Question

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 to 30.0 Calculate the enthalpy change, 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-specific heat x mass x ΔΤ Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures. At constant pressure, the enthalpy change for the reaction, Δ ll, is equal to the heat, 9pi that is View Available Hint(s) but it is usualy expressed per mole of reactant and with a sign opposite to that of g for the surroundings. The total internal energy change, ΔΕ (sometimes referred to as Δυ)-is the sum of heat and work done, u kJ/mol Submit However, at constant volume (as with a bomb calorimeter) w- and so AE - Part B Consider the reaction C11 DD(s) + 1202(g) 12CO2(g) + 11H20(1) in which 10.0 g of sucrose, Ci 21was burned in a bomb calorimeter with a heat capacity of 7.50 kJ found to be 22.0 oc calculate the change in internal energy. дЕ for this reaction per mole of sucrose. The temperature increase inside the calorimeter was Express the change in internal energy in kilojoules per mole to three significant figures. View Available Hint(s) kJ/mol

Answer 1

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