Consider the following reaction: Si(s) + 2Cl2(g) ↔ SiCl4(g) When the reaction is started with 0.75...

Consider the following reaction: Si(s) + 2Cl2(g) ↔ SiCl4(g) When the reaction is started with 0.75 moles of Si and 0.20 moles of Cl2 in a one liter flask, 0.050 moles of SiCl4 are obtained at equilibrium. Calculate the equilibrium constant, Kc.

Expert Solution

queen_honey_blossom answered 1 year ago

Consider the following reaction at 0ºC: S(s) + 4NO(g) ↔ SO2(g) + 2N2O(g). A student places...

Consider the following reaction at 0ºC: S(s) + 4NO(g) ↔ SO2(g) + 2N2O(g). A student places 0.025 moles of solid sulfur and 0.100 moles of nitrogen monoxide gas in a closed 1.00 L container at 0ºC for several days. Calculate the number of molecules of NO in the 1.00L container after equilibrium is reached, given the following thermodynamic data: S(s) NO(g) SO2(g) N2O(g) 31.9 211 256 220 Sº (J K-1 mol-1) 0.00 90.4 -297 81.6 ΔHºf(kJ mol-1) My...

Consider the following reaction which is at equilibrium at 100°C: A(g) + B(g) ↔ AB (g)...

Consider the following reaction which is at equilibrium at 100°C: A(g) + B(g) ↔ AB (g) ΔH=420 kJ/mol Predict the direction where the reaction would proceed, and explain your reasoning: a. The reaction vessel were pressurized to 5atm with helium b. The temperature were increased to 200°C c. The reaction were coupled with another reaction: AB + D2 → AD + BD d. The volume of the reaction vessel were increased from 2.0L to 5.0L without removing any gas e....

Consider the following reaction: S↔P where the rate constant for the forward reaction is k1, and...

Consider the following reaction: S↔P where the rate constant for the forward reaction is k1, and the rate constant for the reverse reaction is k2, and Keq= [P]/[S] Which of the following would be affected by an enzyme? Please answer yes or no and give a short explanation (5-20 words maximally) a) decreased Keq b) increased k1 c) increased Keq d) increased Δ G# e) decreased Δ G# f) increased k2 g) more negative Δ G0

For the reaction 4HCl(g) + O2(g)2H2O(g) + 2Cl2(g) H° = -114.4 kJ and S° = -128.9...

For the reaction 4HCl(g) + O2(g)2H2O(g) + 2Cl2(g) H° = -114.4 kJ and S° = -128.9 J/K The maximum amount of work that could be done when 2.05 moles of HCl(g) react at 308 K, 1 atm is kJ. Assume that H° and S° are independent of temperature.

The equilibrium constant for the reaction CCl4(g) = C(s) + 2Cl2(g) at 700ºC is 0.85. Determine the...

The equilibrium constant for the reaction CCl4(g) = C(s) + 2Cl2(g) at 700ºC is 0.85. Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 2.30 atm at 700ºC.

Consider the reaction: I2(g) + Cl2(g) ↔ 2 ICl (g) Calculate ΔGrxnfor the reaction at 25oC...

Consider the reaction: I2(g) + Cl2(g) ↔ 2 ICl (g) Calculate ΔGrxnfor the reaction at 25oC under each of the following conditions: a. Standard conditions b. At equilibrium c. PICl= 2.55 atm; PI2= 0.325 atm; PCl2= 0.221 atm

Consider the following reversible Hetererogenes reaction: C(s) + CO2(g) -><- 2CO(g) When equalibrium is reached at...

Consider the following reversible Hetererogenes reaction: C(s) + CO2(g) -><- 2CO(g) When equalibrium is reached at a certain point the total pressure of the system is found to be 4.98 atm. If the equilibrium constant Kp for this reaction is equal to 1.67 at this temperature, calculate the equilibrium partial pressures of CO2 and CO gases? P(CO)eq= ? P(CO2)eq=?

Express the equilibrium constant for the following reaction. 10PCl5(g) ↔ 10PCl3(g) + 10Cl2(g)

1. Given the following: C(s) + 2H2(g) → CH4(g) ΔH= −74.6 kJ C(s) + 2Cl2(g)...

1. Given the following: C(s) + 2H2(g) → CH4(g) ΔH= −74.6 kJ C(s) + 2Cl2(g) → CCl4(g) ΔH= −95.7 kJ H2(g) + Cl2(g) → 2HCl(g) ΔH= −184.6 kJ Calculate the enthalpy of reaction for: CH4(g) + 4Cl2(g) → CCl4(g) + 4HCl(g) 2. There was a lot of talk among football fans about "deflate-gate" last week (hopefully it's not still going on this week) where the New England Patriots grounds crew seem to have decreased the pressure...

For the following reaction, Kc = 481 at 1000 K. CO (g) + Cl2 (g) ↔...

For the following reaction, Kc = 481 at 1000 K. CO (g) + Cl2 (g) ↔ COCl2 (g) If the reaction mixture initially contains a CO concentration of 0.2500 M and a Cl2 concentration of 0.185 M at 1000 K, what are the equilibrium concentrations of CO, Cl2, and COCl2 at 1000K

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