Determine ΔH for the third reaction from the information given.   C3H8(g) + 3 H2O(g) ↔ 3 CO(g) + 7 H2(g) ΔH = 499.0 kJ CO(g) + H2O(g) ↔ CO2(g) + H2(g) ΔH = -41.00 kJ C3H8(g) + 6 H2O(g) ↔ 3 CO2(g) + 10 H2 ΔH = ?

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  1. Determine ΔH for the third reaction from the information given.

 

C3H8(g) + 3 H2O(g) ↔ 3 CO(g) + 7 H2(g) ΔH = 499.0 kJ

CO(g) + H2O(g) ↔ CO2(g) + H2(g) ΔH = -41.00 kJ

C3H8(g) + 6 H2O(g) ↔ 3 CO2(g) + 10 H2 ΔH = ?

 

 

Q2. How much heat (in kilojoules) is involved in the oxidation of 160.5 g of Fe at 25°C?

 

4 Fe(s) + 3 O 2(g)↔ 2 Fe 23(l) --> ΔH = -1648 kJ

 

 

Q3. The specific heat capacity of Pt is 0.1328 J/g*°C. How many joules of heat are necessary to raise the temperature of 49.06 g of Pt from 25.0°C to 35.25 °C?

 

 

Q4. What is the sign of ΔH for the process of below?

 

2(l) → I 2(s)

 

A. positive and the process is endothermic

B. negative and the process is exothermic

C. positive and the process is exothermic

D. negative and the process is endothermic

 

 

 

 

Q5. The first step in the preparation of lead from galena, PbS, consists of roasting the ore in oxygen. The reaction is

 

2 PbS(s) + 3 O 2(g) ↔ 2 SO 2(g) + 2 PbO(s)

 

What is ΔH° rxn (in kilojoules)?

PbS(s) ΔH f o = -98.3 kJ/mol.

SO 2(g) ΔH f o = -296.8 kJ/mol.

PbO(s) ΔH f o = -219 kJ/mol.

 

 

Q6. What is the sign of ΔH for the process of below?

 

NaCl(l) → NaCl(g)

 

 

A. negative and the process is exothermic

B. positive and the process is exothermic

C. positive and the process is endothermic

D. negative and the process is endothermic

 

 

 

Q7. A simple method for the laboratory preparation of hydrogen involves reaction of zinc with hydrochloric acid;

 

Zn(s) + 2 HCl(aq) → ZnCl 2(aq) + H 2(g) ΔH = -152.5 kJ

 

How much heat in kilojoules is evolved if a total of 732.0 mL of H 2 was collected over water at 20.00 ° C and an atmospheric pressure of 338.8 mm Hg. The partial pressure of water at this temperature is 17.54 mm Hg? Assume heat evolved is directly proportional to the moles produced.

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