Please don't provide handwriting solution The plot below shows the masses of product and reactant present in a reversible reaction as afunction of time. Which statements correctly describe this reaction? [Select all that apply.]masstimereactantproductThe rate of conversion of product to reactant increases as the reaction progresses.The reaction started with 100% reactant.The rate of conversion of reactant to product increases as the reaction progresses.The reaction reaches equilibrium.The reactant is favored at equilibrium.

We are given here a plot of mass vs time of a reversible reaction. We have to select the correct…

The plot below shows the masses of product and reactant present in a reversible reaction as a function of time. Which statements correctly describe this reaction? [Select all that apply.] mass time reactant The reactant is favored at equilibrium. product The rate of conversion of product to reactant increases as the reaction progresses. The reaction started with 100% reactant. The rate of conversion of reactant to product increases as the reaction progresses. The reaction reaches equilibrium.

The plot below shows the masses of product and reactant present in a reversible reaction as a function of time. Which statements correctly describe this reaction? [Select all that apply.] mass time reactant The reactant is favored at equilibrium. product The rate of conversion of product to reactant increases as the reaction progresses. The reaction started with 100% reactant. The rate of conversion of reactant to product increases as the reaction progresses. The reaction reaches equilibrium.

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter17: Chemical Equilibrium

Section: Chapter Questions

Problem 85A

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The boxes shown below represent a set of initial conditions for the reaction: Draw a quantitative molecular picture that shows what this system looks like after the reactants are mixed in one of the boxes and the system reaches equilibrium. Support your answer with calculations.
. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
The boxes shown below represent a set of initial conditions for the reaction: Draw a quantitative molecular picture that shows what this system looks like after the reactants are mixed in one of the boxes and the system reaches equilibrium. Support your answer with calculations. Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the foll owing equation: A+BC+D a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. b. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
Classify each of the following statements as true or false. aSome equilibria depend on a steady supply of a reactant in order to maintain the equilibrium. bBoth forward and reverse reactions continue after equilibrium is reached. cEvery time reactant molecules collide, there is a reaction. dPotential energy during a collision is greater than potential energy before or after the collision. eThe properties of a transition state are between those of the reactants and products. fActivation energy is positive for both the forward and reverse reactions. gKinetic energy is changed to potential energy during a collision. hAn increase in temperature speeds the forward reaction but slows the reverse reaction. iA catalyst changes the steps by which a reaction is completed. jAn increase in concentration of a substance on the right-hand side of an equation speeds the reverse reaction rate. kAn increase in the concentration of a substance in an equilibrium increases the reaction rate in which the substance is a product. lReducing the volume of a gaseous equilibrium shifts the equilibrium in the direction of fewer gaseous molecules. mRaising temperature results in a shift in the forward direction of an endothermic equilibrium. nThe value of an equilibrium constant depends on temperature. oA large K indicates that an equilibrium is favored in the reverse direction.
Consider the following equilibrium system. N2(g)+O2(g)2NO(g) a. Write the chemical equation for the forward reaction. b. Write the chemical equation for the reverse reaction.
What happens to the reactants in an ineffective molecular collision?
. Before two molecules can react, chemists envision that the molecules must first collide with one another. Is collision among molecules the only consideration for the molecules to react with one another?
When writing a chemical equation for a reaction that comes to equilibrium. how do we indicate symbolically that the reaction is reversible?
. Consider the following exothermic reaction at equilibrium: N2(g)+3H2(g)2NH3(g)Predict how the following changes affect the number of moles of each component of the system after equilibrium is re-established by completing the table. Complete the table with the terms increase, decrease, or no change. N2 H2 NH3 Add N2(g) Remove H2(g) Add NH3(g) Add Ne(g) (constant V) Increase the temperature Decrease the volume (constant T) Add a catalyst
. For the reaction system C(s)+H2O(g)H2(g)+CO(g)which has already reached a state of equilibrium, predict the effect that each of the following changes will have on the position of the equilibrium. Tell whether the equilibrium will shift to the right, will shift to the left, or will not be affected. a. The pressure of hydrogen is increased by injecting an additional mole of hydrogen gas into the reaction vessel. b. Carbon monoxide gas is removed as it forms by use of a chemical absorbent or “scrubber.” c. An additional amount of solid carbon is added to the reaction vessel.