The equilibrium constant, Ke, for the following reaction is 0.0952 at 350. K. CH4 (9) + CCl4 (9) 2CH₂Cl₂ (g) Calculate the equilibrium concentrations of reactants and product when 0.205 moles of CH4 and 0.205 moles of CC14 are introduced into a 1.00 L vessel at 350. K. [CH] = M [CC14] = [CH₂Cl₂] m M M

Be sure to answer all parts. The equilibrium constant K, for the reaction H2(g) + I2(g) =2 HI(g) is 54.3 at 430°C. Calculate the equilibrium concentrations of H,, I,, and HI at 430°C if the initial concentrations are [H2] = [I2] = 0.222 M and [HI] = 0 M. (H2leq = |0.0692 [Lleg =|0.182 [HI]eg =0.826 < Prev 18 of Microsoft Store

15.0 g of glucose reacts with oxygen in a 15.0 L container. At 250°C the system reaches equilibrium. At equilibrium it is determined that there are 5.25 mol of oxygen, 1.84 mol of carbon dioxide and 5.66 mol of steam. Calculate the value of the the equilibrium constant Kc. C6H12O6(s) + 602(g) = 6 CO2(g) + 6H2O(g) O9.64 x 10-5 O5.35 x 10 6 9- O1.87 x 105 O 0.0164 60.9

At a certain termperature, Kc = 0.914 for the reaction NO₂(g) + NO(g) = N₂O(g) + O₂(g) A mixture was prepared containing 0.200 mol NO2, 0.300 mol NO, 0.150 mol N₂O, and 0.250 mol O₂ in a 8.00 L container. What will be the equilibrium concentrations of each gas? [NO₂] [NO] [N₂O] [0₂] i i i i M M M M

The equilibrium constant, Ke, for the following reaction is 10.5 at 350 K. 2CH,Cl2(g)CH,(g) + CC14(g) =CH¾(g) + CC1¼(g) Calculate the equilibrium concentrations of reactant and products when 0.374 moles of CH2C1, are introduced into a 1.00 L vessel at 350 K. [CH2C2] =| M [CH4] M [CCL4] M ||

The value of the equilibrium constant is Ke = 0.052 at 600 °C for the reaction: 2 S03 (g) = 2 S02 (g) + 02 (g). Now we mix 0.72-mol SO3, 0.31-mol SO2 (g) and 0.11-mol 02 (g) in a 1-L container. Which of the following statements is (or are) true? a) The reaction will proceed to left (shift to the reactant side) to reach equilibrium. b) The concentration of SO3 will increase during the reaction course. c) The concentration of SO2 will increase during the reaction course. %3! a) only bi only Og only Oa and b) O b) and c) O and a) O a), b) and c) Neither of the 3 statements is true.

In a 250 ml sealed container at 150 degrees celsius, 0.50 mol of both iodine gas 12(g)and bromine gas. Br2(g), are mixed and allowed to react until they form an equilibrium with iodine mono-bromide gas, IBR(g). The equilibrium constant for the reaction is 1.2*10^2. What are the equilibrium concentrations for iodine and bromine gas?

A 3 L flask is filled with 0.45 mol SO3, 0.50 mol SO2, and 0.20 mol O2, and allowed to reach equilibrium. Assume the temperature of the mixture is chosen so that Kc = 0.12. Predict the effect on the concentration of SO3 as equilibrium is achieved by using Q, the reaction quotient. 2SO3(g)  ⇆  2 SO2(g) + O2(g) [SO3] will decrease because Q > K. [SO3] will decrease because Q < K. [SO3] will increase because Q < K [SO3] will increase because Q > K. [SO3] will remain the same because Q = K.

Be sure to answer all parts. The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) = 2NO(g) K = 4.3 x 10-25 2NO(g) + O2(g) == 2NO,(g) K= 6.4 × 10' Determine the value of the equilibrium constant for the following equation at the same temperature: N2(g) + 202(g) = 2NO2(g) K. - x 10 (Enter your answer in scientific notation.)

Use the References to access important values if needed for this question. The equilibrium constant, Kc, for the following reaction is 0.0290 at 1150 K. 2SO3 (g)2SO2(g) + O2(g) If an equilibrium mixture of the three gases in a 19.7 L container at 1150 K contains 0.251 mol of SO3(g) and 0.353 mol of SO2, the equilibrium concentration of O₂ is M. Submit Answer Retry Entire Group 9 more group attempts remaining