1.The equilibrium-constant expression depends on the __________ of the reaction.A) stoichiometryB) mechanismC) stoichiometry and mechanismD) the quantities of reactants and products initially presentE) temperature2.At a certain temperature, 0.200 moles of NO, 0.300 moles of Cl2, and 0.500 moles of ClNO were placed in a 25.0 L vessel and allowed to reach equilibrium:2NO(g) + Cl2(g) = 2ClNO(g)At equilibrium, 0.600 moles of ClNO were present. How many moles of Cl2 are present at equilibrium? [enter number with three decimal places]3.The relationship between the concentrations of reactants and products of a system at equilibrium is given by the law of mass action.A) TrueB) False4.Consider the following three reactions:1. H2(g) + Cl2(g) = 2HCl(g)2. C(s) + H2O(g) = CO(g) + H2(g)3. Fe3O4(s) + 4H2(g) = 3Fe(s) + 4H2O(g)For which of these is Kp not equal to Kc?A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 2 onlyE) 1 and 3 only5.What is the expression for Kc for the following reaction?NH4Cl(s) = HCl(g) + NH3(g)A) 1/[HCl][NH3]B) [HCl][NH3]C) [NH4Cl]/[HCl][NH3]D) [HCl][NH3]/[NH4Cl]E) [NH4Cl]6.CH4(g) + 2H2S(g) = CS2(g) + 4H2(g)If units were explicitly specified for Kp of the reaction above, they would be [atm]n. What would be the value of n for this reaction? [enter integer]7.The number obtained by substituting starting reactant and product concentrations into an equilibrium-constant expression is known as the reaction quotient.A) TrueB) False8.Methanol is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen:CO(g) + 2 H2(g) = CH3OH(g)An equilibrium mixture in a 2.00-L vessel is found to contain 0.0406 mol CH3OH, 0.170 mol CO, and 0.302 mol H2 at 500 K. What is Kp at this temperature?A) 6.22 x 10?3B) 4.22 x 10?2C) 0.57D) 4.65E) 10.59.Consider the reaction:2NH3(g) = N2(g) + 3H2(g)Suppose 3 moles of pure NH3 are placed in a 1.0liter flask and allowed to reach equilibrium. If “x” represents the concentration in moles per liter of N2 present in the system once equilibrium is reached, which one of the following will represent the concentration of H2 at equilibrium in moles per liter?A) 3 – xB) 3 – (x/2)C) 3 – 2xD) 2xE) 3×10.Consider the following reaction at equilibrium:2NH3(g) = N2(g) + 3H2(g)Le Chatelier’s principle predicts that adding N2 (g) to the system at equilibrium will result in __________.A) a decrease in the concentration of NH3 (g)B) a decrease in the concentration of H2 (g)C) an increase in the value of the equilibrium constantD) a lower partial pressure of N2E) removal of all of the H2 (g)
The equilibrium-constant expression depends on the __________ of the reaction.
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