is 7.854kJ/∘C. The temperature of the calorimeter increases from 23.84 ∘C to 31.29 ∘C Part A What is the heat of combustion per gram of quinone? Part B What is the heat of combustion per mole of quinone?
3. A 2.200 g sample of quinone (CH,02) is burned in a bomb calorimeter whose total heat capacity is 7.854 kJ/°C. The temperature of the calorimeter increases from 23.44 to 30.57°C. a. What quantity of heat was produced by the combustion of the quinone? b. What is the heat of combustion per gram of quinone? c. What is the heat of combustion per mole of quinone?
When 0.187 g of benzene, C6H6, is burned in a bomb calorimeter, the temperature of both the water and the calorimeter rises by 4.53 ∘C. Assuming that the bath contains 250.0 g of water and that the heat capacity for the calorimeter is 525 J/∘C , calculate the combustion energy (ΔE) for benzene in kilojoules per gram.
When 0.187 g of toluene, C7H8, is burned in a bomb calorimeter, the temperature of both the water and the calorimeter rises by 4.83 ∘C. Assuming that the bath contains 250.0 g of water and that the heat capacity for the calorimeter is 525 J/∘C, calculate the combustion energy (ΔE) for toluene in kilojoules per gram.
A 0.1785 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity of the calorimeter plus water was 5,760 J/C. If the temperature rise of the calorimeter with water was 1.25*C, calculate the enthalpy of combustion(in kJ/mol) of magnesium. Mg(s) + 1/2O2(g) -> MgO(s) Write answer to three significant figures. Numeric Response
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.
. (15. A 1.600g sample of quinone (C6H,02) was burned in a bomb calorimeter whose total heat capacity is 7.854 kJ/°C. The temperature of the calorimeter increases from 21.34 °C to 32.57 °C. What is the heat of combustion per gram of quinone? Per mole of quinone? (10 pts.)
When 0.605 g of biphenyl (C12H10) undergoes combustion in a bomb calorimeter, the temperature rises from 26.8 ∘C to 29.6 ∘C. Part A Find ΔErxn for the combustion of biphenyl. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.86 kJ/∘C. Express the energy in kilojoules per mole to three significant figures.
A 1.20-g sample of maleic acid (C4H4O4) is burned in a bomb calorimeter and the temperature increases from 24.70 °C to 27.41 °C. The calorimeter contains 1000 g of water and the bomb has a heat capacity of 839 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 maleic acid burned.