A 650 mL reaction vessel initially contains 0.0125 mol of H,S at 800 °C. Calculate partial pressure of H, at equilibrium. 2 H2S (g) = 2 H2 (g) + S2(g) Kc = 1.67x107 at 800 °C 1 atm = 760 mmHg = 760 torr = 1.013 bar R = 0.08206 L atm mol-1 K-1 = 8.314 J mol-1 K-1 31.4 mmHg 16.7 mmHg 33.3 mmHg 46.2 mmHg 62.9 mmHg

A 650 mL reaction vessel initially contains 0.0125 mol of H,S at 800 °C. Calculate partial pressure of H, at equilibrium. 2 H2S (g) = 2 H2 (g) + S2(g) Kc = 1.67x107 at 800 °C 1 atm = 760 mmHg = 760 torr = 1.013 bar R = 0.08206 L atm mol-1 K-1 = 8.314 J mol-1 K-1 31.4 mmHg 16.7 mmHg 33.3 mmHg 46.2 mmHg 62.9 mmHg

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 equilibrium system described by the chemical reaction below. At equilibrium, a 6.5 L…

A: Recall the given reaction, The volume of the reaction vessel = 6.5…

Q: Consider the following system at equilibrium at 723 K: 2 NH3 (g) + 26.6 kcal — N2 (g) + 3 H2 (g)…

A: Note: As per guidelines, solution of 1st question has been made. For the expert solution of 2nd…

Q: At 1000 K, a sample of pure NO₂ gas decomposes: 2NO₂(g) = 2NO(g) + O₂(g) The equilibrium constant…

Q: Dinitrogen tetroxide, N2O4, is a colorless gas, which dissociates to give nitrogen dioxide, NO2, a…

Q: N2(g) + 3H2(g) 2NH3(g) When he introduced N2(g) and H2(g) into a 1.00 L evacuated container, so…

A: Equilibrium constant for a gaseous reaction is denoted as Kp .in other words Kp means equilibrium…

Q: While ethanol (CH2CH2OH) is produced naturally by fermentation, e.g. in beer- and wine-making,…

A: Given,

Q: Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 6.5 L…

A: Given the equilibrium chemical reaction isN2(g)+3H2(g)⇆2NH3(g)the equilibrium partial pressure of…

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: Which one of the following equilibrium reactions is not affected by a change in pressure? H2(g) +…

A: In this question we have to tell the effects on equilibrium by changing in pressure.

Q: An equilibrium mixture of NO2(g) and N2O4(g) has a total mass of 10.00 g. The mixture is allowed to…

A: This question is based on equilibrium. Data given : Total mass of the equilibrium = 10.00 g…

Q: Suppose a 500. mL flask is filled with 1.9 mol of NO and 1.5 mol of NO₂. The following reaction…

A: Recall the given reaction, NO3 g + NO g ↔ 2 NO2 g…

Q: While ethanol (CH2CH2OH) is produced naturally by fermentation, e.g. in beer- and wine-making,…

A: Step 1:Step 2:Step 3:

Q: Consider the following reaction at equilibrium, What will happen if the volume decreased at constant…

A: Le Chatelier's principle: When a change is applied to a system at equilibrium, the equilibrium will…

Q: Ethyl Acetate (EA) + Water = РАА = 0.15 atm PEth = 0.15 atm PH₂O = 0.25 atm PEA = 0.50 atm кр Acetic…

Q: For the reaction below, Keg = 2.62x10-7 (at 1000. C). If you place 12 atm of nitroger gas and 36 atm…

Q: 5. The reaction: 2NO₂(g) + 7H₂(g) = 2NH3(g) Analysis showed that there was 34.6 g of NO2, 53.2 g of…

Q: A reaction vessel is prepared by mixing 1.20 mmol SO2(g), 0.50 mmol O2(g), and 0.10 mmol SO3(g) in a…

A: Given: mmol of SO2 =1.20 mmol of O2 = 0.50 mmol of SO3 = 0.10 Volume of container =0.50 L Reaction:…

Q: The equilibrium constant Ke for the reaction 1₂(g) → 21(g) is 3.77 × 10-5 at the same temperature.…

Q: Consider the reaction N₂(g) + O₂(g) = 2 NO(g) that has an equilibrium constant, Kc, fof 4.10 x 104…

A: The objective of the question is to find the percentage of O2 that will react to form NO in a given…

Q: While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making,…

Q: For the equilibrium -3 2IBr(g) = I₂(g) + Br₂ (g) K₂ = 8.5 x 107 at 150 °C. If 2.2x10-2 atm of IBr is…

A: Given : Kp = 8.5 x 10-3 atm Initial pressure of IBr(g) = 2.2 x 10-2 atm Volume of vessel = 2.0 L…

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: The reaction mixture below contains 0.305 atm of H2, 0.060 atm of S2, and 0.420 atm of H2S. 2 H2S(g)…

A: Given 2H2S ↔ 2 H2(g) + S2(g)PH2 = 0.305 atmPS2 = 0.060 atmPH2S = 0.420 atm

Q: Suppose 1.000 mol CO and 3.000 mol H2 are put in a 10.00 L vessel at 1200 K. The equilibrium…

A: NOTE : I'm assuming that the equilibrium constant given is concentration equilibrium constant as…

Q: A 3.10 L vessel contains 1.52 mol N2, 1.52 mol H2, and 0.697 mol NH3. What is the direction of…

Q: For the following reaction H₂(g) + 1₂(g) ⇒ 2HI(g) AH° = -10.64 kJ/mol and AS° = 21.48 J/mol K. A…

A: The reaction H2( g) + I2( g) ⇌ 2HI (g) ΔH∘=−10.64 kJ/mol ΔS∘=21.48 J/mol.K =21.48 x10-3…

Q: Consider the following equilibrium: 2NH3(g) N₂ (g) + 3H₂(g) AG = 34. KJ Now suppose a reaction…

A: Answer: In the question a system involving 3 gases is mentioned and we have to find out the…

Q: Determine whether each of the changes below will cause a shift to the left (L), right (R), or no…

A: At a given temperature, if the concentration of any one of the reactants or products is changed,…

Q: While ethanol (CH3CH2OH) is produced naturally by fermentation, e.g. in beer- and wine-making,…

A: Given that,volume of flask = 5.0 LPressure of ethylene gas,PC2H4= 1.0 atmPressure of water vapour,…

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: While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making,…

A: The chemical reaction that occurs in the given conditions is CH2CH2(g) +H2O(g)⇔CH3CH2OH(g)

Question

A 650 mL reaction vessel initially contains 0.0125 mol of H,S at 800 °C. Calculate partial pressure of H, at equilibrium.
2 H2S (g) = 2 H2 (g) + S2(g) Kc = 1.67x107 at 800 °C
1 atm = 760 mmHg = 760 torr = 1.013 bar
R = 0.08206 L atm mol-1 K-1 = 8.314 J mol-1 K-1
31.4 mmHg
16.7 mmHg
33.3 mmHg
46.2 mmHg
62.9 mmHg

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

Trending now

This is a popular solution!

Step by step

Solved in 5 steps with 1 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

Be sure to answer all parts. The equilibrium constant K, for the reaction I(g) 5 21(g) is 3.75 x 10 at 726°C. Calculate K, and Kp for the equilibrium 21(g) S1(g) at the same temperature. K.= X 10 %3D (Enter your answer in scientific notation.) Kp = %3D
You place 4.57 mol of dinitrogen trioxide, N2O3, into a flask, where it decomposes at 25.0°C and 1.00 atm. N2O3(g) NO2(g) + NO(g) What is the composition of the reaction mixture at equilibrium if it contains 0.59 mol of nitrogen dioxide, NO2?N2O3(g) molNO2(g) molNO(g) mol
A gas mixture consists of 3.74 atm of C₂H5Br, 4.22 atm of HBr, 0.11 atm of C₂H6, and 0.882 atm of Br₂. Calculate the reaction quotient for this system prior to the establishment of the equilibrium below. C₂H5Br(g) + HBr(g) = C₂H6(g) + Br₂(g) Report your answer to three significant figures in scientific notation. Submit Answer Tries 0/5
While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 5.0 L flask with 4.9 atm of ethylene gas and 1.9 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 4.27 atm of ethylene gas and 1.27 atm of water vapor. The engineer then adds another 2.5 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. 000 Ar [ atm x10 X S ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check 0 A 1
While ethanol (CH3CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 500. mL flask with 0.77 atm of ethylene gas and 0.98 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.34 atm of ethylene gas and 0.55 atm of water vapor. The engineer then adds another 0.19 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm
4. For the reaction CH4(g) + 2 H2S(g) = CS2(g) + 4 H₂(g) Kc = 3.59 at 900 °C. For each of the following measured concentrations determine whether the reaction is at equilibrium. If not, in which direction will the reaction proceed to get to equilibrium? [CH] [H₂S] [CS₂] [H2] Expt 1 Expt 2 Expt 3 1.15 1.07 1.10 1.20 1.20 1.49 1.51 0.90 1.10 1.08 1.78 1.68
A student ran the following reaction in the laboratory at 479 K: PCI3(g) + Cl₂(g) =PC15(g) When she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of PCI3 was 2.13 atm and the initial partial pressure of Cl₂ was 1.34 atm, she found that the equilibrium partial pressure of PCI5 was 1.12 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp Submit Answer Retry Entire Group 8 more group attempts remaining
As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C
The reaction mixture below contains 0.305 atm of H2, 0.060 atm of S2, and 0.420 atm of H2S. 2 H2S(g) 2 2 H2(g) + S2(g) Kp = 2.4x104 at a particular temperature. Based on the information provided, select the correct relationship. K; the reaction will proceed to form more S2(g). Q > K; the reaction will proceed to the left. O More experimental data are needed to answer a question of this type. Q = K; the reaction is at equilibrium and no change is expected.
Please don't provide handwritten solution ...
this one is asking for atm