Explanation Given The rate constant for the reaction is 3.5 × 10 − 2 M − 1 ⋅ s − 1 . At a given time, the concentration of H 2 S is 2.0 × 10 − 4 M . At a given time, the concentration of Cl 2 is 0.025 M . It is given that rate of the reaction is first order in each reactant. The rate of a reaction at a given time is calculated by the formula, Rate = k [ H 2 S ] [ Cl 2 ] Where, Rate is the rate of the reaction at the given time. k is the rate constant for the reaction. [ H 2 S ] is the concentration of H 2 S at the given time. [ Cl 2 ] is the concentration of Cl 2 at the given time. Substitute the value of k , [ H 2 S ] and [ Cl 2 ] in the above equation. Rate = 3.5 × 10 − 2 M − 1 ⋅ s − 1 × 2

Chemistry: The Central Science (14th Edition)

14th Edition

ISBN: 9780134414232

Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus

Publisher: PEARSON

See similar textbooks

Question

Chapter 14, Problem 90AE

Interpretation Introduction

To determine: The rate of formation of Cl− at a given time.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Chapter 14, Problem 89AE

Chapter 14, Problem 91AE

Students have asked these similar questions

a) A favorable entropy change occurs when ΔS is positive. Does the order of the system increase or decrease when ΔS is positive? (b) A favorable enthalpy change occurs when ΔH is negative. Does the system absorb heat or give off heat when ΔH is negative? (c) Write the relation between ΔG, ΔH, and ΔS. Use the results of parts (a) and (b) to state whether ΔG must be positive or negative for a spontaneous change. For the reaction, ΔG is 59.0 kJ/mol at 298.15 K. Find the value of K for the reaction.

A sample of hydrated magnesium sulfate (MgSO4⋅xH2O) is analyzed using thermogravimetric analysis (TGA). The sample weighs 2.50 g initially and is heated in a controlled atmosphere. As the temperature increases, the water of hydration is released in two stages: (a) The first mass loss of 0.72 g occurs at 150°C, corresponding to the loss of a certain number of water molecules. (b) The second mass loss of 0.90 g occurs at 250°C, corresponding to the loss of the remaining water molecules. The residue is identified as anhydrous magnesium sulfate (MgSO4) Questions: (i) Determine the value of x (the total number of water molecules in MgSO4⋅xH2O) (ii) Calculate the percentage of water in the original sample. Write down the applications of TGA.

The solubility product of iron(III) hydroxide (Fe(OH)3) is 6.3×10−38. If 50 mL of a 0.001 M FeCl3 solution is mixed with 50 mL of a 0.005 M NaOH solution, will Fe(OH)3 precipitate? Show all step-by-step calculations. To evaluate the equilibrium constant, we must express concentrations of solutes in mol/L, gases in bars, and omit solids, liquids, and solvents. Explain why.

Chapter 14 Solutions

Chemistry: The Central Science (14th Edition)

Ch. 14.2 - If the experiment in Figure 14.2 is run for 60 s,...Ch. 14.2 - Prob. 14.1.2PE Ch. 14.2 - Which of the following could be the instantaneous...Ch. 14.2 - Using Figure 14.3, determine the instantaneous...Ch. 14.2 - At a certain time in a reaction, substance A is...Ch. 14.2 - Prob. 14.3.2PE Ch. 14.3 - Suppose the rate law for the reaction in this...Ch. 14.3 - Assuming that rate = k[A][B], rank the mixtures...Ch. 14.3 - Prob. 14.5.1PE Ch. 14.3 - Prob. 14.5.2PE

Knowledge Booster

The rate of formation of Cl − at a given time.

To determine: The rate of formation of Cl− at a given time.

Want to see the full answer?

Chapter 14 Solutions