Skip to main content
Pearson+ LogoPearson+ Logo
Ch.15 - Chemical Equilibrium
Back
Previous problem
Next problem
All textbooksBrown 15th EditionCh.15 - Chemical EquilibriumProblem 34a

Chapter 15, Problem 34a

Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas: PCl3(𝑔) + Cl2(𝑔) β‡Œ PCl5(𝑔). A 7.5-L gas vessel is charged with a mixture of PCl3(𝑔) and Cl2(𝑔), which is allowed to equilibrate at 450 K. At equilibrium the partial pressures of the three gases are 𝑃PCl3 = 0.124 atm, 𝑃Cl2 = 0.157 atm, and 𝑃PCl5 = 1.30 atm. (a) What is the value of 𝐾𝑝 at this temperature?

Verified Solution
Video duration:
2m
This video solution was recommended by our tutors as helpful for the problem above.
1357
views
Was this helpful?

Video transcript

hi everyone. So we may have sulfur dioxide gas reacting with oxygen gas to produce sulfur oxide. We have a 5.5 liter reaction vessel that's charged with the mixture of sulfur dioxide and oxygen gas at 300 degrees Celsius. When the equilibrium was established to make sure that the three gasses that these partial pressures for the partial pressure of sulfur dioxide. We have 1.15 atmosphere for the partial pressure of oxygen gas. We have 2.35 atmosphere for the partial pressure of sulfur trioxide. We have 0.855 atmosphere. Who asked to determine the K. P. Just for us to find the K. P. When we're giving the partial pressure of the gas is we need to look at the K. P. Expression for the reaction we call that the K. P. Expression is the partial pressure of the products raised to the power of the coefficient provided by the pressure pressure of the reactant. Right to the power of the coefficient. So for this reaction we have K. P. Because the partial pressure of sulfur trioxide raise to the power of two because we have two moles of sulfur dioxide in the reaction divided by the partial pressure of sulfur dioxide. The power of two because we have two moles of sulfur dioxide and the reaction pressure pressure of 02. For the power of one. For the partial pressure of sulfur trioxide, We have 0.855 atmosphere for the partial pressure of sulfur dioxide. We have 1.15 atmosphere for the partial pressure of oxygen gas, We have 2.35 atmosphere. If we plug in the values for K. P, We're gonna get 0.855 atmosphere where Divide by 1.15 atmosphere square Times 2.35 atmosphere for K. P. We get 0.235 K. P. Does not have any units. Thanks for watching my video, and I hope it was helpful.
Previous problemNext problem
Related Practice
Textbook Question

Consider the equilibrium N2(𝑔) + O2(𝑔) + Br2(𝑔) β‡Œ 2 NOBr(𝑔) Calculate the equilibrium constant 𝐾𝑝 for this reaction, given the following information at 298 K:

2 NO(𝑔) + Br2(𝑔) β‡Œ 2 NOBr(𝑔) 𝐾𝑐 = 2.02

NO(𝑔) β‡Œ N2(𝑔) + O2(𝑔) 𝐾𝑐 = 2.1Γ—1030

989
views
Textbook Question

The equilibrium 2 NO(𝑔) + Cl2(𝑔) β‡Œ 2 NOCl(𝑔) is established at 500.0 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, Cl2, and NOCl, respectively. (a) Calculate 𝐾𝑝 for this reaction at 500.0 K.

396
views
Textbook Question

The equilibrium 2 NO(𝑔) + Cl2(𝑔) β‡Œ 2 NOCl(𝑔) is established at 500.0 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, Cl2, and NOCl, respectively. (b) If the vessel has a volume of 5.00 L, calculate Kc at this temperature.

932
views
1
comments
Textbook Question

A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium is established at 500 K: CO2(𝑔) + H2(𝑔) β‡Œ CO(𝑔) + H2O (𝑔) (d) Calculate 𝐾𝑐 for the reaction.

1565
views
Textbook Question

Indicate whether each of the following statements about the reaction quotient Q is true or false: (a) The expression for 𝑄𝑐 looks the same as the expression for 𝐾𝑐.

Textbook Question

Indicate whether each of the following statements about the reaction quotient Q is true or false: (b) If 𝑄𝑐 < 𝐾𝑐, the reaction needs to proceed to the right to reach equilibrium.