Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen:

CO (g) + 2H2 (g) -> CH3OH (g)

An equilibrium mixture in a 2.50 L vessel is found to contain 2.62e-2 mol CH3OH, 0.170 mol CO, and 0.303 mol H2 at 500 K.

Calculate Kc at this temperature.

Write the Keq expression.

That is
Kc = (CH3OH)/(H2)^2(CO)
Calculate concns of each by dividing the equilibrium in moles/2.50 L, plug those into the Keq expression and run the numbers through a calculator.

the density of methanol at 20c is 0.791g/ml. what is the mass in grams of 280ml sample

1.67

To calculate the equilibrium constant (Kc) at this temperature, you need to use the concentrations of the reactants and products. The balanced equation for the reaction is:

CO (g) + 2H2 (g) -> CH3OH (g)

The coefficients in the balanced equation tell us the mole ratio between the reactants and products. Thus, the concentration of CH3OH is already given as 2.62e-2 mol in a 2.50 L vessel, giving a concentration of:

[CH3OH] = 2.62e-2 mol / 2.50 L = 1.05e-2 M

Next, we need to determine the concentration of CO and H2 using the given moles and the volume of the vessel. The concentration can be calculated as:

[CO] = 0.170 mol / 2.50 L = 0.068 M
[H2] = 0.303 mol / 2.50 L = 0.121 M

Now, we can apply the law of mass action to calculate the equilibrium constant Kc. The expression for Kc is:

Kc = [CH3OH] / ([CO] * [H2]^2)

Plugging in our values:

Kc = (1.05e-2 M) / ((0.068 M) * (0.121 M)^2)

Now, calculate the value of Kc using this equation.