For combustion of ethanol C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l), the amount of heat produced as measured in bomb calormeter, is 1364.47 kJ/mol at 25°C. Assuming all gases are behaving ideally, the enthalpy of combustion ΔCH, for ethanol will be : (R = 8.314 kJ/mol)

For the combustion reaction of ethanolCH3CH2OH(l)  +  3 O2(g)  →  2 CO2(g)  +  3 H2O(l)     ΔH  =  - 1368 kJ / mol CH3CH2OHchoose the correct energy profile:

0.3 g of ethane undergoes combustion at 27°C in a bomb calorimeter. The temperature of calorimeter system (including the water) is found to rise by 0.5°C. The heat evolved during combustion of ethane at constant pressure is ________kJ mol–1.(Nearest integer)[Given : The heat capacity of the calorimeter system is 20 kJ K–1, R = 8.3 JK–1 mol–1.Assume ideal gas behaviour. Atomic mass of C and H are 12 and 1 g mol–1 respectively]

Calculate the energy required to heat 101.0mg of ethanol from 17.8°C to 24.0°C. Assume the specific heat capacity of ethanol under these conditions is ·2.44J·g−1K−1 . Round your answer to 2 significant digits.

The molar heat of combustion of compound C is 1,250 kJ mol-1. If I were to burn 0.115moles of this compound in a bomb calorimeter with a reservoir that holds 2.50 dm3ofwater, what would the expected temperature increase be?

Calculate the energy required to heat 0.20kg of ethanol from 4.5°C to 10.0°C. Assume the specific heat capacity of ethanol under these conditions is ·2.44J·g−1K−1 . Be sure your answer has the correct number of significant digits.