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03:20
07:32 03:20At 700 K, the equilibrium constant for the reaction CCl4(𝑔) ⇌ C(𝑠) + 2 Cl2(𝑔) is 𝐾𝑝 = 0.76. A flask is charged with 2.00 atm of CCl4, which then reaches equilibrium at 700 K. (b) What are the partial pressures of CCl4 and Cl2 at equilibrium?
Consider the hypothetical reaction A(𝑔) + 2 B(𝑔) ⇌ 2 C(𝑔), for which 𝐾𝑐 = 0.25 at a certain temperature. A 1.00-L reaction vessel is loaded with 1.00 mol of compound C, which is allowed to reach equilibrium. Let the variable x represent the number of mol/L of compound A present at equilibrium. (e) From the plot in part (d), estimate the equilibrium concentrations of A, B, and C. (Hint: You can check the accuracy of your answer by substituting these concentrations into the equilibrium expression.)
At a temperature of 700 K, the forward and reverse rate constants for the reaction 2 HI(𝑔) ⇌ H2(𝑔) + I2(𝑔) are 𝑘𝑓=1.8×10−3 𝑀−1s−1 and 𝑘𝑟 = 0.063 𝑀−1s−1. (b) Is the forward reaction endothermic or exothermic if the rate constants for the same reaction have values of 𝑘𝑓 = 0.097 𝑀−1s−1 and 𝑘𝑟 = 2.6 𝑀−1s−1 at 800 K?
The following equilibria were measured at 823 K: CoO1s2 + H21g2 ΔCo1s2 + H2O1g2 Kc = 67 H21g2 + CO21g2 ΔCO1g2 + H2O1g2 Kc = 0.14 (d) If the reaction vessel from part (c) is heated to 823 K and allowed to come to equilibrium, how much CoO1s2 remains?
The phase diagram for SO2 is shown here. (d) At which of the three points marked in red does SO2(g) most closely approach ideal-gas behavior?
The phase diagram for SO2 is shown here. (e) At which of the three red points does SO2(g) behave least ideally?
