At 900 °C, 𝐾_𝑐= 0.0108 for the reaction
CaCO₃(𝑠) ⇌ CaO(𝑠) + CO₂(𝑔)
A mixture of CaCO₃, CaO, and CO₂ is placed in a 10.0-L vessel at 900°C. For the following mixtures, will the amount of CaCO3 increase, decrease, or remain the same as the system approaches equilibrium?
(a) 15.0 g CaCO3, 15.0 g CaO, and 4.25 g CO2
(b) 2.50 g CaCO3, 25.0 g CaO, and 5.66 g CO2
(c) 30.5 g CaCO₃, 25.5 g CaO, and 6.48 g CO₂

Verified step by step guidance

Calculate the initial concentration of CO_2 using its mass and the volume of the vessel. Use the formula: \( \text{Concentration} = \frac{\text{mass}}{\text{molar mass} \times \text{volume}} \).

Determine the reaction quotient, \( Q_c \), using the initial concentration of CO_2. Since CaCO_3 and CaO are solids, they do not appear in the expression for \( Q_c \). Thus, \( Q_c = [\text{CO}_2] \).

Compare \( Q_c \) to the equilibrium constant \( K_c \). If \( Q_c < K_c \), the reaction will proceed to the right, increasing the amount of CO_2 and decreasing CaCO_3. If \( Q_c > K_c \), the reaction will proceed to the left, decreasing the amount of CO_2 and increasing CaCO_3.

Use the comparison from the previous step to determine if the amount of CaCO_3 will increase, decrease, or remain the same as the system approaches equilibrium.

Conclude based on the direction of the shift in equilibrium whether the amount of CaCO_3 will increase, decrease, or remain the same.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Equilibrium Constant (Kc)

The equilibrium constant, Kc, quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction CaCO3(s) ⇌ CaO(s) + CO2(g), Kc = [CO2] / [CaCO3]. A Kc value less than 1 indicates that at equilibrium, the reactants are favored, while a value greater than 1 suggests that products are favored.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. In this context, adding or removing reactants or products, or changing temperature or pressure, will shift the position of equilibrium, affecting the amounts of CaCO3, CaO, and CO2.

Stoichiometry of the Reaction

Stoichiometry involves the quantitative relationships between the amounts of reactants and products in a chemical reaction. For the reaction CaCO3(s) ⇌ CaO(s) + CO2(g), the stoichiometric coefficients indicate that one mole of CaCO3 produces one mole of CaO and one mole of CO2. Understanding these relationships is crucial for predicting how changes in the amounts of substances will affect the equilibrium state.

Recommended video:

Guided course

01:16

Stoichiometry Concept

Related Practice

Textbook Question

A 0.831-g sample of SO₃ is placed in a 1.00-L container and heated to 1100 K. The SO₃ decomposes to SO₂ and O₂: 2SO₃(𝑔) ⇌ 2 SO₂(𝑔) + O₂(𝑔) At equilibrium, the total pressure in the container is 1.300 atm. Find the values of 𝐾_𝑝 and 𝐾_𝑐 for this reaction at 1100 K.

views

Textbook Question

Nitric oxide (NO) reacts readily with chlorine gas as follows: 2 NO(𝑔) + Cl₂(𝑔) ⇌ 2 NOCl(𝑔) At 700 K, the equilibrium constant 𝐾_𝑝 for this reaction is 0.26. For each of the following mixtures at this temperature, indicate whether the mixture is at equilibrium, or, if not, whether it needs to produce more products or reactants to reach equilibrium. (b) 𝑃_NO= 0.12atm, 𝑃_Cl2= 0.10atm, 𝑃_NOCl= 0.050atm

Textbook Question

The equilibrium constant constant 𝐾_𝑐 for C(𝑠) + CO₂(𝑔) ⇌ 2 CO(𝑔) is 1.9 at 1000 K and 0.133 at 298 K. (a) If excess C is allowed to react with 25.0 g of CO2 in a 3.00-L vessel at 1000 K, how many grams of CO are produced? (b) If excess C is allowed to react with 25.0 g of CO₂ in a 3.00-L vessel at 1000 K, how many grams of C are consumed?

views

Textbook Question

At 700 K, the equilibrium constant for the reaction CCl₄(𝑔) ⇌ C(𝑠) + 2 Cl₂(𝑔) is 𝐾_𝑝= 0.76. A flask is charged with 2.00 atm of CCl₄, which then reaches equilibrium at 700 K. (a) What fraction of the CCl₄ is converted into C and Cl₂?