General Chemistry
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The reaction PH3BCl3(s) ⇌ PH3(g) + BCl3(g) has Kc = 6.96 × 10–5 at 60 ºC. Determine the value of Kp.
The reaction 2 NO(g) + Br2(g) ⇌ 2 NOBr(g) has Kp = 2.40 at 100 ºC. Determine the value of Kc.
Calculate Kc for each reaction. b. CH4(g) + H2O(g) ⇌ CO(g) + 3 H2(g), Kp = 2.5 x 103 (at 1200 K)
At 63.5 °C, ethanol (CH3CH2OH) has a vapor pressure of 0.526 atm. Determine the Kp and Kc values for the equilibrium CH3CH2OH(l) ⇌ CH3CH2OH(g) at 63.5 °C.
Consider the following equilibrium:
2NO(g) + Br2(g) ⇌ 2NOBr(g)
At 600 K, the partial pressures of the three gases in the equilibrium mixture, NO, Br2, and NOBr, are 0.150 atm, 0.115 atm, and 0.348 atm, respectively.
Determine the value of Kc at this temperature.
Write the expression for the equilibrium constant, Kp, and provide the equation that relates Kp to Kc for the reaction C2H6(g) + Cl2(g) ⇌ C2H5Cl(s) + HCl(g).
Cyclobutane gas decomposes to butene gas when heated.
The equilibrium constant Kc for this reaction is 3.0×104 at 700 K. What is the value of Kp at 700 K?
A hypothetical gas phase reaction C → D has a forward rate constant of 4.22×10−2 s−1. The reverse reaction D → C has a rate constant of 1.74×10−4 s−1. Which component, C or D, has a smaller partial pressure at equilibrium?
When the reaction CH4(g) + H2O(g) ⇌ CO(g) + 3 H2(g) occurs at 1200 K, the Kp = 2.47×103. Calculate the Kc for the reaction at this temperature.
The value of Kc for the following reaction 2 NO2(g) ⇌ N2O4(g) is 4.72 at 100°C. Determine its Kp value at this temperature.
Consider the following diagram of a gas-phase reaction wherein each molecule represents 1.0 mol and a box with a volume of 1.0 L. What is the change in the number of gas molecules (Δn) as a result of the reaction?
What is the change in the number of gas moles (Δn) for each of the following reactions?
I) H2(g) + Br2(l) → 2HBr(g)
II) (NH4)2CO3(s) → 2NH3(g) + CO2(g) + H2O(g)
III) 3H2(g) + N2(g) → 2NH3(g)
IV) Mg(s) + I2(s) → MgI2(s)