2) I500J of heat is added to a metal with a mass of 50 g and a specific heat capacity of 0.8 What is the change in temperature of the metal?

3) Some water is heated up with 540 J causing its temperature to increase by 8.0 degrees C. What was the mass of the water?

4) When 26.7 g of H2S was burned in excess oxygen, 406 kJ was released. What is ∆H for the following equation?
2 H2S(g) + 3 O2(g) 2 SO2(g) + 2 H2O(g) ∆ H = ???

5) Calculate ∆H for the following equation:
PbCl2(s) + Cl2(g) → PbCl4(l) ∆ H = ??? Given: Pb(s) + Cl2(g) PbCl2(s) ∆ H1 = -359.4 kJ Pb(s) + 2 Cl2(g) PbCl4(l) ∆H2 = -329.3 kJ

6) Calculate ∆H for the following equation:
2 C(s) + 3 H2(g) → C2H6(g) given the following data: ∆H = ??? (1) 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(l) ∆H1 = -3120 kJ (2) C(s) + O2(g) → CO2(g) ∆H2 = -394 kJ
(3) 2 H2(g) + O2(g) → 2 H2O(l) ∆H3 = -572 kJ
7) Given table shows standard molar enthalpy of formation of some matters. Find enthalpy of C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) using data given in the table above.
8) To calculate the enthalpy of; CO2(g) + H2(g) → CO(g) + H2O(g) which ones of the following must be known?
I. Molar formation enthalpy of H2O(g)
II. Molar formation enthalpies of CO(g) and CO2(g)
III. Enthalpy of reaction; H2(g) + 1/2O2(g) → H2O(g)
9) Find molar combustion enthalpy of C2H5OH using following molar enthalpies of matters; ∆H C2H5OH(l)= -67 kcal/mol ∆H CO2(g)= -94 kcal/mol ∆H H2O(l)= -68 kcal/mol
10) There are 32 g S in 1000 g vitreous calorimeter having 1000 g water in it. If 32 g S is burned up in calorimeter, temperature rises from 20 0C to 90 0C. Find molar combustion enthalpy of S. Note that the glass temperature of the calorimeter also increases. Given specific heat of water = 4.186 j/g℃ Specific heat of glass = 0.8 j/g℃
11) During reaction of formation Al2O3 from 5,4 g Al and enough amount of O2, temperature of 2 kg water increases 20 0C. Find formation enthalpy of Al2O3 ? (molar mass of Al=27 g/mol, cwater=1 cal/g.0C)
12) Enthalpies of two reaction are given below.
I. A + B → C + 2D ∆H1=+X kcal/mol
II. C + E → A + F ∆H2=-Y kcal/mol Find enthalpy of A + 2B + E → C + 4D + F reaction in terms of X and Y.
13) C(s) reacts with O2(g) and after reaction, 8,96 L CO2 gas is formed and 37,6 kcal heat is released. According to this information, which one of the following statements are true? Explain (M(C)=12 g/mol, M(O)=16 g/mol) note: volume is measured at STP.
I. Reaction is exothermic
II. 94 kcal heat is required to decompose CO2(g) into its elements
III. 23,5 kcal heat is required to form 11g CO2(g)
IV. Sum of enthalpies of products is smaller than the sum of enthalpies of reactants