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Chapter 13: Q82E (page 760)

Question: Calculate the equilibrium concentrations that result when 0.25 M O2 and 1.0 M HCl react and come to equilibrium.

Short Answer

Expert verified

The equilibrium concentration is

Step by step solution

01

Determine change in concentration:

Given information:


  • The concentration of O2 is 0.25M
  • The concentration of HCL is 1.0M
  • The equilibrium constant is

We have to find the equilibrium concentrations.

Sinceis large, we will assume that the reaction goes to completion and then comes back to equilibrium.

We will assume that the volume of a solution is 1 L, hence the number of moles of O2 is 0.25 mol and the number of moles of HCL is 1.0 mol

Since 4 moles of HCL reacts with 1 mole of O2, to produce 2 moles of Cl2 and 2 moles of H2O 1.0 mole of HCL will react with 0.25 mole of O2, and produce 0.50 moles of Cl2 (0.50 M) and 0.50 moles of H20 (0.50 M)

We have to determine the value of x,

Since is too large, we will neglect the change in concentration of Cl2, and H2O, and get

02

Determine equilibrium concentration of all species:

The change in the concentration obtained

Therefore, the equilibrium concentrations are

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Most popular questions from this chapter

Assume that the change in pressure of \({H_2}S\) is small enough to be neglected in the following problem.(a) Calculate the equilibrium pressures of all species in an equilibrium mixture that results from the decomposition of H2S with an initial pressure of 0.824 atm.

\(2{H_2}S(g) \rightleftharpoons 2{H_2}(g) + {S_2}(g)\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,{K_p} = 2.2 \times {10^{( - 6)}}\)

(b) Show that the change is small enough to be neglected.

Question: A 1.00-L vessel at 400 掳C contains the following equilibrium concentrations: N2, 1.00M; H2, 0.50M; and NH3, 0.25M. How many moles of hydrogen must be removed from the vessel to increase the concentration of nitrogen to 1.1M?

Question: Butane exists as two isomers, n鈭抌utane and isobutane.

\({K_P} = 2.5\;at\;2{5^o}C\)

What is the pressure of isobutane in a container of the two isomers at equilibrium with a total pressure of 1.22 atm?

The following reaction has \({K_P} = 4.50 \times {10^{ - 5}}\) at \(720\;{\rm{K}}\).

\({{\rm{N}}_2}(g) + 3{{\rm{H}}_2}(g) \rightleftharpoons 2{\rm{N}}{{\rm{H}}_3}(g)\)

If a reaction vessel is filled with each gas to the partial pressures listed, in which direction will it shift to reach equilibrium?

\(P\left( {{\rm{N}}{{\rm{H}}_3}} \right) = 93\;{\rm{atm}},\;P\left( {\;{{\rm{N}}_2}} \right) = 48\;{\rm{atm}},\;{\rm{and}}\;P\left( {{{\rm{H}}_2}} \right) = 52\)

A sample of ammonium chloride was heated in a closed container. NH4 Cl (s)鈬� NH3 (g) + HCl(g)at equilibrium, the pressure of NH3 (g)was found to be 1.75 atm. What is the value of the equilibrium constant, Kp, for the decomposition at this temperature?
See all solutions

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