The reaction. N₂0₁2 NO₂ is allowed to reach equilibrium in a chloroform solution at 25 °C. The equilibrium concentrations are 0.490 mol/L N₂O, and 2.34 mol/L NO₂. Calculate the equilibrium constant, K., for this reaction. K₂ = An additional 1.00 mol NO₂ is added to 1.00 L of the solution and the system is allowed to reach equilibrium again at the same temperature. Select the direction of the equilibrium shift after the NO, is added. O towards the reactant towards the product no change Determine how the addition of extra NO, in the previous step will affect the rate constant, K. Ke will increase Ke will decrease Ke will not change

Chemistry
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Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 23Q: Consider the reaction 2N2O(g) + O2(g) 4NO(g) Suppose the system is at equilibrium, and then an...
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Determine how the addition of extra NO₂ in the previous step will affect the rate constant, Ke
OK, will increase
K, will decrease
OK, will not change
Calculate the equilibrium concentrations of N₂O, and NO₂ after the extra 1.00 mol NO₂ is added to 1.00 L of solution.
[N₂O₁] =
[NO₂] =
mol/L
mol/L
Transcribed Image Text:Determine how the addition of extra NO₂ in the previous step will affect the rate constant, Ke OK, will increase K, will decrease OK, will not change Calculate the equilibrium concentrations of N₂O, and NO₂ after the extra 1.00 mol NO₂ is added to 1.00 L of solution. [N₂O₁] = [NO₂] = mol/L mol/L
The reaction.
N₂0₁2 NO₂
is allowed to reach equilibrium in a chloroform solution at 25 °C. The equilibrium concentrations are 0.490 mol/L N₂O, and
2.34 mol/L NO₂.
Calculate the equilibrium constant, K., for this reaction.
K₂ =
An additional 1.00 mol NO₂ is added to 1.00 L of the solution and the system is allowed to reach equilibrium again at the
same temperature. Select the direction of the equilibrium shift after the NO, is added.
towards the reactant
towards the product
no change
Determine how the addition of extra NO, in the previous step will affect the rate constant, Ke
Ke will increase
Ke will decrease
Ke will not change
Transcribed Image Text:The reaction. N₂0₁2 NO₂ is allowed to reach equilibrium in a chloroform solution at 25 °C. The equilibrium concentrations are 0.490 mol/L N₂O, and 2.34 mol/L NO₂. Calculate the equilibrium constant, K., for this reaction. K₂ = An additional 1.00 mol NO₂ is added to 1.00 L of the solution and the system is allowed to reach equilibrium again at the same temperature. Select the direction of the equilibrium shift after the NO, is added. towards the reactant towards the product no change Determine how the addition of extra NO, in the previous step will affect the rate constant, Ke Ke will increase Ke will decrease Ke will not change
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