The heat of combusion of a substance is defined as the enthalpy change that occurs when 1 mole of a substance reacts with elemental oxygen to form liquid water and gaseous CO2. Determine the heat available from the combustion of methane, CH419) at 25°C and a constant pressure. Express the answer in terms of kcal/mole and kcal/g.

Number 1A food product containing 82% moisture content is being frozen. Estimate the specific heat of the product at -8°C when 82% of the water is frozen. The specific heat of the dry product is 2,5 kJ/(kg°C). It is assumed that the specific heat of water at -10°C is the same as the specific heat of water at 0°C, and that the specific heat of ice follows the function Cp es = 0.0062 Tbeku + 2.0649. identify :a. Cp frozen product = Answer in kJ/kg°C

The heat capacities for each of the substances involved for a particular reaction are given below. The enthalpy change for the same reaction at 298 Kelvin is -282.987 KJ/mole. From these, answer the questions that follow. Temperature-Dependence of the heat capacities of the Substances for the given reaction + (1/2)02(9) → CO2(9) For the gaseous reaction; CO the heat capacities are: Cp°co P(g) 26.86 + 6.97 x10-3 T - 8.20 x10-7 T2 %3D Cp°o2 25.72 + 12.98 x10-3 T - 38.60 x10-7 T² %3D Cp°co2 26.00 + 43.50 x10-3 T 148.32 x10-7 T² %3D What would be the overall enthalpy change at 1,000 Kelvin (AH @ 1000K, in KJ)?

Ethanol has a heat of fusion, AHfus of 4.90 kJ/mol. Calculate the entropy change of the surroundings, ASgurr, when ethanol freezes at -125°c. Report your answer in units of J/(mol·K), to one decimal place. If your answer has a negative sign, be sure to include the negative sign.