12. The following gases are added to a 1.00 L container: 2.0 mole of A; 4.0 mole of B. The gases react as follows: A (g) + 3B (g) = C (g) + 2D (g) a. Create an ICE table to indicate the initial concentrations, the change in concentrations with respect to x, and the equilibrium concentrations al all the reactants and produces with respect to x. b. If the container contains 0.4 moles of D at equilibrium, calculate the equilibrium concentrations of A, B, C, and D. c. Calculate the value for the equilibrium constant at this temperature.

12. The following gases are added to a 1.00 L container: 2.0 mole of A; 4.0 mole of B. The gases react as follows: A (g) + 3B (g) = C (g) + 2D (g) a. Create an ICE table to indicate the initial concentrations, the change in concentrations with respect to x, and the equilibrium concentrations al all the reactants and produces with respect to x. b. If the container contains 0.4 moles of D at equilibrium, calculate the equilibrium concentrations of A, B, C, and D. c. Calculate the value for the equilibrium constant at this temperature.

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

Related questions

Q: sider the equilibrium 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H2O(g). Predict the effect on the…

A: We have given that 4NH3(g) + 3O2(g) ⇌ 2N2(g) + 6H2O(g) Effect on the equilibrium…

Q: Given the following equilibrium, which of the following will result in an increased amount of…

A: Which of the following will increase the amont of Cl2?

Q: The equilibrium constant, K, for the following reaction is 1.20x10-² at 500K. PCI5(g) PC13 (8) +…

A: Answer:For any reaction, value of equilibrium constant KC is equal to the ratio of molar…

Q: 2. For this chemical reaction at 298K, the concentration of the product is concentration of…

Q: Consider the following system at equilibrium at 350 K: 2CH,Cl2(g) CH4(g) + CC4(g) When some CH,C2(g)…

A: According to Le Chatelier's principle if factors(like temperature,pressure,molar concentration etc)…

Q: For the following chemical reaction, CO (g) + H₂O (g) → CO2 (g) + H2 (g) Kc = 0.0257 If a 2.00L…

Q: Nitrogen and water react to form nitrogen monoxide and hydrogen, like this: N2g) + 2 H,0(g) → 2…

A: Calculate Kc of the given reaction----

Q: 2. Given the reaction, UO₂ (g) + 4 HF (g) → UF4 (g) + 2 H₂O (g), predict the effect each of the…

Q: 10. Consider the following gas phase equilibrium CO(g) +2NO(g) = N₂O(g) + CO₂(g) Increasing the…

A: According to Le Chatelier principle if a system is in equilibrium is subjected to change of…

Q: Consider the following reaction: 2 A (g) → B (g) + C (g) Kc = 196 at 400 °c If you add 2.35 mol A…

A: We have 2.35 mole of A , in 5 L of flask , we have to calculate the equilibrium concentration of all…

Q: 1a. For the following reaction 6.0 moles of H2 were combined with 4.5 moles of Cl2. The reaction…

A: Answer:Given data:

Q: Given the reaction, UO 2 (g) + 4 HF (g) ⇌ UF 4 (g) + 2 H 2 O (g), predict the effect each of the…

A: Le Chatelier's principle: This principle is used to predict the effect of a change in conditions on…

Q: O ADVANCED GENERAL CHEMISTRY Calculating an equilibrium constant from an equilibrium. Nitrogen and…

Q: Consider the reaction: 2 A (g) + B (s) ⇌ 2 C (s) + D (g) To increase the partial pressure of D at…

A: Consider the reaction: 2A(g) + B(s) ⇌ 2C(s) + D(g) To increase the partial pressure of D at…

Q: 8. The equilibrium constant (K.) for this reaction is 1.60 at 990 °C H2(g) + CO2(g) E H20(g) + CO(g)…

Q: Consider the reaction: A(g) + B(g) = 2C(g), Kc = 44.4. Suppose an 3.80-L mixture initially contains…

A: We have to calculate the equilibrium concentration of C.

Q: Write a balanced chemical reaction which corresponds to the following equilibrium constant…

A: The equilibrium constant is a numerical value that represents the ratio of the concentrations of the…

Q: For the following reaction, initially you start with 1.33 mol of N2(g) and 2.80 mol of O2(g) in a…

A: Note: As per our guidelines, we are supposed to answer only one question when multiple questions are…

Q: Carbon disulfide and oxygen react to form carbon dioxide and sulfur dioxide, like this: Cs,(g)+30,…

Q: Consider the following system at equilibrium at 1150 K: 250;(g) + O2(g) 2 2s0;(g) When some O,(g) is…

A: Answer :- a) The reaction must: - (B) run in reverse direction to re-establish equilibrium. b) The…

Q: Hydrogen and iodine gas react to form hydrogen iodide: H2(g) + I2(g) ⇌ 2Hl(g) Kc=54.4 A…

Q: Identify the equilibrium constant expression for the reaction so,(3) + NO,(3) = so,(g) +NO(g) given…

Q: 4-(N-Morpholino)butanesulfonic acid (MOBS) is a weak acid used to prepare buffers for biological…

A: Given,The mass of 4-(N-Morpholino)butanesulfonic acid (MOBS) = 5.00 g pKa of MOBS = 7.48 Molar mass…

Q: 1. Write the expression for the equilibrium constant K for the following reactions below. a. N₂ (g)…

A: In equilibrium the active concentration of pure solid and liquid substances are considered to be…

Q: Consider the equilibrium system described by the chemical reaction below, which has a value of Kc…

A: Given: Kc = 1.2 x 10-4 The given balanced equation for the reaction is

Q: In a 3.0 L vessel, 1.5 mols of H2, 1.5 mols of F2 and 3.0 mols of HF are put in. If the equilibrium…

Q: Consider the following system at equilibrium at 350 K: CHĄ(g) + CCl4(g) ? 2CH,Cl,(g) When some…

Question

12. The following gases are added to a 1.00 L container: 2.0 mole of A; 4.0 mole of B. The gases react as
follows:
A (g) + 3B (g) = C (g) + 2D (g)
a. Create an ICE table to indicate the initial concentrations, the change in concentrations with respect to x,
and the equilibrium concentrations al all the reactants and produces with respect to x.
b. If the container contains 0.4 moles of D at equilibrium, calculate the equilibrium concentrations of A, B,
C, and D.
c. Calculate the value for the equilibrium constant at this temperature.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider the following reaction at equilibrium:2SO2(g) + O2 (g) <==> 2SO3(g)Determine if the following changes will increase, decrease or not affect the partial pressure of SO2.a. Decreasing the amount of oxygen in the systemb. Decreasing the volume of the systemc. Decreasing the temperature of the systemd. Decreasing the pressure of the systeme. Adding a catalyst to the reaction system
Consider the following system at equilibrium at 600 K:COCl2(g) =CO(g) + Cl2(g)When some COCl2(g) is added to the equilibrium system at constant temperature: The reaction must: fill in the blank 1 A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CO will: fill in the blank 2 A. Increase. B. Decrease. C. Remain the same.
d. he following system establishes an equilibrium at 545 K: NH₂HS (s)- NH₂ (8) + H₂S (8) AND >O Briefly explain the effect in terms of the expected shift (toward reactant, toward product or no change) of each of the following: a b. The volume of the container is doubled. The temperature of the system is raised to 825 K C. Some additional solid NH4HS is added. The reaction flask has 1.25 atm of the inert gas argon added to it. 5. (10 points) At 355 K, a 10.00 L reaction flask is charged with 1.44 atm each of hydrogen and fluorine gas. The following reaction takes place: H2 (8) + F2 (g) = 2 HF (g) Kp = 176 Based on building an ICE table, determine the partial pressure of H2, F2 and HF once equilibrium has been established.
Consider the following system at equilibrium at 698 K: 2 HI (g)=H2 (g) + I2 (g) When some H2 (g) is added to the equilibrium system at constant temperature: The reaction must: A. Run in the forward direction to reestablish equilibrium. B. Run in the reverse direction to reestablish equilibrium. C. Remain the same. It is already at equilibrium. The concentration of I, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 9 more group attempts remaining
5. The equilibrium constant expression of a gas reaction is [CS2] [H2]* _ [CH4] [H2S]? K. Write the balanced chemical equation corresponding to this expression
HBr=.....M
Consider the reaction A + B C+D, which has an equilibrium constant, K, equal to 3.4 x 102. If one begins a reaction by placing 0.600 moles of A in a 1.0 L container as well as 0.150 moles of 1. B, what will be the equilibrium concentrations of A, B, C, and D? Write your answers in the spaces provided below. a. [А] b. [B]= [C]= С. d. [D]= Once the reaction in problem 1 reaches equilibrium, some additional B is injected into the flask 2. from an outside source. LeChatelier's principle says the reaction will (circle one): be unchanged shift to the right shift to the left Pyridine is a weak base with a Kb 1.7 x 109. If 0.300 moles of pyridine is added to 1.00 L of 3. water, what will be the equilibrium concentrations of the species below: a. [Pyridine] = b. [Pyridine-H] (the pyridinium ion) [ОН-] 3 С. What is the pH of the solution in problem 4 (above)? .
20.
In a 5.00 L reaction vessel 2.00 moles of ICl (g) are added. one Begin The reaction that occurs in the container is Chores 2 ICs| (g) = 12 (g) + Cl2 (g) Kc = 4.8 x 10-6 Students a. Write the expression for Kc. b. Complete the ICE table. My classes c. Calculate all the equilibrium concentrations.