Chapter 6: Q80. (page 196)
At 25oC, gaseous SO2Cl2 decomposes to SO2(g) and Cl2(g) to the extent that 12.5% of the original SO2Cl2 (by moles) has decomposed to reach equilibrium. The total pressure (at equilibrium) is 0.900 atm. Calculate the value of Kp for this system.
The value of Kp for this system is.
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Question: Old-fashioned “smelling salts” consist of ammonium carbonate [(NH4)2CO3]. The reaction for the decomposition of ammonium carbonate
is endothermic. Would the smell of ammonia increase or decrease as the temperature is increased?
At 4500C, Kp =6.5 x 10-3 for the ammonia synthesis reaction. Assume that a reaction vessel with a movable piston initially contains 3.0 moles of H2(g) and 1.0 moles of N2(g). Make a plot to show how the partial pressure of NH3(g) present at equilibrium varies for the total pressures of 1.0 atm, 10.0 atm, and 100. atm, and 1000. atm (assuming that Kp remains constant). [Note: Assume these total pressures represent the initial total pressure of H2(g) plus N2(g), where PNH3 = 0.]
GIVEN: Kp = 6.5 X 10-3
A type of reaction we will study is that having a very small K value (K << 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be performed. However, the math involved in solving equilibrium problems for reactions having small K values (K << 1) is simplified. What assumption is made when solving equilibrium concentrations for reactions having small K values? Whenever assumptions are made, they must be checked for validity. In general, the “5% rule” is used to check the validity of assuming that x (or 2x, 3x, and so on) is very small compared to some number. When x (or 2x, 3x, and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?
An 8.00-g sample of SO3 was placed in an evacuated container, where it decomposed at 6000C according to the following reaction:
At equilibrium the total pressure and the density of the gaseous mixture were 1.80 atm and 1.60 g/L, respectively. Calculate Kp for this reaction.
A sample of S8(g) is placed in an otherwise empty, rigid container at 1325 K at an initial pressure of 1.00 atm, where it decomposes to S2(g) by the reaction
At equilibrium, the partial pressure of S8 is 0.25 atm.Calculate Kp for this reaction at 1325 K.
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