**General Chemistry 4th Edition***McQuarrie • Rock • Gallogly***University Science Books** presented by Macmillan Learning---Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is:\[ \text{S}_2(g) + \text{C}(s) \rightleftharpoons \text{CS}_2(g) \quad K_c = 9.40 \, \text{at} \, 900 \, \text{K}\]How many grams of \(\text{CS}_2(g)\) can be prepared by heating 13.1 mol \(\text{S}_2(g)\) with excess carbon in an 8.50 L reaction vessel held at 900 K until equilibrium is attained?**mass of \(\text{CS}_2(g)\):** \_\_\_\_\_ g---Question Source: McQuarrie, Rock, and Gallogly 4e - General Chemistry | Publisher: University Science Books*Note: This is a text-based transcription of an educational content image for learning purposes.* **Equilibrium Concentration Calculation****Consider the reaction:**\[ \text{A(aq)} \rightleftharpoons 2\text{B(aq)} \]\[ K_c = 4.46 \times 10^{-6} \text{ at 500 K} \]**Problem Statement:**If a 4.70 M sample of A is heated to 500 K, what is the concentration of B at equilibrium?\[ \text{[B]} = \_\_\_\_\_\_\_\_ \text{ M} \]**Explanation:**This is a classic equilibrium problem where you are given the initial concentration of A and the equilibrium constant (\(K_c\)) at a particular temperature (500 K). You are asked to find the equilibrium concentration of product B. To solve this:1. **Set up an ICE table (Initial, Change, Equilibrium) for the reaction.**2. **Use the expression for the equilibrium constant:** \[ K_c = \frac{[\text{B}]^2}{[\text{A}]} \] **where \([\text{A}]\) is the concentration of A at equilibrium, and \([\text{B}]\) is the concentration of B at equilibrium.**3. **Solve for \([\text{B}]\) using the given values and the assumed changes at equilibrium.**This approach helps in visually organizing how the concentrations change and applying the stoichiometry of the reaction to find the solution.

Answered: Image /qna-images/answer/d615f2fe-67d2-4702-8b6a-4939d67cc332.jpg

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S,(g)+C(s) = CS,(g) K. = 9.40 at 900 K How many grams of CS,(g) can be prepared by heating 13.1 mol S,(g) with excess carbon in a 8.50 L reaction vessel held at 900 K until equilibrium is attained? mass of CS,(g):

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S,(g)+C(s) = CS,(g) K. = 9.40 at 900 K How many grams of CS,(g) can be prepared by heating 13.1 mol S,(g) with excess carbon in a 8.50 L reaction vessel held at 900 K until equilibrium is attained? mass of CS,(g):

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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