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Chapter 13: Q58 E (page 717)

When heated, iodine vapor dissociates according to this equation: I2 (g) 鈬� 2I (g). At 1274K a sample exhibits a partial pressure of I2 of 0.1122 and a partial pressure due to I atoms of 0.1378 atm. Determine the value of the equilibrium constant, Kp for the decomposition at 1274K

Short Answer

Expert verified

The value of equilibrium constant Kp=0.17.

Step by step solution

01

Define the Equilibrium constant

The Definition of equilibrium constant: a number that expresses the relationship between the amounts of products and reactants present at equilibrium in a reversible chemical reaction at a given temperature

02

Calculation of equilibrium constant

The need to calculate the equilibrium constant Kp for this reaction:

I2 (g)鈬� 2I (g).

We calculate the value Kp

\({K_p} = \frac{{p(I)_{eq}^2}}{{p{{\left( {{I_2}} \right)}_{eq}}}}\)

03

The equilibrium constant of the compound

The peq is equilibrium pressure of the compound. We are given all the data in the task:

\begin{aligned}{p{{(I)}_{eq}}=0.1378{\rm{atm}}}\\{p{{\left({{I_2}}\right)}_{eq}}=0.1122{\rm{atm}}}\end{aligned}

We calculate Kp

\begin{aligned}{{K_p}=\frac{{{{0.1378}^2}}}{{0.1122}}}\\{{K_p}=0.17}\end{aligned}

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Most popular questions from this chapter

The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction) in which each system will proceed to leach equilibrium.

Question: Consider the equilibrium

4NO2(g) + 6H2 O(g) 鈬� 4NH3(g) + 7O2(g)

(a) What is the expression for the equilibrium constant (Kc) of the reaction?

(b) How must the concentration of NH3 change to reach equilibrium if the reaction quotient is less than the equilibrium constant?

(c) If the reaction were at equilibrium, how would a decrease in pressure (from an increase in the volume of the reaction vessel) affect the pressure of NO2?

(d) If the change in the pressure of NO2 is 28 torr as a mixture of the four gases reaches equilibrium, how much will the pressure of O2 change?

Question: The binding of oxygen by hemoglobin (Hb), giving oxyhemoglobin (HbO2), is partially regulated by the concentration of H3O+ and dissolved CO2 in the blood. Although the equilibrium is complicated, it can be summarized as

HbO2(aq) + H3 O+(aq) + CO2(g) 鈬� CO2 鈭扝产鈭扝+ + O2(g) + H2 O(l)

(a) Write the equilibrium constant expression for this reaction.

(b) Explain why the production of lactic acid and CO2 in a muscle during exertion stimulates release of O2 from the oxyhemoglobin in the blood passing through the muscle.

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.

What is the approximate value of the equilibrium constant KP for the change C2H5OC2H5 (濒)鈬孋2 H5OC2H5 (g) at 25 掳C.

(Vapor pressure was described in the previous chapter on liquids and solids; refer back to this chapter to find the relevant information needed to solve this problem.)
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