At a particular temperature, 12.0 moles of SO3 is placed into a 3.0-L rigid container, and the SO3 dissociates by the reaction 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) At equilibrium. 3.0 moles of SO2 is present Calculate K for this reaction.

Gaseous ammonia was introduced into a sealed container and heated to a certain temperature: 2 NH3(g) ⇌ N2(g) + 3 H2(g) At equilibrium, [NH3] = 0.0238 M, [N2] = 0.117 M, and [H2] = 0.347 M. Calculate Kc for the reaction at this temperature.

Calculate the value of K for the following reaction if the equilibrium concentrations are: [N2] = 0.600 M, [H2] = 0.600 M, and [NH3] = 1.25 M. N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g)

Sulfuryl chloride, SO2Cl2 , is a compound with very irritating vapors; it is used as a reagent in the synthesis of organic compounds. When heated to a sufficiently high temperature, it decomposes to SO2 and Cl2 .   An 1.00-L flask containing 4.93 g of SO2Cl2 is heated to 375 °C. What is the concentration of SO2Cl2 in the system when equilibrium is achieved?

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g) + 2B(g)↽−−⇀4C(g)   ?c=2.13×10^25 If, at this temperature, 2.30mol of A and 3.60mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A]=                                                             M   [B]=                                                             M   [C]=                                                             M

The equilibrium constant K = 53.09 for H2(g) +12(g) 2 HI(g) has been determined at a certain temperature. If 1.00 mol each of H2 and 12 is placed in a 0.500-L flask at that temperature, what are the concentrations of H2, 12, and HI when equilibrium has been achieved? [H₂]= M [12]= M [H0] => M

A student ran the following reaction in the laboratory at 672 K: 2NH3(g)     N2(g) + 3H2(g) When she introduced 6.42×10-2 moles of NH3(g) into a 1.00 Liter container, she found the equilibrium concentration of H2(g) to be 9.09×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

Initially, 0.280 mol of A is present in a 5.00 L solution (no other compounds are present). 2A(aq) ⇌ 2B(aq) + C(aq) At equilibrium, 0.200 mol of C is present. Assume the solution volume doesn't change during the reaction. Calculate K.

For the reaction 2CO2 (g) ⇌ 2CO (g) + O2 (g), Kc = 6.4 x 10-7. If 1.0 x 10-3 moles of CO2 is placed in a 1.0 liter vessel, what are the concentrations of all species at equilibrium?

A 10.0 L reaction vessel at 489°C contained 0.100 mol H2, 0.361 mol I2, and 1.27 mol HI. Assuming that the substances are at equilibrium, find the value of K. at 489°C for the reaction of hydrogen and iodine to give hydrogen iodide. The equation is H2 (g) + I2 (9) = 2HI(9) K. =