A mixture of 0.04096 mol of C₂H6, 0.05994 mol of N₂, 0.04520 mol of NH3, and 0.02898 mol of C₂H4 is placed in a 1.0-L steelpressure vessel at 1900 K. The following equilibrium is established:3 C₂H6(9) + 1 N₂(9)=2 NH3(g) + 3 C₂H4 (9)At equilibrium 0.02365 mol of C₂H4 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of C₂H6, N₂, NH3, and C₂H₁.Peq(C₂H6)Peq(N₂) =Peq(NH3)=Peq(C₂H4)=(b) Calculate Kp for this reaction.Kp =

The given reversible reaction is 3C2H6(g) + 1 N2(g) <====> 2 NH3(g) + 3 C2H4(g) Ideal gas…

A mixture of 0.04096 mol of C₂H6, 0.05994 mol of N₂, 0.04520 mol of NH3, and 0.02898 mol of C₂H4 is placed in a 1.0-L steel pressure vessel at 1900 K. The following equilibrium is established: 3 C₂H6(9) + 1 N₂(9)=2 NH3(g) + 3 C₂H₂(9) At equilibrium 0.02365 mol of C₂H4 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of C₂H6, N₂, NH3, and C₂H₁. Peq(C₂H)= Peq(N₂) = Peg(NHy) = Peq(C₂H4) (b) Calculate Kp for this reaction. Kp

A mixture of 0.04096 mol of C₂H6, 0.05994 mol of N₂, 0.04520 mol of NH3, and 0.02898 mol of C₂H4 is placed in a 1.0-L steel pressure vessel at 1900 K. The following equilibrium is established: 3 C₂H6(9) + 1 N₂(9)=2 NH3(g) + 3 C₂H₂(9) At equilibrium 0.02365 mol of C₂H4 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of C₂H6, N₂, NH3, and C₂H₁. Peq(C₂H)= Peq(N₂) = Peg(NHy) = Peq(C₂H4) (b) Calculate Kp for this reaction. Kp

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: (a) Calculate the equilibrium partial pressures of O2, NOCl, NO2, and Cl2. Peq(O2) = . Peq(NOCl)…

Q: A mixture of 0.02445 mol of C2H6, 0.05019 mol of N2, 0.02122 mol of NH3, and 0.03692 mol of C2H4 is…

Q: The equilibrium constant, Kp, for the following reaction is 0.558 at 523 K: C6H5CH2OH(g) C6H5CHO(g)…

Q: At T = 250 °C the reaction PCI5(g) =PC13(g) + Cl₂(g) has an equilibrium constant in terms of…

A: The direction in which the reaction proceeds to reach equilibrium can be predicted by determining…

Q: Write the expression for the equilibrium constant K, for the following reaction. Enclose pressures…

A: Equilibrium Constant, Kp is the equilibrium constant determined from the partial pressures of an…

Q: The equilibrium constant, Kc, for the following reaction is 0.967 at 650 K. 2NH3(g) N2(g) + 3H2(g)…

Q: A mixture of 0.02431 mol of C2H6, 0.02411 mol of N2, 0.03217 mol of NH3, and 0.02028 mol of C2H4 is…

A: Given that : Moles of C2H6=0.02431 molMoles of N2=0.02411 molMoles of NH3=0.03217 molMoles of…

Q: Predict v ianges in the compositions the engineer should expect next time he measures the…

Q: The equilibrium constant for the reaction NO(g) + NO2(g) ⇆ N2O3(g) is Kp…

Q: 3. Consider the following reaction where Kc = 3900 at 2000 K 2SO2(g) + O2(g) = 250³(g) a Write the…

Q: The equilibrium constant, Ke, for the following reaction is 0.00650 at 298 K. 2NOBr(g) 2NO(g) + Br₂…

Q: A chemical engineer is studying the following reaction: N₂(g) + 3H₂(g) → 2 NH3(g) At the temperature…

A: The direction in which the reaction proceeds to reach equilibrium can be predicted by determining…

Q: A chem gineer is studying the following reaction: 2 NO(g) + 2H₂(g) → N₂(g) + 2H₂O(g) At the…

A: Answer:When , reaction mixture is at equilibrium.When , reaction mixture is not at equilibrium and…

Q: At a certain temperature, a 17.0-L17.0-L container holds four gases in equilibrium. Their masses are…

A: The volume of the four gases is = 17.0 L The mass of SO3 is = 3.5 g The mass of SO2 is = 4.6 g The…

Q: A mixture of 0.02445 mol of C2H6, 0.05019 mol of N2, 0.02122 mol of NH3, and 0.03692 mol of C2H4 is…

A: The given reaction is : 3C2H6(g) + 1N2(g) ⇌ 2NH3(g) + 3C2H4(g) Inital moles of C2H6=0.02445…

Q: Solid carbon can react with gaseous water to form carbon monoxide gas and hydrogen gas. The…

A: The equilibrium reaction can be written as

Q: A mixture of 0.06906 mol of CH4, 0.01224 mol of H2S, 0.08482 mol of CS2, and 0.01029 mol of H2 is…

A: Given that : Initial moles of CH4=0.06906 molInitial moles of H2S=0.01224 molInitial moles of…

Q: A chemical engineer is studying the following reaction: CH (9)+2H,S(9) CS,(9)+4H,(9) At the…

A: Answer:- This question is answered by using the simple concept of reaction quotient and equilibrium…

Q: Solid carbon can react with gaseous water for form carbon monoxide gas and hydrogen gas. The…

A: The equilibrium reaction can be written as

Q: The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H₂(g) + I₂(g) =2HI(g)…

A: Given : Kc = 55.6 Initial moles of H2 = 0.265 Initial moles of I2 = 0.265 Volume = 1.00 L

Q: Hydrogen sulfide decomposes according to the following reaction, for which Kc is 9.30 x10-8 at 700…

A: Given data: Equilibrium constant Kc = 9.30 x 10-8. Number of moles of H2S = 0.45 mol. The volume of…

Q: At 1285° C the equilibrium constant for the reaction Br2 (g) 2 Br (g) is K. = 1.04 x 10 3. A 0.898-L…

A: Kc = [Br]^2/[Br2] Given mass of Br2 = 0.918 g Kc =0.00104 Concentration = moles /volume (in L)…

Q: H2O, 0.02864 mol of CH4, 0.07516 mol of CO, and 0.01990 mol of H2 is placed in a 1.0-L steel…

Q: The equilibrium constant, Kp, is 79.9 at 2500 K for the following reaction: XY2(g) + XZ2(g) = 2…

A: ICE table of Reaction XY2 (g) + XZ2 (g) →2 XYZ (g) Initial 0…

Q: perature the engineer picks, the equilibrium constant K, for this reaction is 0.047. er charges…

Q: the pressure or PCI5 hot dissociate. bar ulate the partial pressure of PCI5 at equilibrium. x bar t…

A: We have given that Consider the reaction PCI5(g) -----> PCI3(g) + Cl₂(g) for which Kp 1.05 at…

Q: Bromine monochloride is synthesized using the reaction Br₂(g) + Cl₂ (g) 2 BrCl(g) Kp = 1.1 x 104 at…

A: The objective of this question is to calculate the mass of Bromine monochloride (BrCl) that is…

Q: An experimenter placed 1.000 mol of H2 and 1.000 mol of Iz in a 1.000 L flask. The substances…

A: The equilibrium constant can be written as the ratio of concentration of products to the…

Q: The equilibrium constant, Kc, for the following reaction is 32.4 at 298 K. 2CH2CI2(g) =CH4(g) +…

Q: In an experiment conducted at 300 0C, the equilibrium concentrations of the species involved in the…

A: The given reaction is : 2NH3(g) ⇌ N2(g) + 3H2(g) at 300°C The equilibrium…

Q: The equilibrium constant K for the reaction H₂(g) + CO₂(g) H₂O(g) + CO(g) is 4.20 at 1650.00 °C.…

Q: A student ran the following reaction in the laboratory at 317 K:2NO(g) + Br2(g) 2NOBr(g)When she…

A: The objective of the question is to calculate the equilibrium constant, Kp, for the given reaction.…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

A mixture of 0.04096 mol of C₂H6, 0.05994 mol of N₂, 0.04520 mol of NH3, and 0.02898 mol of C₂H4 is placed in a 1.0-L steel
pressure vessel at 1900 K. The following equilibrium is established:
3 C₂H6(9) + 1 N₂(9)=2 NH3(g) + 3 C₂H4 (9)
At equilibrium 0.02365 mol of C₂H4 is found in the reaction mixture.
(a) Calculate the equilibrium partial pressures of C₂H6, N₂, NH3, and C₂H₁.
Peq(C₂H6)
Peq(N₂) =
Peq(NH3)=
Peq(C₂H4)=
(b) Calculate Kp for this reaction.
Kp =

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Step by step

Solved in 6 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

2 NO2CI (g) = 2 NO2 (g) + Cl2 (g) K = 7.81 x 10-5 NO2CI is placed into an evacuated container to an initial pressure of 1.984 M and allowed to reach equilibrium via the above reaction at 548 K. What is the molarity of NO2CI at equilibrium?
A student ran the following reaction in the laboratory at 675 K: (3) I + (3)*H =2HI(g) When she introduced H2(g) and I(g) into a 1.00 L evacuated container, so that the initial partial pressure of H2 was 4.53 atm and the initial partial pressure of Iz was 3.44 atm, she found that the equilibrium partial pressure of I, was 0.413 atm. Calculate the equilibrium constant, K. she obtained for this reaction. Kp =
A mixture of 0.01076 mol of Cl₂, 0.04718 mol of H₂0, 0.02718 mol of HCI, and 0.01676 mol of O₂ is placed in a 1.0-L steel pressure vessel at 1846 K. The following equilibrium is established: 2 Cl₂(g) + 2 H₂O(g) = 4 HCl(g) + 1 O₂(g) At equilibrium 0.001782 mol of Cl₂ is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of Cl₂, H₂O, HCl, and 0₂. Peq(Cl₂)= Peq(H₂O) = Peq (HCI) Peq(O₂) = = (b) Calculate Kp for this reaction. Kp =
The equilibrium constant, K. for the following reaction is 77.5 at 600 K. Co(g) + C,(g)=cOC»(g) Calculate the equilibrium concentrations of reactant and products when 0.231 moles of CO and 0.231 moles of Cl, are introduced into a 1.00 L vessel at 600K. [CO] M [CL] M [COCL] =| M
At a certain temperature, a 18.0-L18.0-L container holds four gases in equilibrium. Their masses are 3.53.5 g SO3SO3, 4.64.6 g SO2SO2, 19.619.6 g N2N2, and 0.980.98 g N2ON2O. What is the value of the equilibrium constant at this temperature for the reaction of SO2 with N2O to form SO3 and N2? Make sure you balance the reaction using the lowest whole-number coefficients.
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K.CO(g) + Cl2(g) COCl2(g)Calculate the equilibrium concentrations of reactant and products when 0.501 moles of CO and 0.501 moles of Cl2 are introduced into a 1.00 L vessel at 600 K.
A mixture of 0.06529 mol of CH4, 0.04045 mol of H2S, 0.06585 mol of CS2, and 0.03325 mol of H2 is placed in a 1.0-L steel pressure vessel at 1304 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g) 1 CS2(g) + 4 H2(g)Peq the equilibrium partial pressures of CH4, H2S, CS2, and H2. (CH4) = 7.5Peq(H2S) = 5.35Peq(CS2) = 6.42Peq(H2) = 1.5195 At equilibrium 0.01420 mol of H2 is found in the reaction mixture. Calculate KP for this reaction.KP = _____ .
Consider the following reaction: CO(g) + H₂O(g) = CO₂(g) + H₂(g). Exactly 200 torr each of CO and water vapor were introduced into a 500 ml flask. When the mixture reached equilibrium at 800 K, the partial pressure of CO2 was found to be 99 torr. Calculate the value of Kp.
The partial pressures at equilibrium in a 4.530L flask are: HI(g) at 0.533atm and p H2(g)=p I2(g)=0.0533atm. If additional HI(g) is added to the flask so it's partial pressure is increased to 0.750atm, calculate the partial pressures of HI,H2 and I2 once equilibrium is re-established.
A sample of N₂H6CO₂ weighing 22.5 grams is heated to 80°C in a 1.0 L container. All of the salt sublimes into NH3(g) and CO₂(g) according to the following equilibrium process. N₂H6CO₂ (s) + CO₂ (g) + 2NH3 (g) Determine the partial pressure of the NH3(g) in the system in atmospheres. This discussion is closed. M CAL -:00- 0:50- CI 2:00 Submit Answer Tries 0/99 3 F1 @ 2 ост 21 9: F2 3 80 F3 $ 4 10 a F4 % 5 S F5 6 tv A MacBook Air C F6 & 7 F7 ( Î DII FB F9 F10 F11 54 F13 Send 22
1 A + 2 B → 2 C Calculate the equilibrium constant (K) for the following reaction at 1000. K, using this information: A and B are placed in a flask and at the beginning of the reaction [A] is 8.95 M and [B] is 6.21 M. After the reaction has reached equilibrium,[B] is 1.94 M. Please ignore significant figures for this problem.
A chemical engineer is studying the following reaction: 2 NO(g)+2H2(g) → N,(9)+2H2O(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.0038. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction compound pressure expected change in pressure vessel NO 7.58 atm f increase I decrease (no change) H2 8.02 atm f increase I decrease (no change) A N, 4.16 atm f increase I decrease (no change) H,0 2.79 atm f increase I decrease O (no change) NO 8.89 atm ↑ increase I decrease (no change) H2 9.33 atm f increase I decrease (no change) В N2 3.51 atm f increase I decrease (no change) H,0 1.48 atm f increase I decrease (no change) NO…