Consider the following reaction where Kp = 2.01 at 500 K:
PCl3(g) + Cl2(g) -> PCl5(g)
If the three gases are mixed in a rigid container at 500 K so that the partial pressure of each gas is initially one atm, what will happen?
Indicate True (T) or False (F) for each of the following:
1. A reaction will occur in which PCl5(g) is produced.
2. Kp will decrease.
3. A reaction will occur in which PCl3 is produced.
4. Q is greater than K.
5. The reaction is at equilibrium. No further reaction will occur.
Consider the following reaction where Kc = 1.80×10-2 at 698 K:
2 HI (g) -> H2 (g) + I2 (g)
A reaction mixture was found to contain 0.278 moles of HI (g), 4.10×10-2 moles of H2 (g), and 4.37×10-2 moles of I2 (g), in a 1.00 liter container.
Indicate True (T) or False (F) for each of the following:
1. In order to reach equilibrium HI(g) must be consumed.
2. In order to reach equilibrium Kc must increase.
3. In order to reach equilibrium H2 must be consumed.
4. Qc is greater than Kc.
5. The reaction is at equilibrium. No further reaction will occur.
Consider the following reaction where Kc = 83.3 at 500 K:
PCl3(g) + Cl2(g) -> PCl5(g)
A reaction mixture was found to contain 2.58×10-2 moles of PCl3(g), 4.24×10-2 moles of Cl2(g), and 0.117 moles of PCl5(g), in a 1.00 Liter container.
Indicate True (T) or False (F) for each of the following:
1. In order to reach equilibrium PCl5(g) must be produced.
2. In order to reach equilibrium Kc must decrease.
3. In order to reach equilibrium PCl3 must be consumed.
4. Qc is less than Kc.
5. The reaction is at equilibrium. No further reaction will occur.