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Chapter 13: Q87E (page 760)

Question: What is the minimum mass of CaCO3 required to establish equilibrium at a certain temperature in a 6.50-L container if the equilibrium constant (Kc) is 0.050 for the decomposition reaction of CaCO3 at that temperature?

Short Answer

Expert verified

The minimum mass of CaCO3required is 3.25 g.

Step by step solution

01

Determine amount of CO2 required

For the given reaction,

Here \({{\rm{K}}_{\rm{c}}} = \left( {{\rm{C}}{{\rm{O}}_2}} \right) = 0.005{\rm{mo}}{{\rm{l}}^{ - 1}}\)

For 6.5 L container moles of CO2 required is

Moles of CO2=\(6.5 \times 0.005\)

= 0.0325 mole

02

Determine mass of CaCO3 required

Moles of CO2 required =0.0325 mole

Therefore, moles of CaCO3 required = 0.0325 mole

Minimum mass of CaCO3

\(\begin{array}{l} = \,number\,of\,moles\,of\,CaC{O_3} \times \,Molecular\,weight\,of\,CaC{O_3}\\ = 0.0325 \times 100\\ = 3.25\,gm\end{array}\)

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Most popular questions from this chapter

Question: In a 3.0-L vessel, the following equilibrium partial pressures are measured: \({{\rm{N}}_2}\),190 torr;\({{\rm{H}}_2}\), 317 torr;\({\rm{N}}{{\rm{H}}_3}\)\(1.00 \times {10^3}\)torr.

  1. How will the partial pressures of\({{\rm{H}}_2},{{\rm{N}}_2}\)and \({\rm{N}}{{\rm{H}}_3}\)change if \({{\rm{H}}_2}\) is removed from the system? Will they increase, decrease, or remain the same?
  2. Hydrogen is removed from the vessel until the partial pressure of nitrogen, at equilibrium, is 250 torr. Calculate the partial pressures of the other substances under the new conditions.

Calcium chloride 6鈭抙ydrate, \(CaC{l_2}.6{H_2}O\), dehydrates according to the equation

\(CaC{l_2} \times 6{H_2}O(s) \rightleftharpoons CaC{l_2}(s) + 6{H_2}O(g)\)

\({K_P} = 5.09 \times 1{0^{ - 44}}at2{5^o}C\)

What is the pressure of water vapor at equilibrium with a mixture of \(CaC{l_2}.6{H_2}O\)and \(CaC{l_2}\)?

Question: Calculate the number of grams of HI that are at equilibrium with 1.25 mol of H2 and 63.5 g of iodine at 448掳C.

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?

The following equation represents a reversible decomposition:

\({\mathbf{CaC}}{{\mathbf{O}}_3}{\text{ }}\left( {\mathbf{s}} \right) \rightleftharpoons {\mathbf{CaO}}\left( {\mathbf{s}} \right){\text{ }} + {\text{ }}{\mathbf{C}}{{\mathbf{O}}_2}{\text{ }}\left( {\mathbf{g}} \right):\)

Under what conditions will decomposition in a closed container proceed to completion so that no \({\bf{CaC}}{{\bf{O}}_3}\) remains?

See all solutions

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