Question

uestion Completion Status: N204(8) <...> 2 NO 2(8) At 25°C, 0.11 mole of N204 reacts to form 0.10 mol of N204 and 0.02 mole of NO 2. At 90'C, 0.11 mole of N204 forms 0.050 moles of N204 and 0.12 mole of NO2. From this data, we can conclude The reaction is exothermic the equilibrium constant for the reaction above increases with an increase in temperature. N204 molecules react faster at 25°C than at 90°C. O None of these are correct QUESTION 10 2.5 points Save Answer For the reaction system, N2(g) + 3H2(8) 2NH3(g) + heat the conditions that would favor the maximum conversion of the reactants to products would be high temperature and high pressure O high temperature, pressure unimportant O high temperature and low pressure O low temperature and high pressure QUESTION 11 2.5 points Save Answer Solid Hgo, liquid Hg, and gaseous O2 are placed in a glass bulb and are allowed to reach equilibrium at a given temperature. 2HgO(s) <-> 2Hg(l) + O2(g) AH = +43.4 kcal The mass of Hgo in the bulb could be increased by O Adding more Hg O removing some 02 O reducing the volume of the bulb O increasing the temperature

Answer 1

9. Option B, equilibrium constant is increased With temperature.

Since more no of moles of NO2 is formed at 90°C and less no of moles of Reactant remains  

10. Option D, at low temperatures and high pressure. Since it is an example for exothermic reaction as it involves the liberation of heat.

11. Option C, teducing the volume of the bulb.

Since it is an endothermic reaction and decrease in the volume will shift the equilibrium towards less no of moles of molecules, ie, Reactant side.