None Scoring: Your score will be based on the number of correct matches minus the number of incorrect matches. There is no penalty for missing matches.Use the References to access important values if needed for this question.For the following reaction, the reactants are favored at equilibrium. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids orbases.F+CH₂NH3 HF + C6H5NH2HFClear AllStronger Bronsted-Lowry acidWeaker Bronsted-LowryC6H5NH3+acidF-Stronger Bronsted-Lowry baseWeaker Bronsted-LowryC6H5NH2base

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Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

Section: Chapter Questions

Problem 17STP

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Describe any thermochemical (heat of reaction) evidence for the Arrhenius concept.
For the generalized chemical reaction A(g)+B(g)C(g)+D(g) determine whether the concentration of A in an equilibrium mixture will (1) increase, (2) decrease, or (3) not change when each of the following changes is effected. a. concentration of B is increased b. concentration of C is decreased c. concentration of D is increased d. concentration of D is decreased
For the generalized chemical reaction A(g)+B(g)C(g)+D(g) determine whether the concentration of D in an equilibrium mixture will (1) increase, (2) decrease, or (3) not change when each of the following changes is effected. a. concentration of A is increased b. concentration of B is decreased c. concentration of C is increased d. concentration of C is decreased
For the equilibrium reaction in Question 4, write the expression for the equilibrium constant. (a) How would this equilibrium constant change if the total pressure on the system were doubled? (b) How would the equilibrium constant change if the temperature were increased?
When writing an equation, how is a reversible reaction distinguished from a nonreversible reaction?
Which direction of the equilibrium 2NO2(g)N2O4(g)+59.0kJ will be favored if the system is cooled? Explain.
For each of the changes listed will the rate of the following chemical reaction increase, decrease, or remain the same? Fe(s)+2HCl(aq)FeCl2(aq)+H2(g) a. the concentration of HCl is decreased b. the iron is ground into a powder c. a catalyst is added to the reaction mixture d. the temperature of the solution is decreased
12.19 For each of the following equations, write the equilibrium expression for the reverse reaction. 2C(s) + O,(g)^2CO(g) AgCl(s)5=BAg+(aq) + Cr
When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200. °C in a closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established. Write a balanced chemical equation for the equilibrium reaction. Use bond enthalpies from Table 6.2 ( Sec. 6-6b) to estimate the enthalpy change for the reaction. Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium, the entropy effect or the energy effect? In which direction will the equilibrium shift as the temperature increases above 200. °C? Explain. Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift? Why is the equilibrium not established at room temperature?
Please answer question 11 Part A and B
Which statement correctly describes a chemical reaction at equilibrium? 1. The concentrations of the products and reactants are equal. 2. The rate of the forward reaction is less than the rate of the reverse reaction. 3. The rate of the forward reaction is greater than the rate of the reverse reaction. 4. The concentrations of the products and reactants are constant.
Define chemical equilibrium. Group of answer choices The reaction rate in the forward direction equals the reaction rate in the reverse direction resulting in a continuous reaction with no net change. The chemical reaction stops when the reaction rate in the forward direction equals the reaction rate in the reverse direction. The chemical reactions stops when the concentration of reactants and the forward reactions rate equals the concentration of the products and the reverse reaction rate. The chemical reaction stops when the concentration of the reactants equals the concentration of the products. The concentration of the reactants equals the concentration of the products resulting in a continuous reaction with no net change.

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