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Using the following two reactions and their equilibrium constants: Cs) + CO2(g) +200 K= 2.4 X...
Given that K1 and K2 are the respective equilibrium constants for the two reactions CO2(g) + H2(g) = CO(g) + H2O(l) K1 = 3.08×10-4 CdO(s) + H2(g) = Cd(s) + H2O(l) K2 = 40.7 Determine the equilibrium constant for the reaction CO(g) + CdO(s) = CO2(g) + Cd(s) K =
02 INTRO UNIV CHEM Il (LEC D1 Wi18) Te left Use the following equilibrium constants co2(g) + H2(g) <→ CO(g) + H2O(g) K,(400 K) 6.5 x 10 E(s) + 1 /202(g) <==> CO(g) K,(400 K) 1.3 x 1019 CO(g)+ 1/2 O2(g)CO2(g) K,(400 K) 2.8 x 102 CO(g) + 2 H2(g)CH3OH(g) K,(400 k) -2.3 H2(g) + 1 /202(g)-> H2O(g) (400 K)-1.8 x 1029 to determine the equilibrium constant for the following reaction. (You will not need to use all of the...
calculate the equilibrium constants at 25∘C for each of the following reactions. 2 CO(g) + O2(g) = 2 CO2(g) Express your answer using two significant figures. IVO ALQ R o a ? K = Submit Request Answer Part B 2 H2S(9) = 2 H2(g) + S2(g) Express your answer using two significant figures. CO ALQ O ?
Write the equilibrium-constant expression for the equilibrium Cs) + CO2(g) = 200) The table that follows shows the relative mole percent of CO2 and Code) at a total pressure of 1 atm for several temperatures. Calculate the value of Ke at each temperature. Is the reaction exothermic or endothermic? Temperature (°C) 850 950 1050 1250 CO2 (mol %) 6.23 1.32 0.37 0.06 co (mol %) 93.77 98.68 99.63 99.94
Question 26 6 pts 26. Consider the following chemical reaction: CO(g) + Cl2(8) -------------> COC12 (8) At the beginning 0.400 M CO(g) is mixed with 0.0500 M Cl2(g). At equilibrium, 0.0100 M of the product is produced. Calculate the equilibrium constant. OK -8.81 K-1.20 x 10exp-5 K=0.641 OK = 1.99x 10exp-3 Question 27 6 pts 27. Consider the following chemical reaction: N2(g) + 202(8) 2NO2(g) decreasing the pressure of reaction mixture will decrease amounts of O2(g) increase amounts of NO2(g)...
Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 200(g) = CO2(g) + C(s) A. [CO][C]/[CO] B. K [CO] C. [CO] / [CO2) D. [CO]/[CO] E. 2[CO] /[CO][C] In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Châtelier's principle? ООООО A. 2N, () + 0,02N,0 () B. N.O. (g) 2NO, (g) C. N2(g) + 3H2(g)2NH3 (9) D. N2 (9) + 202...
5. Carbonyl fluoride, COF2, can be prepared by the following reaction? CO2(8) + CF4(g) < + 2COF2(g) At 1000°C, K for this reaction is 0.50. What are the partial pressures of all the gases at equilibrium when the initial partial pressures of CO2 and CF4 are 0.513 atm.
For the reaction N2(g) + 3H2(g) = 2NH3(g) what is the value of Ke at 500°C if the equilibrium concentrations are as follows: [H2] = 0.40 M, (N2) = 0.40 M, and (NH3) = 1.9 M Express the equilibrium constant to two significant figures. V AE OE ? Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Set up the equilibrium-constant expression for this reaction using the equilibrium concentrations. The product concentrations a the reactant concentrations are...
PS 50V Consider the reaction below. CO (9) + H2O (9) <=> CO2(g) + H2(g) 200 M CO and 1.00 MH20 are in a one liter flask and the system is allowed to reach equilibrium. Ke at this temperature is 1.56. What is final concentration of CO? (Hint need quadratic) 0.00380 M ООО 2.92 M 1.81 M 127 M 305 x 10M 0.147 M 9.46 x 10M 00432 M
A18. Identify the relationship between the equilibrium constants for the following two reactions at constant temperature H2(g) +Cl2(g)2HCI(g) Equilibrium constant K HCI(g)H2(g)+2Cl2(g) Equilibrium constant K2 Identify the relationship between these equilibrium constants at constant temperature