Suppose a 500. mL flask is filled with 1.9 mol of NO and 1.5 mol of NO₂. The following reaction becomes possible: NO3(g) + NO(g) → 2NO₂(g) The equilibrium constant K for this reaction is 0.433 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M X
Suppose a 500. mL flask is filled with 1.9 mol of NO and 1.5 mol of NO₂. The following reaction becomes possible: NO3(g) + NO(g) → 2NO₂(g) The equilibrium constant K for this reaction is 0.433 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M X
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Transcribed Image Text:Suppose a 500. mL flask is filled with 1.9 mol of NO and 1.5 mol of NO₂. The following reaction becomes possible:
NO3(g) + NO(g) + 2NO₂(g)
The equilibrium constant K for this reaction is 0.433 at the temperature of the flask.
Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
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X
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Expert Solution
Step 1
Given
Initial Concentration of NO = 1.9
Initial Concentration of NO2 = 1.5
K = 0.433
Volume = 500 ml
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It asked me to round up so I put 4.7 and it's still wrong please try again.
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Your answer is incorrect.
Suppose a 500. mL flask is filled with 1.9 mol of NO and 1.5 mol of NO2. The following reaction becomes possible:
NO3(g) + NO(g) → 2NO₂(g)
The equilibrium constant K for this reaction is 0.433 at the temperature of the flask.
Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
4.7 M
X
S
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