The equilibrium constant, kc, for the reaction below is 0.10 at 25°c. 2ICl(g)=Cl2(g)+I2(g) Find the equilibrium concentration for chlorine gas, Cl2(g), if the equilibrium concentrations of ICl(g) and I2(g) are known to be 0.50 M and 0.40 M respectively.

The equilibrium constant, K, for the following reaction is 6.59×10-2 at 546 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 6.59 L container at 546 K contains 0.254 M PCl5,   0.129 M PCl3 and 0.129 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 11.7 L? [PCl5] =  M [PCl3] =  M [Cl2] =  M

A mixture of 0.578 moles of carbon monoxide and 0.443 moles of oxygen was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium at a certain temperature. The equilibrium concentration of CO2 was 0.239 M. What is the value of Ke for this reaction at this particular temperature? CO(g) + O2(g) = CO2(g) Report your answer to three significant figures and do not include units.

The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2(g)+I2(g) <-----> 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.301 moles of H2 and 0.301 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] =       M [I2]   =     M [HI] =        M

Calculate the equilibrium concentrations for all reactants and products if initial concentrations of CH4 is 0.400 M, H2S is 0.800 M, CS2 is 0.400 M, H2 is 0.800 M are mixed and allowed to establish equilibrium.  The Kc for the reaction is 0.0360 and the equilibrium concentration of CH4is 0.556 M.   CH4(g) + 2H2S(g) ↔  CS2(g) + 4H2(g) Group of answer choices [CH4] = 0.556 M, [H2S] = 0.488 M, [CS2] = 0.556 M, [H2] = 1.42 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.244 M, [H2] = 0.176 M. [CH4] = 0.556 M, [H2S] = 0.244 M, [CS2] = 0.956 M, [H2] = 1.36 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.556 M, [H2] = 1.42 M.

The following reaction has an equilibrium constant, Kc equal to 3.59 at 900 °C. CH4(g) + 2H₂S(g) — CS2(g) + 4 H2(g) At a particular time during the reaction, the following composition has been found: [CH4(g)] = 1.20 M, [CS2(g)] = 1.15 M, [H₂S(g)] = 1.31 M, [H2(g)] = 1.85. Predict the activity of the reaction during the particular time above. The reaction should go to the left (or reverse) The reaction should go to the right (or forward) The reaction is at a standstill The reaction activity cannot be determined There is no basis for prediction.

The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K.PCl5(g) PCl3(g) + Cl2(g)Calculate the equilibrium concentrations of reactant and products when 0.246 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K. [PCl5] =  M [PCl3] =  M [Cl2] =  M

The equilibrium constant, Kc, for the following reaction is 0.00650 at 298 K. 2NOBr(g) ⇒ 2NO(g) + Br₂ (g) If an equilibrium mixture of the three gases in a 15.6 L container at 298 K contains 0.201 mol of NOBr(g) and 0.284 mol of NO, the equilibrium concentration of Br₂ is | M.

N2(g) and O2(g) can exist in equilibrium with NO(g), as shown below. The equilibrium constant at 25.0°C is 4.8 x 10-31. If initially there are 1.35 mol of nitrogen and 0.60 mol of oxygen in a 2.00 L vessel, find the equilibrium concentrations of each species. N2(g) + O2(g) → 2NO(g)

A student ran the following reaction in the laboratory at 282 K: 2CH2C12(g)=CH4(g)+ CCI4(g) When she introduced 6.98x102 moles of CH,Ch(g) into a 1.00 liter container, she found the equilibrium concentration of CH,Cl2(g) to be 4.62x10³ M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =