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Question 43723

posted 11 months ago

2NO2(g) + F2(g) →
NO, and F2 can react to produce NO,F as represented above. A proposed mechanism for this reaction has two elementary steps, as shown below.reaction that is consistent with the proposed mechanism.Write a rate law for the overall
NO, + F, → NO,F + F(slow)
NO2 + FNO,F(fast)

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Question 43707

posted 11 months ago

Complete the table by calculating the pK, and pH of buffer solutions.pK.- log( K, )= -

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Question 43698

posted 11 months ago

Based on this particle diagram, what is the percent ionization of this acid?

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Question 43686

posted 11 months ago

5. Which of these particle diagrams represents a sample of pure water? How can you tell?

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Question 43702

posted 11 months ago

A student is given a 25.0 mL sample of a solution of an unknown monoprotic acid and asked to determine the concentration of the acid by titration.standardized solution of 0.110 M NAOH(aq), a buret, a flask, an appropriate indicator, and other laboratory equipment necessary for the titration.The student uses a
A.) The images below show the buret before the titration begins (below left) and at the end point (below right). What should the student record as the volume of NaOH(aq) delivered to the flask?
B.) Based on the given information and your answer to part (a), determine the value of the concentration of the acid that should be recorded in the student's lab report.
C.) In a second trial, the student accidentally added more NaOH(aq) to the flask than was needed to reach the end point, and then recorded the final volume. Would this error increase, decrease, or have no effect on the calculated acid concentration for the second trial? Justify your answer.

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Question 43701

posted 11 months ago

\left(\mathrm{CH}_{3}\right)_{3} \mathrm{~N}+\mathrm{H}_{2} \mathrm{O} \leftrightarrows\left(\mathrm{CH}_{3}\right)_{3} \mathrm{NH}^{+}+\mathrm{OH}^{-}
Trimethylamine, (CH3);N, is a weak base that reacts with water according to the equationshown above. The K, for (CH3);N is 6.4 × 10-5.
A.) Calculate the pH of 0.10 M (CH3);N.
B.) Calculate the percent ionization of 0.10 M (CH3);N.

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Question 43708

posted 11 months ago

A buffer solution contains 1.2 M HNO2 and 0.80 M NaNO2. What is the pH of this buffer solution? (K, = 4.0 × 10¬4)Henderson-Hasselbach Equation7.Solve using the K, expression AND the MEANING THIS PROBLEM SHOULD HAVE TWO--SETS OF ANSWERS

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Question 43709

posted 11 months ago

A buffer solution that contains a mixture of HC,H;02 and NaC2H3O2 has a pH of 5.00. If[HC,H302] = 2.0 M, what is the value of the [C,H;O2¬]? (K, for HC,H;O2 = 1.8 × 10-5)Solve using the K, expression AND the Henderson-Hasselbach Equation -

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Question 43684

posted 11 months ago

\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftarrows 2 \mathrm{NO}_{2}(g) \quad \Delta \mathrm{H}^{\circ}=+58 \mathrm{~kJ} / \mathrm{mol}_{\mathrm{rxn}}
. The chemical equation shown above represents the reversible reaction in which N,0¿(g) isconverted into NO,(g). The value of the equilibrium constant, K, for this reaction is equal to0.005 at 25°C.
If the temperature of the reaction vessel is increased from 25°C to 100°C, do you predict that the value of K will decrease, increase, or remain the same? Justify your answer.

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Question 43724

posted 11 months ago

What is the expected rate law for the overall reaction shown below?
Step 1:NO(g) + Br,(g) 2 NOBr2(g)(fast)
Step 2:NOBR,(g) + NO2 NO (g) + 2 Br(g)(slow)

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