The equilibrium constant for the reaction 2HBr(g) ⇌  H2(g) + Br2(g) is a 10 at a certain temperature, when concentrations are exprssed in moles per liter. Calculate the number of moles of HBr(g), present at equilibruim if 100L of the equiliburim mixture contaon 5 mol of H2(g) and 8mol of Br2(g).  The answer is 2

Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.23-L flask at a certain temperature initially contains 27.3 g CO and 2.33 g H2. At equilibrium, the flask contains 8.63 g CH3OH. Part ACalculate the equilibrium constant  (Kc)   for the reaction at this temperature.

-2 The equilibrium constant K,, for the following reaction is 7.73×10atmat 350°C. What is the value of K. for the reaction at the same temperature? N2(g) +3H2(g)→ 2NH3(g)

Consider the following reaction and associated equilibrium constant at 430 K. 12 (g) + Br2 (g ) ⇌ 2 IBr (g) Kc = 278 If the reaction begins with 0.250 mol of IBr in a 2.00 L flask, calculate the concentration (mol/L) of IBr at equilibrium. Enter your answer with no units. Do not give handwriting solution.

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?

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?

Water gas is a 1:1 mixture of carbon monoxide and hydrogen gas and is called water gas because it is formed from steam and hot carbon in the following reaction: H2 O(g) + C(s) ⇌ H2(g) + CO(g). Methanol, a liquid fuel that could possibly replace gasoline, can be prepared from water gas and hydrogen at high temperature and pressure in the presence of a suitable catalyst.(a) Write the expression for the equilibrium constant (Kc) for the reversible reaction2H2(g) + CO(g) ⇌ CH3 OH(g)                                ΔH = −90.2 kJ(b) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if more H2 is added?(c) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CO is removed?(d) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CH3OH is added?(e) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if the temperature of the system is increased?(f) What will happen to the concentrations of H2, CO,…

In an experiment, 0.37 mol H2 and 0.37 mol Br2 are mixed in a 1.00-L container (without any product initially), and the reaction forms HBr. Br2 (g) + H2 (g) ⇌ 2 HBr (g). If Kc = 64 for this reaction, determine the equilibrium concentration of HBr with 2 SIGNIFICANT FIGURES.

Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. = 1.80 at 250 °C A 0.3668 mol sample of PCI, (g) is injected into an empty 4.30 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCI, (g) at equilibrium. [PCl,] = M [PCI,] = M

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