Consider the following reaction: 2 CH3OH(g)  →  2 CH4(g)  +  O2(g)      ΔH = +252.8 kJ Is this reaction exothermic or endothermic? Endothermic   Calculate the amount of heat transferred when 24.0g of CH3OH is decomposed by this reaction at constant pressure.

A 50.0 mL sample of a 1.00 MM solution of CuSO4CuSO4 is mixed with 50.0 mL of 2.00 MM KOHKOH in a calorimeter. The temperature of both solutions was 24.6 oCoC  before mixing and 32.8 oCoC  after mixing. The heat capacity of the calorimeter is 12.1 J/K.  From these data, calculate ΔHΔH for the process: CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M)CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M) Assume that the specific heat and density of the solution after mixing are the same as those of pure water and that the volumes are additive.

2. A calorimeter contains 100.0 g of water at 39.8 °C. A 12.78 g object at 100.0 ºC is placed inside the calorimeter. When equilibrium has been reached, the new temperature of the water and metal object is 40.6 °C. What is the specific heat of the metal?

What is the enthalpy change for the first reaction? Fe2O3(s) → 2Fe(s) + 3/2O2(g) ΔH =  4Fe(s) + 3O2(g) → 2Fe2O3 (s) ΔH = -1,652 kJ

A chemical reaction takes place in an open flask. The reaction releases 355 kJ of heat and does 25 kJ of work on the surroundings. Is the reaction endothermic or exothermic? Calculate ΔH for the reaction. Calculate ΔU for the reaction.

26. Calculate the enthalpy change for the reaction below. NO(g) + O(g) →→→ NO₂(g) Given following data: NO(g) + O₂(g) →→ NO₂(g) + O₂(g) 03(g) → 1.50₂(g) 0₂(g) →20(g) AH-198.9 kJ AH = -142.3 kJ ΔΗ = 495.0 kJ

What is the enthalpy change for the first reaction? CH4(g) + 1/2O2(g) → CH3OH(g) ΔH =  CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)  ΔH = -806.5 CH3OH(l) + 3/2 O2 → CO2(g) + 2H2O(g)  ΔH = -676.7

Consider the reaction: 4A + B= 2C.        Δ H=-443.6Kj/mol what reaction corresponds to a H of Δ221.8 Kj/mol

6, A 0.213 g sample of an organic compound with a molar mass of 386.0 g/mol was burned in the bomb calorimeter with a heat capacity of 2.54 kJ/K. The temperature in the calorimeter increased by 4.12 K. Calculate the energy of combustion of the compound in kJ/mol. A, –1.896 x103 B, –4.90 x102 C, 0.00937 D, –1.90 x104 E, -531

Determine the amount of heat released when 180.00 g AsBr5(g) reacts according to the following equation: As4O10(g) + 6 AsBr5(g)  →  10 Br3AsO(g) Additional equations that may be useful: 1/4 As4(s) + 3/2 Br2(g)  →  AsBr3(g)  ΔH = -336.4 kJ/mol As4(s) + 5 O2(g)  →  As4O10(g) ΔH = -2967.3 kJ/mol AsBr3(g) + Br2(g)  →  AsBr5(g)  ΔH = -84.2 kJ/mol AsBr3(g) + 1/2 O2(g)  →  Br3AsO(g)  ΔH = -295.7 kJ/mol