Consider the reaction: 2NO(g)+Br2(g)⇌2BrNO(g)K=32.92NO(g)+Br2(g)⇌2BrNO(g) K=32.9 at 315 K In a reaction mixture at equilibrium, the partial pressure of NO is 119 mbarmbar and that of Br2 is 123 mbarmbar .   What is the partial pressure of BrNO in the equilibrium mixture?

For the reaction  2A(g) ⇌ 2B(g) + C(g),  Kc = 1.20 x10−7 at a given temperature.   If the initial concentration of A in a closed container is 0.610 M, what is the approximate equilibrium concentration of B?

Consider the reaction:2NO(g)+Br2(g)⇌2BrNO(g)  K=32.9 at 315 KIn a reaction mixture at equilibrium, the partial pressure of NONO is 119 mbar and that of Br2Br2 is 123 mbar   What is the partial pressure of BrNOBrNO in the equilibrium mixture?

Phosphorus pentachloride is formed when phosphorus trichloride and chlorine react according to the following reaction. PCI2(g) + Cl2(g) ⇌ PCI5(g) The equilibrium constant for the reaction is Kc = 43.7 at 130 °C. If 0.587 mo/ of phosphorus trichloride is added to 0.423 mol of chlorine in a 1.26-L reaction vessel and allowed to react at this temperature, what is the equilibrium concentration (in mol/L) of chlorine? Report your answer to THREE significant figures.

A mixture of ammonia, nitrogen, and hydrogen was allowed to come to equilibrium at 900K. 2NH3 ⇌ 2H2 + N2        Kc = 0.0076. An analysis of the mixture at equilibrium revealed 0.31 M of H2 and 1.8 M of NH3. Determine the equilibrium concentration of N2 (in M) in this mixture. (use 2 significant figures)

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?

In an experiment to study the formation of HI(g),H2(g) + I2(g) ⇌ 2 HI(g)At equilibrium, {H2} = 0.0137, {I2} = 0.0627 and {HI} = 0.0268. Calculate the value of Kc.

At 800 K, the equilibrium constant for the following reaction is Kc=3.1×10−5 I2(g)⇌2I(g) If an equilibrium mixture in a 10.0L vessel contains 2.68×10−2g of I(g), how many grams of I2 are in the mixture?

The equilibrium constant, Kc, for the reaction N2O4(g)⇌2NO2(g) is 5.0×10^-3. If the equilibrium mixture contains [NO2] = 0.055 M , what is the molar concentration of N2O4?

The equilibrium constant, Kc, for the following reaction is 5.10×10-6 at 548 K.NH4Cl(s) NH3(g) + HCl(g)Calculate the equilibrium concentration of HCl when 0.227 moles of NH4Cl(s) are introduced into a 1.00 L vessel at 548 K.[HCl] =  M