Consider the equilibrium: Fe3O4(s) + CO(g) ←à 3 FeO(s) + CO2(g) ΔH= +18 kJ. Which of...
Consider the equilibrium: Fe3O4(s) + CO(g) ←à 3 FeO(s) + CO2(g) ΔH= +18 kJ. Which of the following stresses when applied to an equilibrium mixture of reactants and products, will cause [CO] to increase?
I. Decrease in pressure due to a increase in volume.
II. Doubling the [CO2].
III. Addition of a catalyst.
IV. Halving the mass of solid Fe3O4.
V. Increase in the temperature.
A.I only
B. I, II and V
C. I, III and IV
D. II and III
E. III, IV and V
I'm sure B and C were not correct!
Homework Answers
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Consider the equilibrium: Fe3O4(s) + CO(g) ←à 3 FeO(s) + CO2(g)
ΔH= +18 kJ. Which of...
Question 20 2 Points Consider the equilibrium below: FeO (s) + CO (g) <--> Fe (s) + CO2 (g) Kp = 0.403 at 1000.0 o...
Question 20 2 Points Consider the equilibrium below: FeO (s) + CO (g) <--> Fe (s) + CO2 (g) Kp = 0.403 at 1000.0 oC If we start with 1.000 atm of CO and excess FeO at 1000.0 oC and allow the mixture to equilibrate, what will be the equilbrium partial pressure (in atm) of CO? BLANK-1 (ype in the numeric value, give your answer to 3 significant figures, do not use scientific notation) BLANK-1
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18. Write the equilibrium-constant expression (Kp) for the following reaction FeO() + CO(g) > Fe(s) +...
18. Write the equilibrium-constant expression (Kp) for the following reaction FeO() + CO(g) > Fe(s) + CO2(g)
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Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 3 Fe(s) + CO2(g) = Fe3O4(s) + CO(g) 1/[CO] [Fe304][CO] [FO]*[CO2] O [Coy [CO2] [Feo][CO2] [Fe3O4][CO] O [CO2]/[CO]
Chem1 At 1000 K, iron metal is produced through the reaction FeO(s) + CO(g) Fe(s) +...
Chem1
At 1000 K, iron metal is produced through the reaction FeO(s) + CO(g) Fe(s) + CO_2(g) temperature, the equilibrium constant of the reaction is K_e = 0.259. An experiment, is from a mixture containing a solid phase consisting of 4 moles of FeO and 2 moles of Fe and consisting of 1.000 M CO and 0.500 M CO_2. The reaction was followed until the concentration reactants and products showed no further change with time. At this point, the concentration...
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3. Consider the following reaction at equilibrium. + C(s) + H2O (g) + Heat CO (g) +H, (g) a. Is this reaction endothermic or exothermic? (1 point) 2 b. In which direction (right or left) will the equilibrium shift if the following stresses are applied to the reaction at equilibrium? (4 points) i. Remove heat ii. Add CO (g) iii. Remove H20 (g) iv. Add H2 (g)
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Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 3 Fe(s) + CO2(g) = Fe3O4(s) + CO(g) 1/[CO] [Fe304][CO] [FO]*[CO2] O [Coy [CO2] [Feo][CO2] [Fe3O4][CO] O [CO2]/[CO]
Chem1
At 1000 K, iron metal is produced through the reaction FeO(s) + CO(g) Fe(s) + CO_2(g) temperature, the equilibrium constant of the reaction is K_e = 0.259. An experiment, is from a mixture containing a solid phase consisting of 4 moles of FeO and 2 moles of Fe and consisting of 1.000 M CO and 0.500 M CO_2. The reaction was followed until the concentration reactants and products showed no further change with time. At this point, the concentration...
FeO(s) + CO(g)-> Fe(s) + CO2(g) for which the values of equilibrium constants were measured at two different temperatures: Kp(600°C)=0.900 and Kp(1000°C)=0.396. Calculate: a) Δμ° at 600°C; b)ah" and os", assuming they are independent of temperature. NOTE: give your answers in terms of molar quantities.
More Equilibrium: Please write equilibrium expressions for the following reactions: 1. i. 2 SO2 (g) + O2 (g) 2 SO3 (g) il. NH4NOs (s) N2O (g) +2 H20 (g) i CaCO3 (s) + CaO (s) + CO2 (g) iv. HNO2 (aq) +H2O (I) HaO* (aq) + NO2 (aq) 2. Predict which way the equilibrium will shift for each of the following changes: CO (g) + H2 (g) C (s) H2O (g) + heat i. increase [H2O] ii. increase [C0] iii....
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