At 1024°C, the pressure of oxygen gas from the decomposition of copper(II)oxide is 0.490 bar: 4 CuO (s) 2 Cu₂0 (s) + O₂(g) a. What is the value of Kp for this reaction? (Hint: Use 1 atm as your standard pressure) b. Calculate the fraction of CuO that will decompose if 0.160 mole of it is placed in a 2.00 L flask at 1024°C. c. What would the fraction be if a 1.00 mole sample of CuO were used? d. What is the smallest amount of CuO in moles that is needed in order to establish equilibrium? e. What is the Gibbs standard energy for this reaction?

At 1024°C, the pressure of oxygen gas from the decomposition of copper(II)oxide is 0.490 bar: 4 CuO (s) 2 Cu₂0 (s) + O₂(g) a. What is the value of Kp for this reaction? (Hint: Use 1 atm as your standard pressure) b. Calculate the fraction of CuO that will decompose if 0.160 mole of it is placed in a 2.00 L flask at 1024°C. c. What would the fraction be if a 1.00 mole sample of CuO were used? d. What is the smallest amount of CuO in moles that is needed in order to establish equilibrium? e. What is the Gibbs standard energy for this reaction?

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: consider the reaction of carbon monoxide and chlorine gases to form gaseous phosgene, COCl2.…

Q: he minerals magnetite (Fe302) and hematite (Fe2O3) xygen. exist in equilibrium with atmospheric a.…

A: For any gaseous reaction at equilibrium,aA(g)+bB(g)⇌cC(g)+dD(g)the equilibrium constant at constant…

Q: For the reaction 2BrF₅ (g) ⇋ Br₂ (g) + 5F₂ (g), the equilibrium concentrations at 1500 K are: [BrF₅]…

Q: CHEMWORK A sample of solid ammonium chloride was placed in an evacuated chamber, and then heated…

A: Kp is equilibrium constant in terms of partial pressure of product upon partial pressure of…

Q: At high temperatures bromine molecules can dissociate into bromine atoms. For the reaction Br2(g) =…

A: Given : Initial pressure of Br2 = 7.00 atm Kp = 2.48 * 10-3

Q: When heated, ammonium carbamate decomposes as follows: NH4CO2NH2(s) ⇌ 2NH3 (g) + CO2 (g) At a…

A: NH4CO2NH2(s) ⇌ 2NH3 (g) + CO2 (g)

Q: The equilibrium constant Kc equals 0.0948 for the following reaction at 273°C. CH3OH(g) CO(g) + 2…

A: The reaction given is CH3OH(g) ------> CO(g) + 2 H2(g) Kc = 0.0948

Q: Complete the balanced chemical equation for the following reaction between a weak acid and a strong…

A: Balanced chemical equation is the equation in which number of atoms on both sides of equation are…

Q: A gas sample of N2O4 is placed in an empty cylinder at 25oC. When equilibrium is reached the total…

Q: Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample…

A: Given: volume of solution = 2.50 L Mass of NO = 1.25 g Mass of Br2 = 0.787 g…

Q: 5. The equilibrium constant Kp for the following reaction is 0.403 at 1000 °C. FeO(s) + CO(g) Fe(s)…

A: Answer: Whether a system is at equilibrium or not, it can be checked by calculating the value of…

Q: A flask is charged with 1.390 atm of N2O4(g) and 0.88 atm NO2(g) at 25°C After equilibrium is…

A: Given that : Initial pressure of N2O4 = 1.390 atmInitial pressure of NO2 = 0.88 atm After…

Q: 17. Consider the below equation. At 1000 °C, Kp is 0.403. FeO(s) + CO(g) Fe(s) + CO₂(g) a. When…

Q: For the following reaction in a closed container at 350°C: CaCO 3(s) ⇌ CaO(s) + CO 2(g) The…

Q: A tiny sample of an aqueous solution of two substances R and P is sketched below, as if it was under…

A: Given that, an equilibrium interconversion reaction is R ⇌ P. The value of the equilibrium constant…

Q: e reaction

Q: Represent the equilibrium constants Kp for the following reactions a) PC15(g) → PCl3(g) + Cl₂(g) b)…

Q: Consider the reaction: 2 N₂O5(g) 4 NO₂(g) + O₂(g) Some N₂O5(g) is placed in a container, which…

Q: Dinitrogen tetroxide forms an equilibrium with nitrogen dioxide. Both are gases. In an experiment,…

A: The reaction taking place is N2O4 (g) -----> 2 NO2 (g) Since molar mass of N2O4 = Atomic mass of…

Q: The reddish brown hue of nitrogen dioxide gas is associated with pollution of the atmosphere.…

A: The given reaction in equilibrium is: 2NO(g) + O2(g) <------> 2NO2(g) ; Kp = 1.7*1012

Q: At 40.°C, 2.0 mol of hydrogen and 2.00 mol bromine are put in a 2.0L flask and allowed to react…

A: Ideal gas equation is PV = nRT P= nRTV Given, Temperature =40∘C =…

Q: 1. How many milliliters of 53.40(±0.06) (w/w) % NaOH with a density of 1.52(±0.01)g/mL will you…

Q: 1 For the reaction: Ag₂0 (s) 2 Ag (s) + O₂(g) the pressure of the reaction 2 at 173°C is 422 torr.…

Q: The value of Kp for the reaction 2 A(g) + B(g) + 3 C(g) → 2 D(g) + E(g) is 19350 at a particular…

A: Welcome to bartleby !

Q: Kp for the following reaction at a give temperature is 0.263 at 1000. K: C(s) + 2 H₂(g) CH4(g) What…

A: Answer:Here:'

Q: The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2SO2(g) + O2(g)…

A: Reaction equation : 2SO3(g) → 2SO2(g) + O2(g)Equilibrium constant, Kp, for this…

Q: 1. At 603 K, there are 0.0100 mol of NH,Cl, 0.0100 mol of NH3, and 5.8 x 10-3 mol of HCl in a closed…

Q: When heated, iodine vapor dissociates according to this equation. I2(g) 2 I(g) At 1327 K, a sample…

Q: N204 (g) = 2 NO2 (g) 11 N204 is placed into an empty container to an initial pressure of 1.292 atm…

A: The given equilibrium reaction is as follows: N2O4g ⇌ 2NO2g The initial pressure of N2O4 is = 1.292…

Question

At 1024°C, the pressure of oxygen gas from the decomposition of copper(Il)oxide is 0.490 bar:
4 CuO (s) = 2 Cu2O (s) + O2 (g)
a. What is the value of Kp for this reaction? (Hint: Use 1 atm as your standard pressure)
b. Calculate the fraction of CuO that will decompose if 0.160 mole of it is placed in a 2.00 L flask at 1024°C.
c. What would the fraction be
a 1.00 mole sample of CuO were used?
d. What is the smallest amount of CuO in moles that is needed in order to establish equilibrium?
e. What is the Gibbs standard energy for this reaction?

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

Step 2

Step 3

Step 4

Step 5

Step 6

Step 7

Trending now

This is a popular solution!

Step by step

Solved in 7 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

The value of Kp for the reaction 2 A(g) + B(g) + 3 C(g) → 2 D(g) + E(g) is 16870 at a particular temperature. What does the magnitude of Kp tell us about the equilibrium position of the reaction? A) There are many more products than reactants. B) There are only a few more products than reactants. C) There are many more reactants than products. D) There are only a few more reactants than products.
An empty steel container is filled with 0.0490 atm of HF. The system is allowed to reach equilibrium. If Kp = 2.76 for the reaction below, what is the equilibrium partial pressure of H₂? 2 2 HF (g) → H2 (g) + F2 (g)
Consider the reaction: 2HI(g) ⇀ H2(g)+I2(g). At 500 C∘, a flask initially has all three gases, each at a partial pressure of 0.200 atm. When equilibrium is established, the partial pressure of HI(g) is determined to be 0.480 atm. a. Calculate the Kp for the reaction b. What is the equilibrium partial pressure of H2(g) and I2(g)? c. What is ΔG⊖reaction?
Consider the following equilibrium process at 686. °℃: CO₂(g) + H₂(g) CO(g) + H₂O(g) The equilibrium concentrations of the reacting species are [CO]=0.0560 M, [H₂] = 0.0400 M, [CO₂]=0.0830 M, and [H₂O]=0.0430 M. Part 1 of 5 Calculate K for the reaction at 686. °C. Round your answer to 3 significant digits. с Kc- Part 2 of 5 x10 If we add CO₂ to increase its concentration to 0.510 M, what will the concentrations of all the gases be when equilibrium is reestablished? Round your answer to 3 significant digits. [CO₂] = M x10 X Ś
Kp for the following reaction at a give temperature is 0.263 at 1000. K: C(s) + 2 H2(g) = CH4(g) What is the total pressure (in atm) in a 10.0 L flask when 25.0 g of C(s) and 4.50 g of H2 are introduced to the flask and allowed to equilibrate at 1000. K? Enter your answer without units.
The value of Kp for the reaction 2 A(g) + B(g) + 3 C(g) → 2 D(g) + E(g) is 12770 at a particular temperature. What does the magnitude of Kp tell us about the equilibrium position of the reaction? A) There are many more products than reactants. B) There are only a few more products than reactants. C) There are many more reactants than products. D) There are only a few more reactants than products.
Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)
Some quantity of NOBr is added to an otherwise empty flask. The reaction: 2 NOBr (g) ⇄ 2 NO (g) + Br2 (g) takes place at a particular temperature for which KP is 3.5 x 10-5. Assuming an equilibrium pressure of NOBr = 2.46atm, what is the equilibrium pressure of NO?
In a particular experiment 1.0 mole of H2O (g) and 1.0 mole of CO (g) are put into a flask and heated to 350 oC. In another experiment 1.0 mol of H2 (g) and 1.0 mole of CO2 (g) are put into a different flask with the same volume as the first. This mixture is also heated to 350 oC. After equilibrium is reached, will there be any difference in the composition of the mixture in the two flasks?
Carbon tetrachloride can be produced by the following reaction: CS₂(g) + 3 Cl₂ (g) S₂Cl₂(g) + CCL (g) Suppose 1.20 mol of CS₂ and 3.60 mol of Cl₂ were placed in a 1.00-L flask at an unknown temperature. After equilibrium has been achieved, the mixture contains 0.23 mol CCl4. Calculate Ke at the unknown temperature. Ke- Submit Answer Try Another Version References] 10 item attempts remaining
11. PLease refer to the attached photo. THank youuu
7. Write the equation for the reaction in which solid carbon reacts with gaseous carbon dioxide to form gaseous carbon monoxide. At equilibrium, a 2.0 L reaction vessel is found to contain 0.40 mol of C, 0.20 mol of CO, and 0.10 mol of CO. Find the Keq: