The reaction 2 H₂O(g) 2 H₂(g) + O₂(g) proceeds at an unspecified temperature until the partial pressures of H₂O, H₂, and O₂ reach 0.015 bar, 0.0080 bar, and 0.0085 bar, respectively. What is the value of the equilibrium constant in terms of partial pressures at this temperature? Kp =

The reaction 2 H₂O(g) 2 H₂(g) + O₂(g) proceeds at an unspecified temperature until the partial pressures of H₂O, H₂, and O₂ reach 0.015 bar, 0.0080 bar, and 0.0085 bar, respectively. What is the value of the equilibrium constant in terms of partial pressures at this temperature? 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: The elementary reaction 2 H₂O(g) 2 H₂(g) + O₂(g) = proceeds at a certain temperature until the…

Q: Consider the equilibrium system described by the chemical reaction below. Calculate the value of Qc…

A: Step by step solution are below

Q: At 25 ∘C25 ∘C, the equilibrium partial pressures for the reaction…

A: The standard change in Gibbs free energy of this reaction is calculated as, ∆G = ∆G° + RT lnQ…

Q: The elementary reaction 2 H,O(g) = 2 H,(g) + 0,(g) proceeds at a certain temperature until the…

A: Answer: Given data: PH2O=0.065barPH2=0.0090barPO2=0.0031bar

Q: HCl, at a pressure of 2.300 bar, and O2, at a pressure of 1.000 bar, are placed in a container.…

A: 4 HCl (g) + O2 (g) → 2 Cl2 (g) + 2 H2O (g) The expression for Kp is, Kp = PCl22 × PH2O2…

Q: For the reaction 3A(g)+3B(g)⇌C(g)3A(g)+3B(g)⇌C(g) Kc�c = 92.0 at a temperature of 289 ∘C∘C .…

Q: 20(g), Rp = 4.3 X 1O For a general reaction: A(g) + 3B( equilibrium mixture of the three gases at…

A: Find partial pressure of C....

Q: 8. Suppose 1.00 atm of SO2 and 2.00 atm of NO2 are combined in an empty container. Using the…

A: At equilibrium , equilibrium constant is the ratio of pressure of product at equilibrium to the…

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

A: Given that : Initial pressure of CO(g)=4.8 atmInitial pressure of H2O(g)=1.3 atm At equilibrium,…

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

A: Reaction quotient (Q) tells us about the amount of reactants and products present in a reaction…

Q: Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist…

Q: The equilibrium constant for the equilibrium CO (g) +H 2 O (g) =CO 2(g) +H 2(g) ) is 302 at 600K.…

A: If the equilibrium constant for a general reversible reaction A + B ↔ C + D is K Then , the…

Q: For the ammonia formation reaction, N2 (g) + 3H2 (g) 2 NH3(g) The equilibrium constant Kc, is 2.4 x…

A: The equilibrium constant(Kc) for a reaction is the ratio of the equilibrium concentrations of the…

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

A: Given,

Q: The equilibrium constant for the chemical equation N₂(g) + 3 H₂(g) — 2 NH₂ (g) is Kp = 0.557 at 277…

A: The reaction given is N2 (g) + 3 H2 (g) ------> 2 NH3 (g)Since the relationship between Kp and Kc…

Q: Nitrogen and Hyd eact to nd, like this. N₂(g)+3H₂(g)2NH3(g) The reaction is exothermic. Suppose a…

Q: An air sample with an N2, O2 molar ratio of 79:21 was heated to 2500 K. When the equilibrium is…

A: Given N2 (g) + 02 (g) -----> 2NO(g) The mole percentage of NO is determined to be 1.8% 2[NO] =…

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

A: Step 1:Step 2:Step 3:

Q: At a certain temperature, the given reaction has an equilibrium constant of K, = 399. PCI, (g) + Cl,…

A: The given data contains, Initial pressure = 0.0210 bar. Kp = 399 Kp' = 1 / Kp = 1 / 399 =2.50 x…

Q: In a 3.0 L vessel the following equilibrium partial pressure are measured: N2= 90 torr, H2= 317…

A: The equilibrium reaction is given as: N2g + 3H2g ⇌ 2NH3g At equilibrium, the partial pressures are…

Q: The equilibrium constant in terms of pressure, Kp, for the following process is 0.144 at 72 °C. It…

Q: The equilibrium constant for dissociation of dinitrogen tetroxide N2O4(g) ↔ 2 NO2(g) is KP =…

A: Given, KP = 0.308763 Ptot = 0.86 bar Where, Ptot is total equilibrium pressure.

Q: At 100 oC, Keq = 1.5E8 for the reaction:CO(g) + Cl2(g) COCl2(g)Using appropriate approximation,…

A: According to law of mass action, The concentration of reactant is increases with increase in…

Q: For the reaction 3A(g) + 2B(g) = C(g) K. = 29.8 L4 mol-4 at a temperature of 235 °C. Calculate the…

Q: At 2000 K the partial pressures of an equilibrium mixture of H2S, H2, and S are 0.0353,0.0371, and…

A: The balanced reaction is given as H2S(g) <====> H2(g) + S(g) According to law of chemical…

Q: Phosphorus pentachloride decomposes according to the chemical equation…

A: PCl5(g)↽−−⇀PCl3(g)+Cl2(g) Kc=1.80 at 250 ∘C Moles of PCl5 =0.1974 mol…

Q: Calculate the equilibrium constant K given the following information: The initial pressure of A is…

A: Initial pressure of A = 2.755 bar Initial pressure of B = 3.968 bar Equilibrium pressure of C =…

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

A: The equilibrium constant of the reaction may be calculated as:

Q: At 25.0 °C, the reaction CO2(g) + H2O(l) ⇔ H+(aq) + HCO3-(aq) is at equilibrium when PCO2 = 3.50…

A: Given: PCO2 = 3.50 mbar [H2O] = 55.5 mol L-1 [H+] = 39.8 µmol L-1 [HCO3-] = 1.28 mmol L-1

Q: A mixture of 1.00 mol NaHCO3(s) and 1.00 mol Na2CO3(s) is introduced into a 2.50 L flask in which…

A: A reversible reaction is a type of reaction where the reactant to form product either by combination…

Q: The equilibrium A(g) + B(g) - 2 C(g) has an equilibrium constant of 623.5. If the reaction is…

A: Given data : Equilibrium constant (Kp) = 623.5 PA = 0.150 bar PB = 0.150 bar PC = 22.4 bar

Q: The pressure-based equilibrium constant for the reaction shown below is Kp = 0.974 at 357 ℃. What is…

Q: 4PC13 (1) 2. P4 (s) + 6C12 (g) Calculate the Kc for this reaction if Kp is equal to 3.76 x 10³ at…

A: Dear student , since you have posted multiple questions we are allowed to solve only first…

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

Q: For the reaction: 2 A (g) + B (s) = 2C (s) + D (g) At 298 K in a 10.0 L vessel, the equilibrium…

A: o find the equilibrium constant KpK_pKp for the reaction:2A(g)+B(s)⇌2C(s)+D(g) we start by noting…

Q: The equilibrium constant for dissociation of dinitrogen tetroxide N2O4(g) ↔ 2 NO2(g) is KP =…

A: Given Kp = 0.308763 Total equilibrium pressure Ptotal = 0.86 bar Chemical equation…

Q: 10) Consider the following reaction at 35.0 °C: kJ 2 NOCI(g) → 2 NO(g) + Cl₂ (g) AGº = 20.0 rxn rxn…

A: The reaction is: Temperature = Partial pressure of NOCl = 2.0 atmR = 8.314 J/(mol.K)We have to…

Q: Consider the equilibrium system described by the chemical reaction below. Calculate the value of Qc…

A: Given, volume of the solution= 4 L mass of CO =26.4 g, mass of H2= 6.35 g, mass of CH3OH = 22.1 g…

Question

The reaction
2 H₂O(g) 2 H₂(g) + O₂(g)
proceeds at an unspecified temperature until the partial pressures of H₂O, H₂, and O₂ reach
0.015 bar, 0.0080 bar, and 0.0085 bar, respectively. What is the value of the equilibrium constant in terms of partial pressures at
this temperature?
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

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 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

Consider the chemical equation and equilibrium constant for the formation of ammonia gas; N2(g) + 3 H2(g) ↔2 NH3(g), K = 3.7 x 108 at 25 °CDetermine the equilibrium constant at 25 °C for the reaction NH3(g) ↔ 0.5 N2(g) + 1.5 H2(g).
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 =
Consider the equilibrium: H₂(g) + CO₂(g) ≥ CO (g) + H₂0 (g) 1.59 at 1290 Kelvin. Calculate Ar Gº for this reaction. where Kp = Imagine you fill a reaction vessel with the following pressures: PH₂ = 0.25 bar; Pco₂ 0.25 bar; Pco = 0.66 bar; PH₂0 = 0.66 bar Calculate AG at these conditions. Does the reaction need to go forward or in the reverse direction to achieve equilibrium? Finally, calculate the equilibrium pressures of each gas in bars.
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 = _____ .
For the reaction X(9) + 4Y(g) = 3Z(g) K, = 2.51 × 10-2 bar-2 at a temperature of 361 °C. Calculate the value of Kc. Express your answer numerically.
Consider the following reaction:CH3OH(g) CH2O(g) + H2(g) K = 3.29 x 10−11a. If 14.4 g of CH3OH(g) is added to a 1.50 L container at 298 K, calculate the equilibriumconcentrations of all gases b. Without doing any calculations, predict what happens if the reaction is put in a 2.00 Lcontainer instead of a 1.50 L container. c. . Without doing any calculations, predict what happens if H2SO4 (a catalyst) is added
calculate the value of the reaction quotient. determine is the system is at equilibrium. if not which direction must the reaction proceed to reach equilibrium
The equilibrium constant, K., is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation K₂ = K. (RT)An where R = 0.08206 L-atm/(K-mol), T is the absolute temperature, and An is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N₂(g) + 3H₂(g) = 2NH3(g) for which An=2-(1+3) = -2.
Consider the reaction: 2 NO(g) + Br₂(g) ⇌ 2 NOBr(g) A chemist placed 0.0322 mol of NO and 1.70 g of bromine (Br₂) into a sealed 1.00 L reaction vessel and then allowed the reaction to reach equilibrium. The pressure of the NOBr at equilibrium at 25.0°C is 0.444 bar. (R = 0.08314 L･bar/mol･K and MW of Br₂ is 159.808 g/mol.) Calculate the Kp.
The formation of ammonia gas from molecular nitrogen and molecular hydrogen gas has the following Kp value. Get the value for the reverse reaction.
At high temperature, HCl and O2 react to give Cl2 gas: 4HClg) + O2(g) ⇌ 2 Cl2 (g) + 2H2O(g) If HCl at 2.30 bar and O2 at 1.00 bar react at 750K, the equilibrium pressure of Cl2 is measured to be 0.93 bar. Determine the value of Keq at 750 K. Use a systematic approach to include setting up an ICE table, constructing equilibrium constant expression and show calculation involved.
Calculate the reaction quotient, QR for the following reactions and conditions: 2 NOCl(g) : KP = 2.5 x 103; PNO = 0.0032 atm; PCl2 = 0.023 atm; PNOCl = 0.210 atm 2 NH3(g) N2(g) + 3H2(g) : KP = 17.0; PNH3 = 0.13 atm; PN2 = 0.34 atm; PH2 = 1.1 atm