Question

(7 pts.) Calculate the heat absorbed when 4.20 g of H2 are produced according to the following equation. CH3OH (g) → CO(g) + 2 H2(g) AH = 90.2 kJ (7 pts.) When one adds 1.475 kJ of heat energy to a sample of gold, the temperature goes from 12.5 °C to 84.6 °C. Calculate the mass of the sample of gold. Gold has a specific heat capacity of 0.129 J/g.°C. (6 pts.) 10. Write the thermochemical equation for the standard enthalpy of formation of solid a NILCI given that the reaction releases 314 kilojoules per mole of ammonium chloride (10 pts.) 11. In a coffee-cup calorimeter, 3.88 g of NH.NO, is mixed 23.00 °C. After the dissolving of the salt, the final enthalpy change for the dissolution of NH.NO, ink assume that the heat capacity of the calorimeter is zero and the solu erimeter. 3.88 g of NHINO, is mixed with 60.0 g of H2O at an initial temperature of dissolving of the salt, the final temperature of the solution is 18.40 °C. Calculate the dissolution of NHINO, in kJ/mol. Assume that the masses are additive. Also, alorimeter is zero and the solution has a specific heat of 4.18 J/g °C. NH.NO: (s) 13% NH.NO, (aq)

Answer 1

® CH3 04 (g) → cough+ 2H2(g) Oro go.2 kJ moled or ha mass -- molar mass 4.20- gimol 2.10 mol 1 By ran, Heat absorbed by producing 2 mol H₂ = 90.2 kJ 7 Heat absorbed when producing 2.10 mol H2 = ( 90.24 x2010) kJ - 94.71KI]