CHM 101L M5 Equilibrium and LeChatlier Lab Report

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When a product is added as a stressor on equilibrium, there is a(n): Group of answer choices increase in the forward reaction rate decrease in the forward reaction rate increase in the reverse reaction rate decrease in the reverse reaction rate

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Fill in the blanks of the potential/kinetic energy diagram

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According to Le Chatelier's Principle, a reaction at equilibrium will attempt to stay at equilibrium, even if stresses are applied. Which of the following is NOT a stress that chemical reactions respond to?        A decrease in the concentration of an aqueous or gaseous reactant.       A change in temperature.       An increase in the concentration of an aqueous or gaseous product.       A change in pressure when gaseous reagents are nonexistent.       A change in pressure when gases are present in differing mole amounts on each side of the equation.

According to Le Chatelier's Principle, a reaction at equilibrium will attempt to stay at equilibrium, even if stresses are applied. Which of the following is NOT a stress that chemical reactions respond to? A) A change in pressure when gaseous reagents are nonexistent.   B) A change in temperature.   C) An increase in the concentration of an aqueous or gaseous product.   D) A decrease in the concentration of an aqueous or gaseous reactant.   E) A change in pressure when gases are present in differing mole amounts on each side of the equation.

Which one shows an exothermic reaction? Both are exothermic II Neither are exothermic I

Pre-lab question #1: A brief explanation/overview of LeChatelier's Principle: If a system at equilibrium is disturbed, the equilibrium will shift to minimize the disturbing influence. True False

Adding heat to a reversible endothermic reaction at equilibrium will _________.   decrease the amount of product   increase the amount of reactants   shift the equilibrium to the left   all of the above   none of the above

For the reaction below, an increase in gas pressure will ____ N2    +     3H2         <-->          2NH3   a. cause an increase in the concentration of N2   b. have no effect on reactants or products   c. cause an increase in the concentration of H2   d. cause an increase in the concentration of NH3

H PAP Cheistry-29 X PAP Chemistry-29 X G diagram showing x b ar-2903012.agilixbuzz.com/student/135113422/activity/c412d902 Mastery Assess It 8 PAP Chemistry-2903012-42100P-1/ Le Chatelier's Principle /Lesson 128 1. Which of the following would not add stress to an equilibrium reaction shown below? A+B+C+D increasing the pressure removing product C changing the order of reactants A and B adding reactant A

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Which of the following typically increase the rate of a reaction?   Pick all correct responses.   A. Removal of an appropriately designed catalyst   B. Addition of an appropriately designed, and chosen, catalyst   C. Fluctuation in reaction pressure   D. Increase in the initial concentration of the chemical reagents   E. Increase in reaction temperature

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Which one of the following factors DOES NOT affect the rate of a chemical reaction? concentration     C. temperature humidity D. nature of the reactants .The rate of a chemical reaction normally _______________________. increases as temperature decreases decreases when a catalyst is added increases as reactant concentration increases decreases as reactant concentration increases

A. Using the Le Chatelier’s principle, predict the shift in the direction of the equilibrium position and changes that will be observed (e.g. color) in each of the following equilibria when the indicated condition is applied.

Le Chatelier's Principles Complete the following chart by writing left, right or none for equilibrium shift, and decreases, increases or remains the same for the concentrations of reactants and products, and for the K value. N2(g) + 3H2(g) ↔2NH3(g) + 22.0 kcal Stress Equilibrium Shift [N2]  [H2]  [NH3]  K Add N2           Add H2           Add NH3           Remove N2           Remove H2           Remove NH3           Increase Temperature            Decrease Temperature            Increase Pressure            Decrease Pressure

For each organic reaction, say whether at equilibrium there will be more reactants than products (so equilibrium lies to the left), or more produ than reactants (so equilibrium lies to the right). You'll probably find some useful information in the ALEKS Data resource. H3N. OH OH + OH O left + Nha O left + H₂O O left + CH3O O left CI right O HO right O H₂N. right right ► + H₂O + NH3 + H30 + CH3OH X

1. For a solution equilibrium, if the concentration of a product is decreased, Kc will also decrease. Group of answer choices True False   2. Which of the following is the factor that causes a reversible chemical reaction to reach equilibrium? Group of answer choices Reaction stopped. The forward and reverse reaction rates become equal. the concentrations of the reactants and products have become equal. Reactants are used up.

Le Châtelier Principle Learning Goal: To use the equilibrium constant and Le Châtelier's principle to determine how a reaction will respond to external factors. A reaction is at equilibrium when the concentrations of the reactants and products no longer change over time. This does not mean the reaction is over, rather, two competing reactions continue to occur simultaneously at equal rates. The two competing reactions are the forward reaction (reactants → products) and the reverse reaction (products → reactants). If a reaction at equilibrium is subjected to a stress, the concentrations of reactants and products adjust to reestablish equilibrium. This is called Le Châtelier's principle. A stress might be a change in the concentration of reactants or products, a change in the volume of the reaction container, a change in temperature, or the addition of a catalyst. 0 O ▾ Part A Given the concentrations, calculate the equilibrium constant for this reaction: 2SO2(g) +O2(g) = 2SO3(g) At…

How do you solve for the constant equilibrium constant generally?

16

Search the menus (Alt+/) 100% Normal text BI U A Times New.. 15 1 2 | 3 4 5 | 6 7 refer to the following exothermic reaction at equilibrium. 6 P205 + 16 KCl + 9 SO2 3 P4S3 + 16 KC103 + heat Indicate the effect of the changing condition on the position of equilibrium. (shifts left, shifts right, no effect, can shift left or right Remove KCI03 from the mixture. Explain Add P4S3 to the mixture. Explain Cool the mixture. Explain. Decrease the volume of the container.

Classify the conditions given as indicating that a reaction is at equilibrium, is not at equilibrium, or that the conditions may occur in either state. At equilibrium Not at equilibrium May or may not be at equilibrium Answer Bank The products and reactants have equal concentrations. The concentration of products is greater than the concentration of reactants. The concentrations of products and reactants are constant. The forward reaction is occurring at a very slow rate. The concentration of reactants is slowly increasing. The forward and reverse reactions occur at equal rates.

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Select all of the correct statements about equilibrium from the choices below. At equilibrium the rates of forward and reverse reactions are equal.At equilibrium the rate of change of reactant concentration is zero.At equilibrium the rate constants of forward and reverse reactions are equal.At equilibrium concentrations of reactants and products stay constant.As a reaction proceeds forward toward equilibrium the product concentrations rise.At equilibrium the reverse rate equals zero.

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Increasing the concentration of a product in a reversible reaction at equilibrium will shift the reaction to the ___________.     right     left     products     can't be determined from information provided