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ation Page Suppose a 250. mL flask is filled with 0.80 mol of NO and 1.8 mol of NO₂. The following reaction becomes possible: NO3(g) + NO(g) → 2NO₂(g) The equilibrium constant K for this reaction is 0.445 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places.

ation Page Suppose a 250. mL flask is filled with 0.80 mol of NO and 1.8 mol of NO₂. The following reaction becomes possible: NO3(g) + NO(g) → 2NO₂(g) The equilibrium constant K for this reaction is 0.445 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places.

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Why are the initial concentrations for NO and NO2 3.2 and 7.2 respectively? Wouldn't the initial concentration just be 0.8 M and 1.8 M NO2?

Explanation Page ? QUESTION Suppose a 250. mL flask is filled with 0.80 mol of NO and 1.8 mol of NO₂. The following reaction becomes possible: NO3(g) + NO(g) + 2NO₂(g) The equilibrium constant K for this reaction is 0.445 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. 00 EXPLANATION The key to solving an equilibrium composition problem is the connection between the equilibrium molarities of each reactant and the equilibrium constant K: [NO₂] [NO3][NO] = K The equilibrium constant expression is on the left side of this equation. You can use this equation to calculate K from the equilibrium molarities. But if you know K instead, you can use the equation "backwards" to calculate the equilibrium molarities. First, set up a reaction table: [NO3] [NO] [NO₂] initial 0 3.2 7.2 change X -2x equilibrium X 3.2+x7.2-2x X Since we're after the equilibrium molarity of NO3, we might as well let x stand for the change in molarity of NO3 olo 18 Ar
Transcribed Image Text:Explanation Page ? QUESTION Suppose a 250. mL flask is filled with 0.80 mol of NO and 1.8 mol of NO₂. The following reaction becomes possible: NO3(g) + NO(g) + 2NO₂(g) The equilibrium constant K for this reaction is 0.445 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. 00 EXPLANATION The key to solving an equilibrium composition problem is the connection between the equilibrium molarities of each reactant and the equilibrium constant K: [NO₂] [NO3][NO] = K The equilibrium constant expression is on the left side of this equation. You can use this equation to calculate K from the equilibrium molarities. But if you know K instead, you can use the equation "backwards" to calculate the equilibrium molarities. First, set up a reaction table: [NO3] [NO] [NO₂] initial 0 3.2 7.2 change X -2x equilibrium X 3.2+x7.2-2x X Since we're after the equilibrium molarity of NO3, we might as well let x stand for the change in molarity of NO3 olo 18 Ar
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