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5. (8) A mixture of 2.0 mol of COg) and 2.0 mol of HyO(g) was allowed...
5-7 (ACS-style) A mixture of 2.0 mol of CO (g) and 2.0 mol of H20 (g) was allowed to come to equilibrium in a 10.0-L flask at a high temperature. If Kc = 4.0, what is the molar concentration of H2 (g) in the equilibrium mixture? The equation for the reaction is: CO(g) + H20 (g) 5 CO2(g) + H2 (g) A) 0.67 M B) 0.40 M C) 0.20 M D) 0.13 M
please explain why the correct answer is D.) f2.0 mol of CO(g) and 2.0 mol of H-0(g) was allowed to come to equilibrium in a 100 ature. If Ke -4.0, what is the molar concentration of H(g) in the equilibrium COg)+H,Og)CO,(8)+H,g) mixture? (B) 0.40 M (C) 020 M 0.67 M (D) 0.13 M
A 2.0 L flask is filled with 0.30 mol SO3 , 0.40 mol of SO2 and 0.50 mol of O2 and allowed to reach equilibrium. Assume the temperature of the mixture is chosen so that Kc = 0.34. Predict the effect on the concentration of SO3 as the equilibrium is achieved by using Q, the reaction quotient. 2SO3(g) —> 2SO2(g) + O2(g)
2. For the reaction: A(g) +B(g) = 2C(g) K = 1.0 x 10-5 at 25°C When equilibrium was reached at 25°C, the equilibrium concentrations of the reactant gases were: [A] = 2.5 x10-2M [B] = 2.0 x 10- M Calculate the equilibrium concentration of the product gas C? 3. At a certain temperature the reaction has an equilibrium constant of 0.400. CO(g) + H2O(g) = CO2(g) + H2(g) When 1.50 mol of carbon dioxide gas and 1.50 mol of hydrogen...
2. A 2.0-L reaction flask initially contains 0.010 mol CO, 0.80 mol H2, and 0.50 mol CH3OH (methanol). If this mixture is brought in contact with zinc oxide-chromium(III) oxide catalyst, the equilibrium CO(g) + 2H2(g) = CH2OH(g) Is obtained. The equilibrium constant, Kc, for this reaction at 300°C is 1.1 x 10-2. What is the direction of reaction (forward or reverse) as the mixture attains equilibrium?
A mixture of 0.05621 mol of H2O, 0.03410 mol of CH4, 0.04592 mol of CO, and 0.04764 mol of H2 is placed in a 1.0-L steel pressure vessel at 1350 K. The following equilibrium is established: 1 H2O(g) + 1 CH4(g) 1 CO(g) + 3 H2(g) At equilibrium 0.01484 mol of CH4 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of H2O, CH4, CO, and H2. Peq(H2O) = . Peq(CH4) = . Peq(CO) = . Peq(H2) = . (b) Calculate...
Calculate the concentrations of all substances present in the equilibrium mixture, if 2.35 mol of H2 and 2.35 mol of I2 are placed in a 10.0 L flask and allowed to come to equilibrium, at which time 3.76 mol of HI are present. The reaction is H2(g) + I2(g) --> 2HI (g) What is the value of Kc? What is the value of Kp?
A mixture of 2.5 moles of H2O and 100g of C are placed in a 50.0L container and allowed to come to equilibrium in the following reaction: C(s) +H2O(g) <-> CO(g) + H2(g) The equilibrium concentration of hydrogen gas is found to be 0.040M. What is the equilibrium concentration of the water vapour?
I NEED A COMPLETE AND CLEAR SOLUTION PLEASE! thanks A mixture of 0.10 mol of NO, 0.050 mol of H2 and 0.10 mol of H2O is placed in a 1.0-L flask and allowed to reach equilibrium as shown below: 2 NO (g) +2 H(g)N2 (g) + 2 H2O (g) At equilibrium [NO] = 0.062 M. Calculate the equilibrium constants Kc and Kp for this reaction.
Consider the equilibrium C(s)+ CO2(g) ⇌2 CO(g) A 2.0 L flask contains a mixture of 0.10 mol of CO(g), 0.20 mol of CO2(g) and 0.40 mol of C(s) in equilibrium at 700°C. *Note that only atm pressure values are allowed in the K expression.* The value of the equilibrium constant K is