SO2Cl2(g) SO2(g) + Cl2(g) 3. A 4.32 g sample of liquid SO,Cl₂ is placed in a rigid, evacuated (1.50 L reaction vessel. As the container is heated to 400. K, the sample vaporizes completely and starts to decompose-according to the equation above. The decomposition reaction is endothermic. (a) If no decomposition occurred, what would be the pressure, in atm, of the SO₂Ch(g) in the vessel at 400. K? (b) When the system has reached equilibrium at 400. K, the total pressure in the container is 1.26 atm. Calculate the partial pressures, in atm, of SO₂Cl2(g), SO2(g), and Cl₂(g) in the container at 400. K. (c) For the decomposition reaction at 400. K, (d) (i) write the equilibrium-constant expression for Kp for the reaction, and (ii) calculate the value of the equilibrium constant, Kp. (d) The temperature of the equilibrium mixture is increased to 425 K. Will the value of K, increase, decrease, or remain the same? Justify your prediction. ✓ie) In another experiment, the original partial pressures of SO-Cl(g). SO(g), and Clg) are atm each at 400. K. Predict whether the amount of SO,Cl(g) in the container will increase, decrease, or remain the same. Justify your prediction.
SO2Cl2(g) SO2(g) + Cl2(g) 3. A 4.32 g sample of liquid SO,Cl₂ is placed in a rigid, evacuated (1.50 L reaction vessel. As the container is heated to 400. K, the sample vaporizes completely and starts to decompose-according to the equation above. The decomposition reaction is endothermic. (a) If no decomposition occurred, what would be the pressure, in atm, of the SO₂Ch(g) in the vessel at 400. K? (b) When the system has reached equilibrium at 400. K, the total pressure in the container is 1.26 atm. Calculate the partial pressures, in atm, of SO₂Cl2(g), SO2(g), and Cl₂(g) in the container at 400. K. (c) For the decomposition reaction at 400. K, (d) (i) write the equilibrium-constant expression for Kp for the reaction, and (ii) calculate the value of the equilibrium constant, Kp. (d) The temperature of the equilibrium mixture is increased to 425 K. Will the value of K, increase, decrease, or remain the same? Justify your prediction. ✓ie) In another experiment, the original partial pressures of SO-Cl(g). SO(g), and Clg) are atm each at 400. K. Predict whether the amount of SO,Cl(g) in the container will increase, decrease, or remain the same. Justify your prediction.
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Chapter6: Thermochemisty
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Problem 6.27QP: Hypothetical elements A2 and B2 react according to the following equation, forming the compound AB....
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Transcribed Image Text:SO2Cl2(g) SO2(g) + Cl2(g)
3. A 4.32 g sample of liquid SO,Cl₂ is placed in a rigid, evacuated (1.50 L reaction vessel. As the container is
heated to 400. K, the sample vaporizes completely and starts to decompose-according to the equation above.
The decomposition reaction is endothermic.
(a) If no decomposition occurred, what would be the pressure, in atm, of the SO₂Ch(g) in the vessel at 400. K?
(b) When the system has reached equilibrium at 400. K, the total pressure in the container is 1.26 atm.
Calculate the partial pressures, in atm, of SO₂Cl2(g), SO2(g), and Cl₂(g) in the container at 400. K.
(c) For the decomposition reaction at 400. K,
(d)
(i) write the equilibrium-constant expression for Kp for the reaction, and
(ii) calculate the value of the equilibrium constant, Kp.
(d) The temperature of the equilibrium mixture is increased to 425 K. Will the value of K, increase, decrease,
or remain the same? Justify your prediction.
✓ie) In another experiment, the original partial pressures of SO-Cl(g). SO(g), and Clg) are atm each at
400. K. Predict whether the amount of SO,Cl(g) in the container will increase, decrease, or remain the
same. Justify your prediction.
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