Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g)+C(s)−⇀↽−CS2(g)Kc=9.40 at 900 K How many grams of CS2(g) can be prepared by heating 18.1 mol S2(g) with excess carbon in a 8.00 L reaction vessel held at 900 K until equilibrium is attained?

Suppose a 500. mL flask is filled with 1.6 mol of H₂ and 0.30 mol of HI. This reaction becomes possible: H₂(g) + 12₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of I2. You can leave out the M symbol for molarity. initial change equilibrium H₂ 0 1₂ x 0 HI 0 X S

Suppose a 500.mL flask is filled with 1.5mol of CO, 1.1mol of H2O and 1.6mol of H2. The following reaction becomes possible: CO(g)+H2O(g)+CO2(g)+H2(g)   The equilibrium constant K for this reaction is 0.840 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places.

Suppose a 250. mL flask is filled with 0.60 mol of SO₂ and 1.0 mol of SO3. This reaction becomes possible: 2SO₂(g) + O₂(g) — 2SO3(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O₂. You can leave out the M symbol for molarity. initial change equilibrium SO₂ 0₂ 0 X 0 SO₂ 0 010 X Ś

For the equilibrium 2lBr(g) = 12(g) + Br2(g) Kc = 8.50 × 10³ at 150 °C. If 0.0600 mol of IBr is placed in a 1.0-L container, what is the partial pressure of I₂(g) in atm after equilibrium is reached?

A gaseous mixture contains 0.27 mol CO, 0.12 mol H2, and 0.022 mol H,O, plus an unknown amount of CH4, in each liter. This mixture is at equilibrium at a certain temperature. CO(9) + 3H, (9) = CH4 (9) + H,O(9) What is the concentration of CH4 in this mixture? The equilibrium constant K, equals 3.99.

Suppose a 250. mL flask is filled with 0.80 mol of I, and 1.7 mol of HI. The following reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) The equilibrium constant K for this reaction is 0.600 at the temperature of the flask. Calculate the equilibrium molarity of I2. Round your answer to two decimal places. M X

Suppose a 500. mL flask is filled with 0.10 mol of O, and 1.6 mol of NO. The following reaction becomes possible: N2(g) + 0,(g) =2NO (g) The equilibrium constant K for this reaction is 0.679 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. | M

Suppose a 250. mL flask is filled with 1.4 mol of CO, 1.9 mol of H₂O and 1.0 mol of CO₂. The following reaction becomes possible: CO(g) + H₂O(g) + CO₂(g) + H₂(g) 2 The equilibrium constant K for this reaction is 9.28 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X Ś ?

Consider the following reaction: N2 (g)  +  O2 (g) → 2 NO (g), Kc = 0.25 You start the reaction with 14.72 moles of NO (nitrogen monoxide) in a 2.0 L vessel. Calculate the concentration of O2 (in molarity) at equilibrium. (You do not need to solve a quadratic equation to solve this problem.)