At 333 K, this reaction has a K. value of 0.0790. 2 X(g) + 3 Y(g) 2Z(g) Calculate K, at 333 K. Note that the pressure is in units of atmosphere (atm). K, =

The equilibrium constant, K., is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation K₂ = K. (RT)An where R = 0.08206 L-atm/(K-mol), T is the absolute temperature, and An is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N₂(g) + 3H₂(g) = 2NH3(g) for which An=2-(1+3) = -2.

Be sure to answer all parts. The equilibrium constant K, for the reaction I(g) 5 21(g) is 3.75 x 10 at 726°C. Calculate K, and Kp for the equilibrium 21(g) S1(g) at the same temperature. K.= X 10 %3D (Enter your answer in scientific notation.) Kp = %3D

The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl₂(g) 80 F3 [CO] [Cl₂] Calculate the equilibrium concentrations of reactant and products when 0.245 moles of Co and 0.245 moles of Cl₂ are introduced into a 1.00 L vessel at 600 K. = [COCI₂] = = $ 4 Use the References to access important values if needed for this question. Submit Answer NOV 30 Q ? An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer. F4 CoCl₂(g). % 5 M M M Retry Entire Group 16 F5 tv ♫ 9 A 6 9 more group attempts remaining MacBook Air C F6 & 7 F7 * 8 DII F8 9 Previous Email Instructor F9 ) - O Next Save and Exit 4 F10 I