bleach produces a brlef flash of llght. Whlch change would MOST IIkely make the llght produced In the reaction last longer? O adding a catalyst O increasing the luminol concentration O decreasing the quantity of both reagents

bleach produces a brlef flash of llght. Whlch change would MOST IIkely make the llght produced In the reaction last longer? O adding a catalyst O increasing the luminol concentration O decreasing the quantity of both reagents

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

Section17.2: Factors Affecting Chemical Equilibrium

Problem 13SSC

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Similar questions

Colorless N2O4 gas decomposes to form red-brown colored NO2 gas. Describe how the concentrations of N2O4 and NO2 would change increase or decrease as equilibrium was established in a sealed container that initially contained only N2O4. What observation would indicate that equilibrium had been established?
Explain how to recognize the conditions under which changes in pressure would affect systems at equilibrium.
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
A reaction is represented by this equation: 2W(aq)X(aq)+2Y(aq)Kc=5104 (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations of M, make up [we sets of concentrations that describe a mixture of W, X, and Y at equilibrium.
. The reaction C2H2(g)+2Br2(g)C2H2Br4(g)is exothermic in the forward direction. Will an increase in temperature shift the position of the equilibrium toward reactants or products?
. For the reaction 2H2O(g)2H2(g)+O2(g)K=2.4103at a given temperature. At equilibrium ills found that [H2O(g)]=1.1101Mand [H2(g)]=1.9102M. What is the concentration of O2(g) under these conditions?
For the following system, K=4.86105 at 298K: HClO(aq)+F(aq)ClO(aq)+HF(aq) Assuming that you start with equal concentrations of HClO and F, and that no ClO or HF is initially present, which of the following best describes the equilibrium system: a the forward reaction is favored at equilibrium; b the reverse reaction is favored at equilibrium; c appreciable quantities of all species are present at equilibrium?
When molecules collide, a certain minimum energy called the _________ is needed for the reaction to occur.
In the text, the equation G=G+RTIn(Q) was derived for gaseous reactions where the quantities in Q were expressed in units of pressure. We also can use units of mol/L for the quantities in Q, specifical.ly for aqueous reactions. With this in mind, consider the reaction HF(aq)H+(aq)+F-(aq) for which Ka = 7.2 104 at 25C. Calculate G for the reaction under the following conditions at 25C. a. [HF] = [H+] = [F] = 1.0 M b. [HF] = 0.98 M, [H+] = [F] = 2.7 102M c. [HF] = [H+] = [F] = 1.0 105 M d. [HF] = [F] = 0.27 M, [H+] = 7.2 104M e. [HF] = 0.52 M, [F] = 0.67 M, [H+] = 1.0 103M Based on the calculated G values, in what direction will the reaction shift to reach equilibrium for each of the five sets of conditions?
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer
. Hydrogen gas, oxygen gas, and water vapor are in equilibrium in a closed container. Hydrogen gas is injected into the container, and the system is allowed to return to equilibrium. Which of the following occurs? Explain your answer. 2H2(g)+O2(g)2H2O(g)a. The concentration of oxygen gas remains constant. b. The value for K increases. c. The concentration of oxygen gas increases. d. The concentration of water vapor increases. e. The value for K decreases.