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- What is the type of the following reaction?
2HgO(s) 2Hg(I) + O2(g)
The answer is ……………………….
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- A 1.00-L flask was filled with 2.00 moles of gaseous SO2 and 2.00 moles of gaseous NO2 and heated. After equilibrium was reached, it was found that 1.34 moles of gaseous NO was present. Assume that the reaction SO-(9) + NO2 (g) = SO; (g) + NO(9) occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction. K =The equilibrium constant, Kc , for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) is 6.90 x 103 . (a) What is Kc for the reaction 2 SO3 (g) → 2 SO2 (g) + O2 (g) (b) What is Kc for the reaction SO2 (g) + 1/2 O2 (g) → SO3 (g)Write an expression for the equilibrium constant for this reaction: N2O4(g)+ O3(g)=N2O5(s)+O2(g)
- What is the CORRECT equilibrium constant expression for the reaction of N2O (g) and O2(g) to produce NO(g)?Write the balanced chemical equation for conversion of Al(s) to KAl(SO4)2·12H2O(s) in aqueous solution.The reaction 2CO(g) + O2(g) = 2 CO2(g) is known to be exothermic. According to Le Chatelier's principle, how will this reaction's equilibrium be affected if the reaction temperature is increased? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will increase and the reaction will shift to the right. (D) The equilibrium constant will be unchanged, but the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.
- Consider the reaction: N2(g) + 3H2(g) 2NH3(g) where Kc = 0.500 at 400 °C. If 50.0 L reaction vessel contains 1.000 mole N₂; 3.000 mole H₂ and 0.050 mole NH3, which of the following is TRUE? The reaction based on the following parameters is in equilibrium. More ammonia will be produced as the reaction approaches equilibrium. Data provided is not enough to warrant a conclusion regarding equilibrium. More ammonia will dissociate as the reaction approaches equilibrium.If the K eq = 798 at 25°C for the reaction 2So2 (g) + O2 (g) -> 2SO3 (g) calculate the equilibrium concentration of O2 given that the concentrations of the other chemicals are: [SO2] = 4.20 M; [SO3] = 11.0 MExactly 1.0 mol N2O4 is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N2O4(g) 2NO2(g). If at equilibrium the N2O4 is 28.0% dissociated, what is the value of the equilibrium constant, Kc, for the reaction under these conditions? (need to show your calculation.)
- Suppose Cao is placed in a vacuum in which the partial pressure of oxygen is 10-r mm Hg. Will Cao be reduced?Write the equilibrium expression for the following: 4KO2(s) + 2H2O(g) ↔↔ 4KOH(s) + 3O2(g)Write the reaction quotient, Qc, for each of the following reactions:(a) The first step in nitric acid production, NH3(g) + O2(g) ⇌ NO(g) + H2O(g)(b) The disproportionation of nitrogen monoxide, NO(g) ⇌ N2O(g) + NO2(g)