Consider the following reaction at equilibrium, C(s) + H2O (g) = CO(g)+ H, (g) ΔΗ 131 %3| 30 kJ [CO][H2] [H2O] If the equilibrium constant expression is, K 1. What will happen to the concentration of each reactant and product at equilibrium if more solid carbon, C, is added?

Consider the following reaction at equilibrium, C(s) + H2O (g) = CO(g)+ H, (g) ΔΗ 131 %3| 30 kJ [CO][H2] [H2O] If the equilibrium constant expression is, K 1. What will happen to the concentration of each reactant and product at equilibrium if more solid carbon, C, is added?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 118QRT

See similar textbooks

Related questions

Q: Nitrosyl bromide, NOBr, decomposes according to the equation NOBR(g) NO(g) + 1/2 Br2(g) where AG° at…

A: The free energy change of the reaction is = 9.83 kJ/mol = 9.83x103 J/mol The temperature of the…

Q: Consider the equilibrium system: 2ICl(s) ⇌ I2(s) + Cl2(g), the Kc expression for the reaction is?

A: Kc is expressed as the ratio of the product of concentration of products and concentration of…

Q: what is the value of Kc at this temperature?

Q: Consider the following reaction where ΔH° = -103.8 kJ/mol. H2(g) + Br2(g) 2 HBr(g) In a particular…

A: Given: The given reaction is, Volume of reaction flask – 1.00 L Equal moles of reactants are…

Q: The equilibrium constant (K1) for the reaction CO2 (g) 2 CO(g)+1/2 O2(g) is 6.66 x 10-12 at 1000 K.…

Q: using the reaction CO(g) + 2 H2(g) ↔ CH3OH(g) Calculate the equilibrium constant at 298 K.…

A: Equilibrium constant can be defined as the ratio of concentration of products to concentration of…

Q: Construct the expression for Kp for the following reaction. 2 O:(g) = 3 O2(g) 1 Drag the tiles into…

A: A reversible chemical reaction can move in either forward or backward direction. The stage of a…

Q: *Xog pəpIAojd For reactions carried out under standard-state conditions, the equation AG=AH- TAS…

A: This problem can be solved by using the given integrated Arrhenius equation as follows :

Q: What is the correct expression for the equilibrium constant (K) for the reaction between carbon and…

A: Equilibrium constant (Kc) in terms of concentration can be defined as the ratio of concentration of…

Q: 1. Consider the equilibrium N;O4 (g) = 2NO, (g) AH° = 58.0 kJ In which direction will the…

A: Since you have posted multiple questions, we will solve first question for you. To get remaining…

Q: The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K. 2CH,Cl,(g)CH,(g) -…

A: We know that : ln[(Kp)2/(Kp)1] = ∆H/R[1/T1 - 1/T2] ...(1) Here, (Kp)1 = ?, (Kp)2 = 10.5, T1 = 231…

Q: For the reaction, H2(g) + CO(g) > CH3OH(g), hydrogen gas and carbon monoxide gas reacting to form…

A: Given: H2(g) + CO(g)<-----> CH3OH (g) ∆H = -90.2 kJ/mol

Q: Phosphoryl chloride, POCI3(g), is used in the manufacturing of flame retardants. It is manufactured…

A: Given: At 298 K, the equilibrium concentration of POCl3 was 0.68 mol/L, the concentration of NO was…

Q: Carbon reacts with sulfur to form carbon disulfide according to the following reaction. C(s) + 2…

Q: At 1500 °C the equilibrium constant for the reaction CO(g) + 2H₂(g) CH₃OH(g) has the value Kp = 1.4…

A: Given reaction: CO(g) + 2H₂(g) ⇌ CH₃OH(g) Kp = 1.4 x 10⁻⁷ We have to calculate ΔG° for this…

Q: For which one of the following reactions are Kç and K, the SAME? O 2 CO (g)C (s) + CO2 (g) O H2 (g)…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: A mixture of gaseous CO and H2, called synthesis gas, is used commercially to prepare methanol…

A: A mixture of gaseous CO and H2, called synthesis gas, is used commercially to prepare methanol…

Q: Ethane can be formed by reacting acetylene with hydrogen. C,H,G) + 2H,(9) C,H,(g) DHn = -311 kJ At…

A: According to lechatier's principle •If number of moles at reactant side is more 》 low pressue =…

Q: Consider the equilibrium reaction 2 NO2(g) N2O4(g). A sample of pure NO2(g) of concentration…

A: Given: The initial concentration of NO2 is 0.140 M. At equilibrium, 57.0 % of the NO2(g) has reacted…

Q: Write the equilibrium-constantexpression and calculate the value of the equilibrium constant and the…

A: The formula to calculate the ΔG°f is shown below.

Q: Consider the reaction: H2(g) + Br2(g) --> 2HBr(g) ΔH˚ = -103.8 kJ/mol In a particular experiment,…

Q: For the reaction 2 SO2(g) + O2(g) → 2 SO3(g), the standard enthalpy of reaction ARH° is -197.8 kJ,…

A: For the given reaction- 2SO2g + O2g → 2SO3g The…

Q: Calculate the equilibrium constant, Keq, at 25 °C for the following reaction if ΔGfo for methanol is…

Q: An endothermic reaction (AHrxn = +125 kJ) has a Kc of 4.61 x 103 at 25.0 °C. What is its equilibrium…

Q: Calculate ΔG° for each of the following reactions from the equilibrium constant at the temperature…

A: The two factors commonly employed in spontaneity prediction of reactions are the equilibrium…

Q: The equilibrium constant, Kp , has a value of 7.5 x 10-4 at 222 K for the reaction of nitrogen…

A: given temperature = 222 K kp = 7.5 × 10-4

Q: A mixture of gaseous CO and H2, called synthesis gas, is used commercially to prepare methanol…

A: A reversible chemical reaction can move in either forward or backward direction. The stage of a…

Q: Consider the chemical system CO + Cl2 « COCl2; K = 4.6 x 109. If the concentration of the…

A: Equilibrium constant will not change by the change in concentrations of product formed in the…

Q: For the decomposition of silver oxide, at 298 K and 1 atm, according to the chemical equation:…

A: We have to calculate the ∆G and temperature

Q: Balance the equation and write the reaction quotient expression, Qc, for the following synthesis of…

A: Balanced Reaction CH4 (g) + 2H2S(g) ⇌ CS2 (g) + 4H2 (g)

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

A: First calculate the moles of each species in the reaction: Moles of SO2Cl2 = Mass/Molar mass =…

Q: For the reaction N2(g) + 3 H,(g) = 2 NH;(g) a reaction mixture at a certain temperature contains N,,…

A: Qp < Kp ; the reaction will proceed to the right.

Q: 12. For the following reaction at equilibrium in a closed container, AH = 128 kJ 2 NaHCO3 (s) =…

A: The solution is as follows:

Q: Consider the reaction, 2 SO3(g) ⇌ 2 SO2(g) + O2(g) where ∆H° = 198 kJ/mol at 25°C. If the…

Q: The equilibrium constant, Kp, is 5.04 x 1017 at 250C for the following reaction.…

Q: Consider the following chemical equation and equilibrium constant at 25°C: z COFZ (g) = cO2 lg) +…

Q: 17.13 Balance each reaction and write its reaction quotient, Q.: (a) C,H6(g) + O2(g) = CO2(g) +…

A: Balancing of chemical reaction: It is the process of writing the coefficients (numbers) for the…

Q: 1a.At 100 C, Kp = 6.5 x 10-2 for the reaction: 2NO2(g) ⇌ N2O4 (g). What is Kc? 1b.For the…

Q: For the reaction (NH4)2S (s) = N2 (g) + H2S (g) + 3 H2 (g), the expression for Kc is

A: Given ; (NH4)2S(s) <-----> N2(g) + H2S(g) + 3H2(g) To write :- Expression for Kc

Q: what is the value of Kc of the reaction at this temperature?

Q: The equilibrium constant Kp for the reaction: 2SO3 (g) 2 2SO2(g)+ O2(g) 1.8 x 10 at 350°C. What is…

A: 2SO3(g) ⇌ 2SO2(g) + O2(g) Kp = 1.8 × 10-5 Temperature = 350°C

Q: If two reactions sum to an overall reaction, and the equilibrium constants for the two reactions are…

A: If two reactions sum to an overall reaction, then the equilibrium constant of the overall reaction…

Q: If the exothermic reaction 2H2(g)+O2(g)→2H2O(g) has reached equilibrium, what is the effect of…

Q: Consider the following reaction at equilibrium, C(s) + H2O (g) = CO(g)+ H2 (g) ΔΗ .30 kJ [CO][H2]…

A: This can be answered by Le Chatelier's principle.

Q: Consider the following reaction at equilibrium: A (g) = 2B (g) From the data shown below, calculate…

Q: 2. This reaction has an equilibrium constant of K, = 2.2 x 10 at 298K. %3! 2 COF, (g) + C02 (g) +…

A: Kp for reaction (a),…

Q: The equilibrium constant of a reaction triples on raising the temperature from 289°C to 371°C.…

A: According to Arrhenius equation- K =A e-Ea/RT on taking log and at different temperatures,…

Q: If a chemical reaction has AG°298 -29.4 kJ, what is the equilibrium constant Keg at 298 K? O 7.0 x…

Question

100%

Consider the following reaction at equilibrium,
C(s) + H2O (g) = CO (g)+ H2 (g)
ΔΗ=131
. 30 kJ
[CO][H2]
[H2O]
If the equilibrium constant expression is, K =
1. What will happen to the concentration of each reactant and product at
equilibrium if more solid carbon, C, is added?

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

Analysis

VIEW

Explanation

VIEW

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

Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) Suppose you place 2.00 mol NOC1 in a 1.00–L flask, seal it, and raise the temperature to 462 °C. When equilibrium has been established, 0.66 mol NO is present. Calculate the equilibrium constant Kc for the decomposition reaction from these data.
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
Consider the following hypothetical reactions and their equilibrium constants at 75C, 3A(g)3B(g)+2C(g)K1=0.31 3D(g)+2B(g)2C(g)K1=2.8 Find the equilibrium constant at 75C for the following reaction A(g)D(g)+53B(g)
Consider the following equilibria involving SO2(g) and their corresponding equilibrium constants. SO2(g) + 12 O2(g) SO3(g) K1 2SO3(g) 2SO2(g) + O2(g) K2 Which of the following expressions relates K1 to K2? (a) K2=K12 (b) K22=K1 (c) K2 = K1 (d) K2 = 1/K1 (e) K2=1/K12
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.
The equilibrium constant Kc for the synthesis of methanol, CH3OH. CO(g)+2H2(g)CH3OH(g) is 4.3 at 250C and 1.8 at 275C. Is this reaction endothermic or exothermic?
At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?
12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?
Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.