How would the series of figures change in the presence of a catalyst? Would there be different amounts of reactantsand products in the final figure (vi) in the presence of a catalyst?Match the words in the left column to the appropriate blanks in the sentences on the right.soonerincreasesbefore equilibriumdecreasesafter equilibriumdoes not changeA catalystand itthe rate of the reaction,the concentration of theproduct at equilibrium conditions.ResetThus, condition (iii) would occurHelpof reactantsconcentration of the productCondition (vi) would show that the concentrationand the CorrectDynamic equilibrium for a chemical reaction is a condition in which the rate of the forward reaction equals therate of the reverse reaction. Equilibrium is reached in a chemical reaction when the concentrations of thereactants and products no longer change.●●●●●●Figure (i) has 10 H₂ molecules and 10 I2 molecules.Figure (ii) has 5 H₂ molecules, 5 I2 molecules, and 10 HI molecules.Figure (iii) has 3 H₂ molecules, 3 I2 molecules, and 14 HI molecules.Figure (iv) has 3 H₂ molecules, 3 I2 molecules, and 14 HI molecules.Figure (v) has 3 H₂ molecules, 3 I2 molecules, and 14 HI molecules.Figure (vi) has 3 H₂ molecules, 3 I2 molecules, and 14 HI molecules.The concentrations of H₂ and I2 in figures (iii), (iv), (v), and (vi) are identical, as are the concentrations ofHI, so the system reached equilibrium at the point represented by figure (iii).

How would the series of figures change in the presence of a catalyst? Would there be different amounts of reactants and products in the final figure (vi) in the presence of a catalyst? Match the words in the left column to the appropriate blanks in the sentences on the right. sooner increases before equilibrium decreases after equilibrium does not change A catalyst and it product at equilibrium conditions. Thus, condition (iii) would occur of reactants Reset the rate of the reaction, the concentration of the Help Condition (vi) would show that the concentration and the concentration of the product

How would the series of figures change in the presence of a catalyst? Would there be different amounts of reactants and products in the final figure (vi) in the presence of a catalyst? Match the words in the left column to the appropriate blanks in the sentences on the right. sooner increases before equilibrium decreases after equilibrium does not change A catalyst and it product at equilibrium conditions. Thus, condition (iii) would occur of reactants Reset the rate of the reaction, the concentration of the Help Condition (vi) would show that the concentration and the concentration of the product

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...

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Why can an equilibrium be represented mathematically? Please explain!
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explain how it can be concluded from the shape of the Job's graph whether a reaction is an equilibrium or it is a complete 1 way reaction.
Consider this equilibrium 4HC1(g) + O₂(g) 2H₂O(g) + 2Cl (g) The equilibrium law expression for the balanced chemical equation would be [HC][0₂]/[H₂O][C1₂] Option 1 2[H₂0][C1₂]/ 4[HC1][0₂] Option 3 [H₂0][C1₂]/HC1][0₂] Option 5 [H₂OF[C1₂ [HCI][0₂] Option 2 [HCI][0₂]/[H₂O1[C1₂F Option 4
2. A catalyst is a substance that increases the rate of a chemical reaction but is not consumed by the reaction. A catalyst works by lowering the activation energy for a reaction, making it easier for reactants to form products. What effect, if any, would a catalyst have on a system already at equilibrium? Briefly explain.
* Question Completion Status: QUESTION 1 Consider the following reversible reaction at equilibrium: 3 H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the reactants (left side)? O Decreasing the amount of NH3. O Adding a catalyst to the system. O Decreasing the volume of the system. O Decreasing the temperature. O Decreasing the amount of H2. QUESTION 2 Click Save and Submit to save and submit. Click Save All Answers to save all answers. arch DELL prt sc FIO DII F9 F8 F3 F4 FS
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One question with 3 parts
In any chemical system at equilibrium, the rate of the forward reaction equals the rate of the reverse reaction. True False