chem!!

Question:
1. The value of the equilibrium constant for the reaction

H2CO3(aq) + energy ƒnƒnH2O(l) + CO2(g)

can be changed by introducing a change to which component of the equation?

This relates to the Le Chatelier principle.
Thanks!


Keq (the constant itself) changes only with temperature. Which component could you change that would change the temperature?


Probably the side the energy is on. So I would put the energy on the other side. Would that be right?


no. Adding energy in th form of heat or taking heat away in the form of cooling it will change the termperature and that will change Keq. You can't just move the energy from one side to the other without some justification because it's already set and the equation tells us that the reaction is endothermic; i.e., it requires energy to make it do what the equation says it does. I hope this helps. From your answer I don't think you have a good understanding of Le Chatelier's Principle; therefore, I recommend that you reread that section of your text and/or notes (or both) and work some of the problems at the end of the chapter. By all means look at the solved problems (examples) in the text. After doing that, repost with specific questions that you don't understand and perhaps we can help you work through those questions.

  1. 👍
  2. 👎
  3. 👁

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    Concerning the following reaction at equilibrium: 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g), increasing the concentration of the Fe(s) would: Answer A. Shift the equilibrium to the right B. Shift the equilibrium to the left C. No change

  2. chemistry

    What information does an equilibrium constant give about a reaction? A. It tells how long it takes the reaction to reach equilibrium. B. It tells how much energy is required for the reaction to happen. C. It tells what the rate

  3. Chemistry

    Given the two reactions 1.PbCl2 Pb^2+ + 2 Cl^-, K1= 1.82×10^−10 2. AgCl Ag^+ + Cl^-, K2 = 1.15×10−4 what is the equilibrium constant Kfinal for the following reaction? PbCl2+ 2 Ag^+ 2AgCl+ Pb^2+ This is what i have soo far:

  4. Chemistry

    This is a problem I got on my Mastering Chemistry homework: Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture at equilibrium at 175 K contains PH2=0.958atm, PI2=0.877atm, and PHI=0.020atm. A second reaction

  1. chemistry

    Carbon dioxide (CO2) reacts with water (H2O) to form carbonic acid (H2CO3). Which equation demonstrates the law of conservation of matter for this reaction? A. 2 CO + H2O —> H2CO3 B. CO2 + H2O —> H2CO3 C. CO2 + 2 H2O —> 2

  2. Chemistry

    Need help in AP chemistry on Equilibrium When heated, hydrogen sulfide gas decomposes according to the equation 2 H2S(g) ⇄ 2 H2(g) + S2(g) A 3.40 g sample of H2S(g) is introduced into an evacuated rigid 1.25 L container. The

  3. Chemistry

    A chemist trying to synthesize a particular compound attempts two different synthesis reactions. The equilibrium constants for the two reactions are 23.3 and 2.2 X 10^4 at room temp. However, after 15minutes the chemist finds that

  4. Chemistry

    What is the equilibrium constant for H2CO3(aq)->2H+(aq)+CO3-2(aq)

  1. Chemistry

    At a given temperature, the elementary reaction A B in the forward direction is first order in A with a rate constant of 2.60 x 10^-2 s^-1. The reverse reaction is first order in B and the rate constant is 8.50 x 10^-2 s^-1. What

  2. Chemistry

    H2(g) + I2(g) 2 HI(g) The forward reaction above is exothermic. At equilibrium, what happens if I2 is removed from the reaction mixture at constant temperature and volume? select all that apply 1.) Energy is absorbed 2.) Energy is

  3. chemistry

    What effect does raising the temperature of the reaction chamber at a constant pressure have on the following reaction at equilibrium? 2NO2(g) N2O4(g) + heat A. The equilibrium shifts toward the reactants because the reverse

  4. chem

    Given the concentrations, calculate the equilibrium constant for this reaction: I2(g) + Cl2(g)---> 2ICl(g) At equilibrium, the molar concentrations for reactants and products are found to be I2 = 0.50M, Cl2 = 0.60M, and ICl =

You can view more similar questions or ask a new question.