General Chemistry I (Casanova)

Assignment 5: Chapter 5
Name: _____________________________________________
1. Define the following terms: a) Thermodynamics – b) System – c) Surroundings – d) Internal Energy (E) – e) Heat (q) – f) Work (w) – g) First Law of Thermodynamics – h) State function – i) Enthalpy (H) – j) Exothermic process – k) Endothermic process –
l) Specific heat capacity (Cp) – M/W or T/R ? m) Standard states – Setup of each problem must be shown when performing ANY CALCULATION from this point on. Attention
should be given to significant figures. 2. Consider the following figure:
1 atm 1 atm reaction 5 moles
4 moles The following reaction has ΔE = -186 kJ/mol.
a) Is the sign of PΔV negative or positive? Explain. b) What is the sign and approximate magnitude of ΔH? Explain. 3. Assume that a particular reaction evolves 244 kJ of heat and that 35 kJ of PV work is gained by the system.
What is the value of ΔE? 4. Given that: H E P V , at what condition(s) does H E ? Explain. 5. The following chemical equation describes the combustion of methane gas, CH4 (natural gas) in the
presence of atmospheric oxygen: Δ
1CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2O(g) + 74.87 kJ Is this reaction exothermic or endothermic? Explain. c) How much heat is released when 255 ft3 of methane gas is burned with excess oxygen?
( d CH 4 ( g ) 0.717 kg m3 ) (hint: use density to determine mass and use the mass to determine moles) 6. How many calories are required to heat 5.0 g of Pyrex® from 15.0oC to 65.0oC? ( C p 0.20 cal gK ) 7. A substance, metallic in nature, is to be identified, and heat capacity is one of the clues to its identity. A block
of metal weighing 150. g required 38.5 cal to raise its temperature from 22.8oC to 26.4oC. Calculate the specific
heat of the metal and determine if it is the correct alloy, which has a specific heat capacity of 0.0713 cal gK . 8. How much water at 20oC would be necessary to cool a 34.0 g piece of copper (Cu), specific heat 0.0924 cal gK , from 98.0oC to 25.0oC? 9. Determine the heat of formation of liquid hydrogen peroxide, H2O2(l), at 25oC from the following
thermochemical equations. H2(g) + ½ O2(g) H2O(g) ΔHo = -241.82 kJ/mol 2H(g) + O(g) H2O(g) ΔHo = -926.92 kJ/mol 2H(g) + 2O(g) H2O2(g) ΔHo = -1070.60 kJ/mol 2O(g) O2(g) ΔHo = -498.34 kJ/mol H2O2(l) H2O2(g) 10. Using the equation, ΔHo = 51.46 kJ/mol H o n H of (products) m H of (reactants) , determine oxidation of ammonia to nitric oxide, NO.
Pt
4NH 3 (g) +5O 2 (g) 4NO(g) + 6H 2O(g) H rxn for the catalytic

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