1.How much heat is evolved when 27.0 g of glucose is burned according to this equation?

C6H12O6 + 6O2 → 6CO2 + 6H2O; Δ H comb. = -2808 kJ/mol

421kJ

241kJ

280kJ

136kJ

2.How much heat is required to melt 200 grams of ice?

The heat of fusion is 333 J/g.

1.16kJ

6.66kJ

66.6kJ

666kJ

3. Calculate the amount of heat absorbed by 10.0 grams of ice at -15.0°C as it is converted to liquid water at 50.0°C. The specific heat of H2O(s) = 2.09 J/(g°C). The specific heat of H2O(l) = 4.18 J/(g°C). The heat of fusion is 333 J/g.

0.676kJ

5.73kJ

2.83kJ

0.170kJ

4.From the following data,

H2 (g) + Cl2 (g) → 2HCl(g) Δ*H*v = -185 kJ

2H2 (g) + O2 (g) → 2H2O(g) Δ*H* = -483.7 kJ

calculate Δ*H* for the following reaction.

4HCl(g) + O2 (g) → 2Cl2 (g) + 2H2O(g)

-299kJ

114kJ

299kJ

-114kJ

5.Given the following information,

SO3 (g) + H2O(l) → H2SO4 (l) Δ*H* = -133 kJ

Pb(s) + PbO2 (s) + 2H2SO4(l) → 2PbSO4(s) + 2H2O(l) Δ*H* = -509 kJ

calculate the Δ*H* for the reaction below.

Pb(s) + PbO2 (s) + 2SO3 (g) → 2PbSO4 (s)

-775kJ

376kJ

775kJ

-376kJ

#### Top Answer

1 . Amount released when 27.0 g is burned is 421.2 KJ 2. Heat is required... View the full answer

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#### Other Answers

1) Δ H comb will be = -421.2 KJ, option (A) is correct. 2) q = 66.6 KJ.,... View the full answer