Suppose a 250 ml flask is filled with 1.3mol of o2 and 1.5 mol of no. the following reaction becomes possible: the equilibrium constant for this reaction is at the temperature of the flask. calculate the equilibrium molarity of . round your answer to two decimal places.

The equilibrium molarity of oxygen gas is 7.1 M

Explanation:

We are given:

Moles of oxygen gas = 1.3 mole

Moles of NO = 1.5 moles

Volume of the flask = 250 mL = 0.250 L   (Conversion factor:  1 L = 1000 mL)

To calculate the molarity, we use the equation:

Molarity of oxygen gas =

Molarity of NO =

The chemical equation follows:

Initial:                  5.2    -           6.0

At eqllm:          5.2+x     +x      6.0-2x

The expression of for above equation follows:

  (Assuming)

Putting values in above equation, we get:

Neglecting the value of x = 5.4 because this cannot be greater than the initial value.

Concentration of oxygen gas at equilibrium = (5.2 + x) = 5.2 + 1.9 = 7.1 M

Hence, the equilibrium molarity of oxygen gas is 7.1 M

these nuts

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)