4. Consider an equilibrium mixture of the following chemical reaction : Fe"(aq) + SCN (aq) Fe(SCN)"(aq) yellow colourless deep red (a) Write an expression for the equilibrium constant Kc for the reaction. (b) At a certain temperature, the equilibrium constant Kc for the reaction is 1.08 x 10° dm mol*. The equilibrium mixture is prepared by mixing 20.0 cm of 0.030 M Fe(NO3)3(aq) with 10.0 cm of 0.030 M KSCN(aq) in an acidic medium. Calculate the concentration of Fe(SCN)²*(aq) in the equilibrium mixture at that temperature. (c) It is known that the equilibrium constant Kc increases when temperature increases. Suggest and explain whether the enthalpy change of the reaction is positive, negative or zero.

4. Consider an equilibrium mixture of the following chemical reaction : Fe"(aq) + SCN (aq) Fe(SCN)"(aq) yellow colourless deep red (a) Write an expression for the equilibrium constant Kc for the reaction. (b) At a certain temperature, the equilibrium constant Kc for the reaction is 1.08 x 10° dm mol. The equilibrium mixture is prepared by mixing 20.0 cm of 0.030 M Fe(NO3)3(aq) with 10.0 cm of 0.030 M KSCN(aq) in an acidic medium. Calculate the concentration of Fe(SCN)²(aq) in the equilibrium mixture at that temperature. (c) It is known that the equilibrium constant Kc increases when temperature increases. Suggest and explain whether the enthalpy change of the reaction is positive, negative or zero.

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: We have classified the silver halides like AgBr as insoluble compounds, but in truth, a small amount…

A: a) Solubility product may be defined as the product of concentration of dissolved ions each raised…

Q: K

Q: A mixture of 0.446 M Cl₂, 0.535 M F2, and 0.804 M CIF is introduced to a closed reaction vessel at…

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

Q: 1000oC

Q: Phosphorus pentachloride decomposes according to the chemical equation…

A: Phosphorus pentachloride decomposes into phosphorus trichloride and chlorine gas. The equation for…

Q: 2. Consider the reaction CO(g) CH3OH(g) 2H2(g) A reaction mixture in a 1.00L flask initially only…

A: Initial concentration of CO and H2 and also the concentration of CH3OH at equilibrium can be…

Q: 2NO2(g) = N2O4(8) 25O2(g) + 02(g) = 2S03(g) 2SO2 H2(g) + Cl2(g) = 2HCI3)

Q: Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated…

Q: For the reaction 2 A (g) + B (g) = C(g) + D(s) AH = - 33.0 kJ 1. Initially in a 5.0 L flask at 75°C,…

A: 1. Since, solids do not exert any pressure, so D will not have any pressure. Thus, ICE table for the…

Q: A student ran the following reaction in the laboratory at 586 K: CO(g) + Cl2(g) COCI,(g) When she…

A: Molarity = number of moles/ volume in Litre Molarity of CO = 0.376/1 = 0.376M Molarity of Cl2 =…

Q: A sample of NO decomposes according to the following equation: 2 NO(g) 1 N2(g) + 1 O2(g) An…

Q: The equilibrium constant for the “water gas” reaction: C(s)+H2O(g) CO(g)+H2(g) k=2.6 at…

Q: 5. For the equilibrium Br2(g) 2 Br (g) at 1000 K, K = 4.55. In a 1.00-L flask, 0.012 mol of Br₂ is…

Q: Calculate the value of the equilibrium constant KP for the reaction H2(g) + l2(g) 2HI(g) from these…

A: Equilibrium constant is a constant which represent the ratio of pressure of product to the pressure…

Q: For the following equilibrium system, K = 2.86×10-7 at 298 K. CIO (aq) + H,0 (I) — НСIO (аq) + ОН…

A: This is the concept of equilibrium

Q: Write the expression for the equilibrium constants for the following reactions. FeCl3 (s) Fe+ (aq) +…

Q: reaction, I2(s) + Br2(g) ⇋ 2 IBr(g) is 0.25 at 25 °C. (a) Calculate ΔrG⦵ for this reaction. (b)…

A: Given , I2 (S) + Br2 (g) <-----> 2IBr (g) Kc = 0.25 We have to determine ∆°rG and p(IBr)…

Q: The following reaction has an equilibrium constant, Kc, of 2.20 x 10-2 at a particular temperature:…

A: The equilibrium reaction given is, => 2 ICl (g) → Cl2 (g) + I2 (g)…

Q: Write the Ke and Kp(where applicable) expressions for the following equilibrium reactions: a)…

A: a) The Kc and Kp expressions for the first reaction is shown below, N2O4(g) ⇌2NO2(g) Kc =…

Q: Please don't provide handwritten solution .....

A: The objective of this question is to calculate the equilibrium molarity of CO in a chemical…

Q: Consider the reaction: Xe(g) + 2 F2(g) ⇌ XeF4(g). A reaction mixture initially contains 1.702×103…

A: Given data,Initial pressure of Xe=1702torrInitial pressure of F2=3245torrEquilibrium pressure of…

Q: The equilibrium constant for the reaction H2(g) + I½(s) = 2 HI(g) at 25°C is K = 0.345. (a) If the…

Q: Suppose a 250. mL flask is filled with 1.9 mol of Br,, 1.8 mol of BrOCl and 1.6 mol of BrCl. The…

A: Given: The volume of the flask is 250 mL The number of moles of Br2 is 1.9 mol The number of moles…

Q: Calculate the equilibrium constant Kc for the decomposition reaction from these data.

Q: Consider the reaction: 2 NH3(g) = N₂(g) + 3 H₂(g). At T = 740 K, the equilibrium constant K for this…

Q: At 25°C, the equilibrium constant for the reaction Blg) + Clg) 2A(3) is K,-0.0735.If the three gases…

A: The given Kp value for the reaction at 25°C is 0.0735. To calculate whether the reaction is at…

Q: A chemical engineer is studying the following reaction: HCH3CO2(aq)+CH3NH2(aq) →…

A: HCH3CO2^- (Acetate ion):This is the conjugate base of acetic acid (CH3COOH).In Vessel A, HCH3CO2^-…

Question

100%

4.
Consider an equilibrium mixture of the following chemical reaction :
Fe"(aq) + SCN (aq) – Fe(SCN)³"(aq)
yellow colourless
deep red
(a) Write an expression for the equilibrium constant Kc for the reaction.
(b) At a certain temperature, the equilibrium constant Kc for the reaction is 1.08 x 10° dm³ mol1. The
equilibrium mixture is prepared by mixing 20.0 cm³ of 0.030 M Fe(NO3)3(aq) with 10.0 cm³ of 0.030
M KSCN(aq) in an acidic medium. Calculate the concentration of Fe(SCN)²*(aq) in the equilibrium
mixture at that temperature.
(c) It is known that the equilibrium constant Kc increases when temperature increases. Suggest and
explain whether the enthalpy change of the reaction is positive, negative or zero.
(d) When a little amount of Na,SO3(s) is added to the equilibrium mixture, the colour of the mixture
becomes paler. Explain this observation.

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 by step

Solved in 4 steps with 3 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

SO₂ reacts with Cl₂ to form SO₂Cl₂. The equilibrium constant, Kp, for this reaction is 0.417 at 373 K. 4 SO₂(g) + Cl₂(g) =SO₂Cl₂(g) The standard enthalpy change for this reaction (AH°) is -67.2 kJ/mol. (a) Predict the effect on the production of SO₂Cl₂ when the temperature of the equilibrium system is increased. (b) Use the van't Hoff equation to estimate the equilibrium constant for this reaction at 449 K. Kat 449 K =
The following reaction has an equilibrium constant, Kc, of 2.10 x 102 at a particular temperature: N2 (g) + 3 H2 (g) → 2 NH3 (g) +You have a container in which the concentration of N2 is 0.77 M, the the concentration of H2 is 0.84 M, andthe concentration of NH3 is 0.85 M.(a) Calculate the value of the reaction quotient Q.(b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed toreach equilibrium.
References Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 688 K: 2HI(g) H2(g) + I½(g) When he introduced HI(g) at a pressure of 4.87 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of I2(g) to be 0.510 atm. Calculate the equilibrium constant, K,, he obtained for this reaction. %3D Submit Answer
The equilibrium constant for the following reaction is 67.6 at 232 °C. PCI 3(g) + Cl₂(g) PCI5(g) K = 67.6 at 232 °C Calculate the equilibrium constant for the following reactions at 232 °C. (a) PCI5(g) PCl3(g) + Cl₂(g) K= (b) 2 PCI5(g) 2 PCI3(g) + 2 Cl₂(g) K=
2) For the reaction, PCI:(g) = PCl:(g) + Ch(g) at 327°C, the equilibrium constant, Ke is 0.234. Suppose that 2.082 g PCIIS is placed in an evacuated 200 mL bulb, which is then heated to 327°C. (R = 0.082 L atm mol'K', PCIS = 208.2 g/mol) (a) What would be the pressure of PCIs if it did not dissociate? (b) What is the partial pressure of PCIS at equilibrium? (c) What is the total pressure in the bulb at equilibrium? (d) What is the fraction of PCIS at cquilibrium?
Suppose a 250. mL flask is filled with 1.6 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible: (3)H+(3)0ɔ= (3)0°H+(3)0) The equilibrium constant K for this reaction is 0.735 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. OM
The equilibrium constant, Kc, for the following reaction is 1.20\times 10 - 2 at 500 K. PCl5(g) PCl3(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.331 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K.
10