Which direction will the reaction 2NO + O2 <--> 2NO2 move if the initial partial pressure of all the species present is 0.50 atm? Show the calculation of Q to support your answer.

What is Kp?

Qp = ((0.5)^2/(0.5)^2(0.5)
Q = 1/0.5 = 2

The pressure on 100 cm^3 of oxygen gas at 35 degree C 750 mm Hg.What will be the volume of the gas in dm^3 if the pressure is increased by 1-third without changing the temperature?

To determine the direction in which the reaction will move, we need to compare the value of the reaction quotient (Q) to the equilibrium constant (K).

The reaction quotient (Q) is calculated by substituting the partial pressures (in atm) of each species into the equilibrium expression. In this case, the reaction equation is:

2NO + O2 ⇌ 2NO2

Therefore, the Q expression is:

Q = [NO2]^2 / [NO]^2 * [O2]

Given that all the species have an initial partial pressure of 0.50 atm, we substitute these values into the Q expression:

Q = (0.50)^2 / (0.50)^2 * 0.50

Simplifying this expression, we get:

Q = 1 / 0.25 * 0.50

Q = 2.00

Now that we have the value of Q, we compare it to the equilibrium constant (K). If Q is less than K, the reaction will move in the forward direction (to the right), and if Q is greater than K, the reaction will move in the reverse direction (to the left).

Unfortunately, we don't have the value of K specified in the question, so we can't determine the direction of the reaction without additional information.