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Question
What is the net ionic equation for the reaction of aqueous hydrochloric acid and aqueous potassium hydroxide?
A.HCl(aq) + OH-(aq) H2O(
) + Cl-(aq)
B.Cl-(aq) + K+(aq) KCl(s)
C.HCl(aq) + KOH(aq) KCl(aq) + H2O()
D.Cl-(aq) + K+(aq) KCl(aq)
E.H+(aq) + OH-(aq) H2O()
Answer
This answer is hidden. It contains 2 characters.
Related questions
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Q:
An aqueous solution with a pH of 10.60 is diluted from 1.0 L to 2.0 L. What is the pH of the diluted solution?
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An aqueous solution with a pH of 2.00 is diluted from 1.0 L to 3.0 L. What is the pH of the diluted solution?
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Q:
Assume that the following endothermic chemical reaction is at equilibrium.
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2/ Decreasing the temperature will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g).
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Given the following chemical equilibria,
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A.
B.
C.
D.
E.
Q:
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Q:
If the reaction quotient, Q, is equal to K in a gas phase reaction, then
A.the chemical system has reached equilibrium.
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Q:
Write a balanced chemical equation which corresponds to the following equilibrium constant expression.A.HNO2(aq) + H2O() NO2-(aq) + H3O+(aq)B.NO2-(aq) + H3O+(aq) HNO2(aq) + H2O()C.NO2-(aq) + H3O+(aq) HNO2(aq)D.H+(aq) + OH-(aq) H2O()E.HNO2(aq) NO2-(aq) + H3O+(aq)
Q:
For the reaction 2A + B C, the rate law is
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For the reaction A B, the rate law is
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What are the units of the rate constant where time is measured in seconds?
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B.
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D.
E.
Q:
What is the overall order of the reaction below
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Q:
Which statement concerning relative rates of reaction is correct for the chemical equation given below?
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B.The rate of disappearance of CH3OH is two times the rate of appearance of H2O.
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Q:
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Q:
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Q:
The rate constant at 366 K for a first-order reaction is 7.7 10-3 s-1 and the activation energy is 15.9 kJ/mol. What is the value of the frequency factor, A, in the Arrhenius equation? (R = 8.314 J/Kmol)A.0.0047 s-1B.0.70 s-1C.0.93 s-1D.1.1 s-1E.1.4 s-1
Q:
Calculate the activation energy, Ea, forN2O5(g) 2 NO2(g) + 1/2 O2(g)given k (at 45.0 C) = 5.79 10-4 s-1 and k (at 60.0 C) = 3.83 10-3 s-1. (R = 8.314 J/Kmol)A.0.256 kJ/molB.2.83 kJ/molC.31.1 kJ/molD.111 kJ/molE.389 kJ/mol
Q:
What is the half-life of a first-order reaction if it takes 4.4 10-2 seconds for the concentration to decrease from 0.50 M to 0.20 M?A.2.5 10-2 sB.3.3 10-2 sC.1.6 sD.21 sE.27 s
Q:
Hydrogen peroxide decomposes into water and oxygen in a first-order process.
H2O2(aq) H2O() + 1/2 O2(g)
At 20.0 C, the half-life for the reaction is 3.92 104 seconds. If the initial concentration of hydrogen peroxide is 0.52 M, what is the concentration after 7.00 days?
A.1.2 10-5 M
B.0.034 M
C.0.074 M
D.0.22 M
E.0.52 M
Q:
A student analyzed a first-order reaction and obtained the graph below. Unfortunately, the student forgot to label the axes. What are the correct labels for the x and y axes? A.x axis = time, y axis = ln[A]
B.x axis = ln[time], y axis = [A]
C.x axis = ln[time], y axis = [A]
D.x axis = time, y axis = 1/[A]
E.x axis = 1/time, y axis = 1/[A]