Consider the following reaction: 2 A2 (g) + 2 BC (g) ⇄ 2 A2C (g) + B2(g)     A 0.93 L reaction container initially has 0.033 mol A2 and 0.106 mol BC. At equilibrium, the concentration of A2 in the container is 0.008 M. What is the equilibrium concentration of B2? Report your answer with four decimals.

Consider this reaction equation: A2B(g)= 2 A(g) + B(g) If you start with 1.2 M A2B, and if at equilibrium, 50% of it has decomposed, what are the equilibrium concentrations of A and B? What is the value of the equilibrium constant?

At a particular temperature, the equilibrium amounts of hydrogen, iodine and hydrogen iodide present in a 4.00 L flask are found to be: 0.25 moles of hydrogen gas, 0.15 moles of iodine gas and 1.37 moles of hydrogen iodide gas. H2(g) + I2(g)  ↔  2 HI(g) Calculate the equilibrium constant, Kc, value for the reaction.

At a certain temperature, the reaction 2HF(g) H2lg) + F2lg) has K; = 1.2 × 1013. Does this reaction proceed far towards completion when equilibrium is reached? If 0.010 mol HF was placed in a 1.00 L container, and permitted to come to equilibrium, what would be the concentration of H2 and F2 in the container? Concentration of F2 at equilibrium - i M Concentration of H2 at equilibrium - i M

In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H₂O (g) = CO₂ (g) + H₂ (g) In an experiment, 0.35 mol of CO and 0.40 mol of H₂O were placed in a 1.00 L reaction vessel. At equilibrium, there were 0.15 mol of CO remaining. Ke at the temperature of the experiment is Select one: a. Keq = 1.8 b. Keq=1.3 c. Keq=13 d. Keq = 0.75 e. Keq = 0.29

For the equilibrium, 2NO(g)+2H₂(g)→→N₂(g)+2H₂O(g), what will happen if it were in a rigid vessel and argon gas (Ar) were added to the system? Assume temperature remains constant. there will be no change in the equilibrium O the equilibrium will shift toward reactants the equilibrium will be pushed forward there will be a change in the value of the equilibrium constant

The reaction listed below is currently at equilibrium. If you were to suddenly halve the volume of the reaction chamber, what effect would that have on the system? Kr (g) + 2 F2 (3) = KrF4 (s) The reaction will shift to the left in the direction of reactants. O Cannot be determined - The equilibrium concentrations of all species must be provided. The reaction will shift to the right in the direction of products. O The equilibrium constant will increase. O The equilibrium constant will decrease.

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.)

A chemical engineer is studying the following reaction: CH₂(g) + 2H₂S(g) → CS₂(g) + 4H₂(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.7 × 10³. р The engineer charges ("fills") four reaction vessels with methane and hydrogen sulfide, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B compound CH4 H₂S CS₂ H₂ CHA H₂S CS₂ H₂ pressure 5.65 atm 3.56 atm 5.77 atm 7.93 atm 4.69 atm 1.62 atm 6.73 atm 11.81 atm OO expected change in pressure ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase olo ↓decrease ↓decrease ↓ decrease ↓decrease ↓ decrease ↓decrease ↓ decrease ↓ decrease (no change) (no change) (no change) (no change) (no change) (no change) (no change) (no…

Suppose a 250. mL flask is filled with 0.80 mol of H₂O, 0.50 mol of CO₂ and 1.7 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 9.79 at the temperature of the flask. Calculate the equilibrium molarity of CO₂. Round your answer to two decimal places. м X S