The equilibrium constant for the reaction 2HI (g) ⇌ H2 (g) + I2 (g) is 115. If 2.7 mol HI is put into a 1.00 L flask, what will be the concentration of H2 at equilibrium? Report your answer to two significant figures.

Consider the following equilibrium system at 355 K. 2NOBr(g) -----> 2NO(g)+Br2(g). If an equilibrium mixture of the three gases at 355 K contains 3.21x10^-2 M NOBr, 2.01x10^-2 M NO,and 3.98x10^-2 M Br2 what is the value of the equilibrium constant K

At a certain temperature, the equilibrium constant K for the following reaction is 0.71: N2(g) + O2(g) =2 NO(g) Use this information to complete the following table. Suppose a 43. L reaction vessel is filled with 1.0 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little N2 and 02. There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K =0 2 NO(g) N,(9)+O2(9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = 3 N2(9)+30,(9) 6 NO(g)

General Chemistry 4th Edition McQuarrie Rock Gallogly University Science Books presented by Macmillan Learning For the chemical equation SO, (g) + NO, (g) = SO,(g) + NO(g) the equilibrium constant at a certain temperature is 2.10. At this temperature, calculate the number of moles of NO, (g) that must be added to 2.64 mol SO, (g) in order to form 1.20 mol SO, (g) at equilibrium. 3 moles of NO,(g): mol 2. Question Source: MRG - General Chemistry | Publish privacy policy | help terms of use contact us about us careers (? ^ N EV prime video W