The water–gas shift reaction is important in several chemical processes, such as the production of H2 for fuel cells. This reaction can be written as follows: H2(g) + CO2(g) ⇌ H2O(g) + CO(g) with K = 0.106 at 700 K. If a mixture of gases that initially contains 0.632 M CO2 and 0.570 M H2 is allowed to equilibrate at 700 K, what is the final concentrations of CO?

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)

The water–gas shift reaction is important in several chemical processes, such as the production of H2 for fuel cells. This reaction can be written as follows:   H2(g) + CO2(g) ⇌ H2O(g) + CO(g)   with K = 0.106 at 700 K. If a mixture of gases that initially contains 0.632 M CO2 and 0.570 M H2 is allowed to equilibrate at 700 K, what is the final concentration of CO?   0.257   0.366   0.148   0.475

The value of Kc for the reaction between water vapor and dichlorine monoxide, H2O (g) + Cl2O (g) --> 2 HOCl (g) is 0.0900 at 25°C.  Determine the equilibrium concentrations of all three compounds if the starting concentrations of both reactants are 0.00432 M and no HOCl is present.

The equilibrium constant of the reaction 2C02 = 2C0+02 is 1.08. If the concentrations of CO and O2 is 0.86 M and 0.54 M, respectively, what is the concentration of carbon dioxide?

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. =

A student ran the following reaction in the laboratory at 227 K: 2NOBr=NOBr+Br2 When she introduced 0.175 moles of NOBr into a 1.00 liter container, she found the equilibrium concentration of NOBr to be 0.140 M. Calculate the equilibrium constant, kc , she obtained for this reaction.

[References] [Review Topics] Use the References to access important values if needed for this question. The equilibrium constant, K, for the following reaction is 5.10x10-6 at 548 K. NH3(g) + HCI(g) NHẠCI(s) HCI. If the 2.26×103 M NH3 and 2.26x10 M An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.242 mol NH,Cl, concentration of HCI(g) is suddenly increased to 3.46x103 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = [НC] Submit Answer Retry Entire Group 7 more group attempts remaining Previous Next Save and Ex