For questions 14-18. What wil| happen to the number of moles of SO3 in equilibrium with SO2 and 02 in the reaction? 2SO3(g) = 2SO2(g) + 02(g). 17. The temperature is decreased (the reaction is endothermic). * O increase O decrease

Consider the following exothermic reaction: C (s)   +   2 Cl2 (g)   ⇋⇋   CCl4 (g) How would the equilibrium shift if the reaction mixture is heated? Select one: a. The reaction would shift towards the products. b. The reaction would shift towards the reactants. c. The equilibrium would not be affected.

which statement is true?

Question 29 of 30 Consider the reaction of N2O and O2 described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 NO(g) +3 O₂(g) 4 NO2(g) 1 2 NEXT > A 1.00 L reaction vessel was filled with 0.0560 mol O2 and 0.200 mol N2O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. 2N₂O(g) + 302(g) == 4NO2(g) Initial (M) 0.200 -0.0100 0.190 Change (M) 0.0560 -0.0150 0.0410 Equilibrium (M) 0 0.0200 0.0200 RESET 0 0.0560 0.200 -1.00 -0.0560 0.0200 -0.0200 0.0100 -0.0100 -0.0050 0.0050 0.0150 -0.0150 0.210 0.190

Why would answer choice (c) for question 16 be correct?

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Consider the following exothermic reaction: C (s)   +   2 Cl2 (g)   ⇋⇋   CCl4 (g) How would the equilibrium shift if the reaction mixture is heated? Select one: a. The reaction would shift towards the products. b. The reaction would shift towards the reactants. c. The equilibrium would not be affected.

Which way would the equilibrium shift if the temperature was decreased for this reaction (AH = -542 kJ)? H₂ (g) + F₂ (g) → 2HF (g) Shift toward reactants Shift toward products Remain the same None of the above