### Equilibrium Calculation Example**Problem:**Given the reaction: \[ 2 \text{H}_2\text{S(g)} \rightleftharpoons 2 \text{H}_2\text{(g)} + \text{S}_2\text{(g)} \]where \( K_c = 9.3 \times 10^{-8} \) at 400°C.3.5 moles of \(\text{H}_2\text{S}\) are placed in a 3.0 L container and the system is allowed to reach equilibrium. Calculate the concentration of \(\text{H}_2\) at equilibrium.**Options:**1. **3.1 × 10⁻³ M** (Your answer)2. **4.8 × 10⁻³ M**3. **2.7 × 10⁻⁸ M**4. **3.2 × 10⁻⁴ M**5. **6.3 × 10⁻³ M** (Correct answer)

Answered: Image /qna-images/answer/935dd285-baa9-4472-86b3-ff66e43fef05.jpg

(Incorrect) 2 H₂S(g) + 2 H₂(g) + S₂(g) Kc = 9.3x 108 at 400°C 3.5 moles of H₂S are placed in a 3.0 L container and the system is allowed to reach equilibrium. Calculate the concentration of H₂ at equilibrium. 3.1 x 10-3 M (Your answer) 4.8 x 10-3 M 2.7 x 10-8 M 3.2 × 10-4 M 6.3 x 10-3 M (Correct answer)

(Incorrect) 2 H₂S(g) + 2 H₂(g) + S₂(g) Kc = 9.3x 108 at 400°C 3.5 moles of H₂S are placed in a 3.0 L container and the system is allowed to reach equilibrium. Calculate the concentration of H₂ at equilibrium. 3.1 x 10-3 M (Your answer) 4.8 x 10-3 M 2.7 x 10-8 M 3.2 × 10-4 M 6.3 x 10-3 M (Correct answer)

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...

See similar textbooks

Similar questions

Answer the question please.
Consider the following reaction: 2CO (g) + O2 (g) ⇒ 2CO2 (g). In a 2.00 L vessel, 0.5 moles of carbon monoxide gas reacts with 0.5 moles of oxygen gas. Given that K = 2.2 × 10-22, what are the concentrations of all species at equilibrium? The concentration of CO at equilibrium is The concentration of O2 at equilibrium is The concentration of CO2 at equilibrium is
Select all of the correct statements about equilibrium from the choices below.At equilibrium the rates of forward and reverse reactions are equal. As a reaction proceeds forward toward equilibrium the forward rate drops. At equilibrium all reactions stop. Reactants are transformed into products even at equilibrium. As a reaction proceeds forward toward equilibrium the reverse rate constant rises.As a reaction proceeds forward toward equilibrium the forward rate constant drops.
When 2.00 moles of nitrogen gas and 3.00 moles of oxygen gas were combined in a 4.0 L cylinder (at 385oC) there were 0.30 moles of N2O present at equilibrium. Calculate the Kc for this equilibrium reaction.
Consider the following system at equilibrium: CH4(g) + 2H20(g) CO2(g) + 4H2(g) What change will cause the equilibrium to shift to form more CH4? Multiple Choice decrease (H2] increase (H20] decrease the volume of the reaction vessel increase (CH4] decrease [CO2] DELL
At a certain temperature, 0.840 mol SO3 is placed in a 4.50 L container. 2 SO₂ (g) 2 SO₂(g) + O₂(g) At equilibrium, 0.100 mol O₂ is present. Calculate K. Kc = 6.914 ×10−5 Incorrect
For the equilibrium shown below, assess whether the following mixture is at equilibrium. If the mixture is NOT at equilibrium, tell whether the reaction will form more reactant or more products to reach equilibrium. 2 CO2 (g) 2 CO (g) + O2 (g) Kc = 6.4 x 10-7 [CO2] = 5.3 x 10-2 M [CO] = 3.6 x 10-4 M [O2] = 2.4 x 10-3 M
Give typed explanation
Consider the following equilibrium system: 2 NOCI(g) 2 2 NO(g) + Cl2(g) Kc = 57.0 Initially, only NOCI gas is placed in a flask. After equilibrium has been reached it is found that the concentration of the nitrogen monoxide gas in the flask is 1.14 mol/L. What is the initial molar concentration of the NOCI gas? Answer to three decimal places.
Show steps
K = 1.3 \times 10-10 for the reaction HC6H50(aq) = H+(aq) + C6H50-(aq). In which direction is the equilibrium favored? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a Forward b Reverse c Appreciable quantities of all species are present at equilibrium d No direction is favored e There is not enough information to determine the direction
1.QuestionGiven the reaction at equilibrium: 2 SO2(g) + O2(g) <--> 2 SO3(g) + heat Which change will shift the equilibrium to the right? increasing the temperature increasing the pressure decreasing the amount of SO2(g) decreasing the amount of O2(g)