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CS 2(g) + 3C1 2(9) CC1 4(g) + S 2C12(g) At a given temperature, the reaction above is at equilibrium when [CS2] = 0.050 M, [C12] = 0.25 M, [CC14] = 0.15 M, and [S2C12] = 0.35 M. What would be the direction of the reaction when the reactants and products have the following concentrations: CS2 = 0.15 M, C12 = 0.26 M₂ CC14 = 0.31 M, and S2C12 = 0.36 M? O a. no change O b. to the right Oc. to the left O d. cannot predict unless we know whether the reaction is endothermic or exothermic O e. cannot predict unless we know the temperature

CS 2(g) + 3C1 2(9) CC1 4(g) + S 2C12(g) At a given temperature, the reaction above is at equilibrium when [CS2] = 0.050 M, [C12] = 0.25 M, [CC14] = 0.15 M, and [S2C12] = 0.35 M. What would be the direction of the reaction when the reactants and products have the following concentrations: CS2 = 0.15 M, C12 = 0.26 M₂ CC14 = 0.31 M, and S2C12 = 0.36 M? O a. no change O b. to the right Oc. to the left O d. cannot predict unless we know whether the reaction is endothermic or exothermic O e. cannot predict unless we know the temperature

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section12.5: Using Equilibrium Constants
Problem 12.5PSP: For the equilibrium 2 SO2(g) + O2(g) 2 SO3(g) Kc = 245 (at 1000 K) the equilibrium concentrations...
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CS 2(g) + 3C1 2(g) CC1 4(g) + S 2C1 2(g) At a given temperature, the reaction above is at equilibrium when [CS2] = 0.050 M. [C12] = 0.25 M, [CC14] = 0.15 M, and [S2C12] = 0.35 M. What would be the direction of the reaction when the reactants and products have the following concentrations: CS2 = 0.15 M, C12 = 0.26 M. CC14 = 0.31 M, and S2C12 = 0.36 M? a. no change Ob. to the right Oc. to the left O d. cannot predict unless we know whether the reaction is endothermic or exothermic Oe. cannot predict unless we know the temperature
Transcribed Image Text:CS 2(g) + 3C1 2(g) CC1 4(g) + S 2C1 2(g) At a given temperature, the reaction above is at equilibrium when [CS2] = 0.050 M. [C12] = 0.25 M, [CC14] = 0.15 M, and [S2C12] = 0.35 M. What would be the direction of the reaction when the reactants and products have the following concentrations: CS2 = 0.15 M, C12 = 0.26 M. CC14 = 0.31 M, and S2C12 = 0.36 M? a. no change Ob. to the right Oc. to the left O d. cannot predict unless we know whether the reaction is endothermic or exothermic Oe. cannot predict unless we know the temperature
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