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16 Nov 2019

Hydrazine reacts with O2 to form water and N2. N2H4(ℓ) + O2(g) → 2H2O(ℓ) + N2(g) ΔHr° = -622.29 kJ/mol-rxn ΔrS° = 4.87 J/K⋠mol-rxn ΔrG° = -623.75 kJ/mol-rxn Because this is an exothermic reaction, energy is evolved as heat. What temperature change is expected in a heating system containing 3.4 x 10^4 L of water if 1.00 mole of N2H4(ℓ) reacts? Assume no energy is lost to the surroundings.

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16 May 2019

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Express your answer using two significant figures.

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Express answer to 4 sig figs.

5.

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2NO(g) + O2(g) → 2NO2(g);ΔH° = –114.4 kJ

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a. requires a catalyst.

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c. occurs rapidly.

d. is endothermic.

e. cannot occur.

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a. requires a catalyst.

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c. occurs slowly.

d. is exothermic.

e. cannot occur.

5.What is the change in internal energy of the system (ΔU) if 10 kJ of heat energy is released by the system and  70 kJ  of work is done on the system for a certain process?

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6.What is the quantity of heat evolved at constant pressure when   26.3 g   H2O(l)   is formed from the combustion of H2(g) and O2(g)?

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b. 1.184 mol

c. 0.4223 mol

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e. endothermic, and the temperature of the reaction system would rise.

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