73/ If the reaction 2H2S(g) - 2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.0120. Startingfrom pure H2S introduced into an evacuated vessel at 1065°C, what will the totalthe vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H2(g)?pressurein 74. A quantity of liquid methanol, CH3OH, is introduced into a rigid 3.00-L vessel, the vesselis sealed, and the temperature is raised to 500K. At this temperature, the methanol vaporizesand decomposes according to the reactionCH3OH(g) - CO(g) + 2 H2(g), K.= 6.90×10 ?.If the concentration of H2 in the equilibrium mixture is 0.426M, what mass of methanol wasinitially introduced into the vessel?A. 147 gB. 74.3 g

Answered: Image /qna-images/answer/95fbc86b-9bfa-436d-8273-5a6e5f75f03c.jpg

73/ If the reaction 2H2S(g) - 2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.0120. Starting from pure H2S introduced into an evacuated vessel at 1065°C, what will the total the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H2(g)? pressure in

73/ If the reaction 2H2S(g) - 2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.0120. Starting from pure H2S introduced into an evacuated vessel at 1065°C, what will the total the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H2(g)? pressure in

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 mixture of 0.06953 mol of CH. 0.05245 mal of H₂S, 0.02207 mol of CS, and 0.08415 mol of Hy is…

A: Since the volume of the vessel is 1.0 L, the mole is the same as the molarity(M). Hence the initial…

Q: At a particular temperature, Kp = 0.370 for the reaction N2O4 (g) = 2NO2 (g) A flask containing only…

A: Given : Kp for the reaction is 0.370 Initial partial pressure of N2O4(g) is 4.10 atm.

Q: The equilibrium constant, K, for the following reaction is 0.440 at 341 K NH₂HS(s)NH₂(g) + H₂S(g) An…

A: Recall the given reaction, NH4HS s ↔ NH3 g + H2S g Kc = 0.440…

Q: At a certain temperature, the given reaction has an equilibrium constant of Kp=391 .…

A: The balanced reaction given is :PCl3 (g) + Cl2 (g) ↔ PCl5 (g)For this reaction, Kp = 391Initial…

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

A: Given is, Kp= 55.6 Initial pressure= 1.33 atm H2 + I2 -----> 2HI Calculate pH2 =?…

Q: Ammonium iodide, a solid, decomposes to give NH3(g) and HI(g). At 406 °C, some NH4I(s) is placed in…

A: Given: For equation: NH4I(s)→ NH3(g) + HI(g) Total pressure = 1.07 atm Partial pressure of NH3=…

Q: O3(g) 2 SO₂(g) + O = 2.62 x 10-6 at 400° (g) at an initial press ilibrium. What will be

A: Given reaction is : 2 SO₃(g) ⇌ 2 SO₂(g) + O₂(g) Pressure equilibrium constant = Kp = 2.62 × 10⁻⁶…

Q: For the reaction SO2C12(g) = SO2(g) + Cl2(g) Kp = 2.39 at 100°C A quantity of SO2CI2 was introduced…

Q: Be sure to answer all parts. The equilibrium constant K, for the reaction H2(g) + I,(g) =2 HI(g) is…

A: Given, H2(g) + I2(g) ⇌2HI(g) Equilibrium constant (KC) = 54.3 Temperature (T) = 430°C The initial…

Q: 2HI(g) H2(g) + 12(g) Kp = 0.0184 %3D A reaction vessel is filled with HI to a pressure of O.0240…

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: The equilibrium constant expression for the reaction, 2C0(g) + O2(g) 2C02(g) is given by Kp

A: Kp = P2CO2 / P2CO × PO2 -----> option(D)

Q: The reaction 2H,S(g) → 2H2(g) + S2(g)_at 1065°C, K, = 0.0320. Starting from pure H2S introduced into…

A: Given data: Equilibrium constant Kp = 0.0320 Partial pressure of hydrogen at equilibrium PH2 = 0.4…

Q: The equilibrium constant, Ke, for the following reaction is 6.30 at 723K. 2NH3(g) N2(g) + 3H2(g) If…

A: The given reacion is : 2NH3(g) <===> N2(g) + 3H2(g) The expression for Kc in the above…

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: Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 1.5 L…

Q: If the reaction 2H₂S(g) → 2H₂(g) + S₂(g) is carried out at 1065°C, Kp = 0.0120. Starting from pure…

Q: Consider the equilibrium system described by the chemical reaction below. If 0.1908 moles of CO2,…

A: For a general reaction, aA+bB⇌cC+dD The equilibrium…

Q: PNO= ?

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

Q: A mixture of 1.00 mol NaHCO3(s) and 1.00 mol Na,CO3(s) is introduced into a 2.50 L flask in which…

A: The reaction for the process is given below : Since NaHCO3 and Na2CO3 are in solid form, therefore…

Q: At 113 oC the equilibrium constant for the reaction: 2 HBr(g) H2(g) + Br2(g) is KP = 1.81e-12. If…

A: Given , Kp= 1.81× 10-12 Initial pressure of (PHBr) =0.00631 atm Given reaction, 2HBr…

Q: For the reaction 2Mo(s) + CH4(g) MO2C(s) + H2(g) Kp = 3.55 at 973K. What will have to be the initial…

A: Let the initial pressure of CH4 is y. Kp = 3.55 (PH2) = 0.75atm

Q: The reaction C(s)+2H2(g) = CH4(g) has Kp=0.263 at 1000. K. Calculate the total pressure at…

A: Answer:First problem is based on the concept of equilibrium and second problem is based on the…

Q: Determine the equilibrium constant, K.

A: Initial pressure of Cl2 = 3.018 bar Initial pressure of SO2 =1.290 bar Total pressure at equilibrium…

Q: t 298K, K = 6.74 x 10° for the following reaction: C3H,O3 (g) C2H6(g) + 3CO(g) ) If 198g of C5H6O3…

A: Mass of C5H6O3 = 198 g Number of moles of C5H6O3= 198 g÷ 114g/mol =1.737 moles Molarity of C5H6O3…

Q: At a certain temperature, the given reaction has an equilibrium constant of K₂ = 389. PCI, (g) +…

Q: For the reaction system: H2(g) + X2(g) = 2HX(g), Kc = 24.4 at 300 K. A system at equilibrium made up…

Q: At a certain temperature, the Kp for the decomposition of H₂S is 0.822. H₂S(g) = H₂(g) + S(g)…

Q: For the reaction 2 SO3(g) 2 SO₂(g) + O₂(g) Kp = 2.62 x 10-6 at 400 °C. A 1.50 L vessel at 400 °C is…

Q: Consider the reaction N₂(g) + 3H₂(g)2NH3(g), Kp = 0.0150. An equilibrium mixture contains 2.15E1 atm…

A: Since, Equilibrium constant or Kp is the ratio of the equilibrium partial pressure of product over…

Q: Use the References to access Consider the following system 2 NO(g) + Br2 (9) When some Br2 (g) is…

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

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

A: Given Kp, for the following reaction is 0.558 at 523 K: C6H5CH2OH(g) C6H5CHO(g) + H2(g) We have to…

Q: The reaction 2H2S(g) 2H2(g) S2(g) _åt 0.0320 bure H2S introduced into an evacuated vessel at 1065°C,…

A: Daltons law states that mixture of non-reacting gases the total pressure exerted to gases to equal…

Q: A student ran the following reaction in the laboratory at 675 K: H2(g) + I(g)=2HI(g) When she…

Q: The equilibrium constant, K., for the following reaction is 77.5 at 600 K. Co(g) + C(g)=COC,(g)…

A: Kc = 77.5 Temperature 600 K Moles of CO = .231 Moles of Cl2 = .231 Volume of vessel = 1 L

Q: For the reaction SO,Cl2(g) = SO2(g) + Cl2(g) Kp = 2.39 at 100°C A quantity of SO½CI2 was introduced…

Q: Calculate the molality of the solution. (Assume a density of 1.08 g/mL for the solution.) Express…

A: Mass of solute ( NaCl ) = 126 g Molar mass of NaCl = 58.44 g/mol Therefore , Moles of NaCl (…

Q: The reaction C(s) + 2H, (g) = CH,(g) has K, - 0.263 at 1000. K. Calculate he total pressure at…

A: Dalton's law states that total pressure of mixture of gases is equal to the sum of the partial…

Q: The partial pressures at equilibrium in a 4.530L flask are: HI(g) at 0.533atm and p H2(g)=p…

A: We have to calculate the partial pressure once equilibrium is re establish.

Q: The equilibrium constant Kp for the reaction, 2 SO3(g) 2 SO2(g) + O2(g) is 6.710 at 744 °C. If a…

A: firstly construct the ICE table and then with help of Kp find the equilibrium partial pressure of O2…

Q: A mixture of 4.1 atm CO2, 2.1 atm H2, and 3.3 atm H₂O are added to a sealed 2.0 L vessel at 500 K…

A: The reaction is given as, CO2 (g) + H2 (g) <=> CO (g) + H2O (g) Also it is given, a mixture of…

Q: parts. The equilibrium constant K, for the reaction Ig) 21(g) is 3.75 x 10 5 at 726°C. Calculate K,…

Q: A reaction is prepared by adding 2.000 mol each of H2, 12, and HI gases to a 1.0 L container. They…

Q: Ak 1. At 900K, Kp = 0.345 for the following reaction, 2SO2(g) + Oz(9) = 2SO3(g) In the equilibrium…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Question

73/ If the reaction 2H2S(g) - 2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.0120. Starting
from pure H2S introduced into an evacuated vessel at 1065°C, what will the total
the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H2(g)?
pressure
in

74. A quantity of liquid methanol, CH3OH, is introduced into a rigid 3.00-L vessel, the vessel
is sealed, and the temperature is raised to 500K. At this temperature, the methanol vaporizes
and decomposes according to the reaction
CH3OH(g) - CO(g) + 2 H2(g), K.= 6.90×10 ?.
If the concentration of H2 in the equilibrium mixture is 0.426M, what mass of methanol was
initially introduced into the vessel?
A. 147 g
B. 74.3 g

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

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

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

Please don't provide handwritten solution .....
For the reaction PCL5 (g) = PCl3 (g) + Cl₂ (g) at equilibrium, Kp = 321. The equilibrium partial pressures of PCl3 and Cl₂ are 1.00E0 atm and 4.50E0 atm, respectively. What is the equilibrium partial pressure of PCl5?
Some COCI₂ is allowed to dissociate into CO and Cl₂ at 873 K. At equilibrium, [COCI₂] = 0.244 M, and [CO] = [Cl₂] = 0.130 M. Additional COCI₂ is added so that [COCI₂]new = 0.404 M and the system is allowed to once again reach equilibrium. CoCl₂(g)=CO(g) + Cl₂(g) K = 6.98×10-2 at 873 K (a) In which direction will the reaction proceed to reach equilibrium? (b) What are the new concentrations of reactants and products after the system reaches equilibrium? [CoCl₂] = [CO] [Cl₂] = 333 V 4
At a certain temperature, the given reactions has an equilibrium constant of Kp = 389. PCl3(g) + Cl2(g) <> PCl5(g) PCl5 is placed in a sealed container at an i tail pressure of 0.0720 bar. What is the total pressure at equilibrium?
See attached
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 0.593 moles of CO and 0.593 moles of Cl, are introduced into a 1.00 L vessel at 600 K. [CO] M [Cl,] M [COCI,] =
The reaction C(s) + 2 H₂(g) = CH₂(g) has Kp = 0.263 at 1000. K. Calculate the total pressure at equilibrium when 4.305 g of H₂ and 22.06 g of C(s) are placed in a 9.08 L flask and heated to 1000. K. Ptotal = Calculate the total pressure when 4.305 g of H₂ and 7.404 g of C(s) are placed in a 9.08 L flask and heated to 1000. K. Ptotal = atm atm
The equilibrium concentrate of H2: 0.048 M The equilibrium concentrate of N2: 0.304M
For the equilibrium N2(g)+O2 <-->2NO(g), Kp = 0.0017 at 2300 K. At a given point, the partial pressures of the gases are PN2=PO2 = 0.660 atm and PNO= 0.0272atm. Which statment below is true? a. Q < K, so the reaction will continue to make more products. b. Q > K, so the reaction will consume products to make more reactants. c. Q = K, so the system is at equilibrium. d. The value of K will decrease until it is equal to Q. Show your work:
Please provide the correct answer. We typically use ICE tables with these problems but I need help
At a particular temperature, kp= 3.40 * 10^2 for the reaction H2 (g) +I2 (g) <---> 2HI(g) If 1.73 atm of H2 (g) and 1.73 atm of I2 (g) are introduced into a 1.00-L container, calculate the equilibrium partial pressures of all species. Partial pressure of H2 = atm Partial pressure of I2 = atm Partial pressure of HI = atm
7