Consider the following reaction: 2H2(g) + O2(g) → 2H2O(1) ΔH = -572 kJ

Question

Question

1. Consider the following reaction:

2H₂(g) + O2(g) → 2H₂O(1) ΔH = -572 kJ

a. How much heat is evolved for the production of 1.00 mole of H₂O(1)?

b. How much heat is evolved when 4.03g hydrogen are reacted with excess oxygen?

c. How much heat is evolved when 186g oxygen are reacted with excess hydrogen?

2. The specific heat capacity of silver is 0.24J/°C g.

a. Calculate the energy required to raise the temperature of 150.0g Ag from 273K to 298K.

b. Calculate the energy required to raise the temperature of 1.0 mole of Ag by 1.0°C (called the molar heat capacity)

c. It takes 1.25 kJ of energy to heat a sample of pure silver from 12.0°C to 15.2°C. Calculate the mass of the sample of silver.

Answer 1

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Answer 2

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