CO(g) + H2O(g) ⇌ CO2(g) + H2(g) Use the appropriate table(s) to determine ΔG^o and Keq at 552 degrees C.
CO(g) + H2O(g) ⇌ CO2(g) + H2(g) Use the appropriate table(s) to determine ΔG^o and Keq...
Write the equilibrium expression for the following reaction. CO2(g) + H2(g)↔ CO(g) + H2O(g) Select one: a. Keq = [CO2] + [H2]/[ CO]+ [H2O] b. Keq = [ CO][H2O] / [CO2] [H2] c. Keq = [ CO] +[H2O] / [CO2] + [H2] d. Keq = [CO2] [H2]/[ CO][H2O]
Use the given data at 700 K to calculate ΔG°for the reaction H2(g) + CO2(g) → H2O(g) + CO(g) Substance H2(g) CO2(g) H2O(g) CO(g) ΔH°f(kJ/mol) 0 -393 -242 -111 S°(J/K·mol) 131 214 189 198 -472 kJ 10.6 kJ -775 kJ -2.94 x 104 kJ
Consider the following redox equation: CO2(g) + H2(g) = CO(g) + H2O(g). Choose an appropriate chemical formula from the list that identifies the substance reduced. CO2 CO H20 H2 Question 42 2 The proper assignment of oxidation numbers to the elements in the compound CaSO4 would be +2 for Ca, +6 for Sand -8 for +2 for Ca, +2 for S and -4 for O +2 for Ca, +6 for S and -2 for O +2 for Ca, +4 for...
Given: H2(g) + CO2(g) <-> H2O(g) + CO(g) [H2]=0.061M [CO2]=0.012M [H2O]=3.1M [CO]=8.4M Calc.Kc. The reaction is performed at a new temperature. An initial sample of 0.23 M H2 and 0.41 M CO2 gives 0.18M H2O and 0.18 M CO at equilibrium. Determine the composition of the equilibrium mixture. Calc. Kc. Of note, I got Kc = 3.6 e 4 for the first part and needed to know if I got the right answer, and I need to see how to...
Consider the following redox equation: CO2(g) + H2(g) =CO(g) + H2O(g). Choose an appropriate chemical formula from the list that identifies the substance oxidized. CO2 O H20 ca H2 Question 45 2 pts For a collision between molecules to result in reaction, the molecules must possess a certain minimum energy and have a favorable orientation relative to each other when they collide exchange electrons interact with a catalyst carry the same charges
for the reaction CO(g) + H2O(g) <-> CO2(g) + H2(g) K=2 at a certain temperature. If at this temperature, [H2] = 2 M, [CO]=2 M, and [H2O] =0.2 M, calculate [CO2] For the reaction CO(g) + H2O(g) + CO2(g) + H2(g) K = 2 at a certain temperature. If at this temperature, [H2) = 2 M, [CO] = 2 M, and [H2O) = 0.2 M, calculate (CO2). 0.8 M 4M 0.2 M 0.4 M 5 M
If K= 0.00490 for the reaction CO2(g) + H2(g) + CO(g) + H2O(9), what is the K value for the reaction CO(g) + H2O(g) + CO2(g) + H2(g)?
13. Consider the following equation 2 C(s) + 2 H2O(g) + CH, (g) + CO2(g) Determine the standard enthalpy change for this reaction from the following standard enthalpies of reaction : (1) C(s) + H2O(g) + CO(g) + H2(g) AH° = 131.3 kJ (2) CO (g) + H2O(g) + CO2(g) + H2(g) AH° = -41.2 kJ (3) CH, (g) + H2O(g) + 3H2(g) + CO (g) AH° = 206.1 kJ A. 15.3 B. -116.1 C. 378.2 D. -427.0
Consider the following equilibrium process at 686 ° C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0480 M, [H2] = 0.0400 M, [CO2] = 0.0880 M, and [H2O] = 0.0430 M. (a) Calculate Kc for the reaction at 686 ° C. (b) If we add CO2 to increase its concentration to 0.510 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M...
4. Consider the following reaction at equilibrium CO(g) + H2O(g) + CO2(g) + H2(g) 2.50 mole of CO(g) and 2.50 mole of H2O(g) gas at 588 K are mixed in a 10.00 L container. (Kc = 31.4 at 588 K) Calculate the concentration of CO(g), H2O(g), CO (g), and H.(g) at equilibrium. 5. Consider the following reaction: CO(g) + H2O(g) + CO2(g) + H2(g) (a) If a 10.00L container has 2.50 mole of CO(g), 2.50 mole of H2O(g), 5.00 mole...