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Sandria S.

Chemistry 102

1 day, 17 hours ago

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EP

Educator P.

Chemistry 102

2 days, 3 hours ago

You have a solution of two volatile liquids, A and B (assume ideal behavior). Pure liquid A has a vapor pressure of 350.0 torr and pure liquid B has a vapor pressure of 100.0 torr at the temperature of the solution. The vapor at equilibrium above the solution has double the mole fraction of substance A that the solution does. What is the mole fraction of liquid A in the solution?

PG

Paul G.

Chemistry 102

2 days, 3 hours ago

Plants that thrive in salt water must have internal solutions (inside the plant cells) that are isotonic with (have the same osmotic pressure as) the surrounding solution. A leaf of a saltwater plant is able to thrive in an aqueous salt solution (at $25^{\circ} \mathrm{C} )$ that has a freezing point equal to $-0.621^{\circ} \mathrm{C} .$ You would like to use this information to calculate the osmotic pressure of the solution in the cell. a. In order to use the freezing-point depression to calculate osmotic pressure, what assumption must you make (in addition to ideal behavior of the solutions, which we will assume)? b. Under what conditions is the assumption (in part a) reasonable? c. Solve for the osmotic pressure (at $25^{\circ} \mathrm{C} )$ of the solution in the plant cell. d. The plant leaf is placed in an aqueous salt solution (at $25^{\circ} \mathrm{C}$ ) that has a boiling point of $102.0^{\circ} \mathrm{C} .$ What will happen to the plant cells in the leaf?

AW

Amanda W.

Chemistry 102

2 days, 3 hours ago

Which of the following can be classified as buffer solutions? $$ \begin{array}{l}{\text { a. } 0.25 M \mathrm{HBr}+0.25 \mathrm{M} \mathrm{HOBr}} \\ {\text { b. } 0.15 \mathrm{M} \mathrm{HClO}_{4}+0.20 \mathrm{M} \mathrm{RbOH}} \\ {\text { c. } 0.50 \mathrm{M} \mathrm{HOCl}+0.35 \mathrm{MKOCl}}\end{array} $$ $$ \begin{array}{l}{\text { d. } 0.70 M \mathrm{KOH}+0.70 \mathrm{M} \text { HONH_ }} \\ {\text { e. } 0.85 \mathrm{M} \mathrm{H}_{2} \mathrm{NNH}_{2}+0.60 M \mathrm{H}_{2} \mathrm{NNH}_{3} \mathrm{NO}_{3}}\end{array} $$

MH

Michelle H.

Chemistry 102

2 days, 3 hours ago

The freezing-point depression of a $0.091-m$ solution of $\mathrm{CsCl}$ is $0.320^{\circ} \mathrm{C} .$ The freezing-point depression of a $0.091-\mathrm{m}$ solution of $\mathrm{CaCl}_{2}$ is $0.440^{\circ} \mathrm{C} .$ In which solution does ion association appear to be greater? Explain.

PF

Patrick F.

Chemistry 102

2 days, 3 hours ago

Neon and HF have approximately the same molecular masses. (a) Explain why the boiling points of Neon and HF differ. (b) Compare the change in the boiling points of Ne, Ar, Kr, and Xe with the change of the boiling points of HF, HCl, HBr, and HI, and explain the difference between the changes with increasing atomic or molecular mass.

ST

Steve T.

Chemistry 102

2 days, 3 hours ago

How many liters of HCl gas, measured at $30.0^{\circ} \mathrm{C}$ and 745 tor, are required to prepare 1.25 $\mathrm{L}$ of a $3.20-\mathrm{M}$ . solution of hydrochloric acid?

RB

Ray B.

Chemistry 102

2 days, 3 hours ago

Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid, (b) chromium with hydrobromic acid, (c) tin with hydrochloric acid, (d) aluminum with formic acid, HCOOH.

MP

Melanie P.

Chemistry 102

2 days, 3 hours ago

Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each: (a) solid cadmium sulfide reacts with an aqueous solution of sulfuric acid; (b) solid magnesium carbonate reacts with an aqueous solution of perchloric acid.

MO

Michelle O.

Chemistry 102

2 days, 3 hours ago

Classify each of the following substances as a nonelectrolyte, weak electrolyte, or strong electrolyte in water: (a) $\mathrm{H}_{2} \mathrm{SO}_{3}$ , (b) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}$ (ethanol), $(\mathbf{c}) \mathrm{NH}_{3},(\mathbf{d}) \mathrm{KClO}_{3}$, $(\mathbf{e}) \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}$.

MH

Michelle H.

Chemistry 102

2 days, 3 hours ago

Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (a) HF, (b) acetonitrile,$\mathrm{CH}_{3} \mathrm{CN},(\mathbf{c}) \mathrm{NaClO}_{4},(\mathbf{d}) \mathrm{Ba}(\mathrm{OH})_{2} .$

BP

Brian P.

Chemistry 102

2 days, 3 hours ago

We have learned in this chapter that many ionic solids dissolve in water as strong electrolytes; that is, as separated ions in solution. Which statement is most correct about this process? (a) Water is a strong acid and therefore is good at dissolving ionic solids. (b) Water is good at solvating ions because the hydrogen and oxygen atoms in water molecules bear partial charges. (c) The hydrogen and oxygen bonds of water are easily broken by ionic solids.

AA

Andrea A.

Chemistry 102

2 days, 3 hours ago

Which data set, of the two graphed here, would you expect to observe from a titration like that shown in Figure 4.18$?$ [Section 4.6$]$

PA

Patrick A.

Chemistry 102

2 days, 3 hours ago

Find the pH of each mixture of acids. a. 0.115 M in HBr and 0.125 M in HCHO2 b. 0.150 M in HNO2 and 0.085 M in HNO3 c. 0.185 M in HCHO2 and 0.225 M in HC2H3O2 d. 0.050 M in acetic acid and 0.050 M in hydrocyanic acid

CC

Carolyn C.

Chemistry 102

2 days, 3 hours ago

Calculate the amount of heat required to completely sublime 50.0g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol.

GG

Gary G.

Chemistry 102

2 days, 3 hours ago

A 100.0 mL sample of water is heated to its boiling point. How much heat (in kJ) is required to vaporize it? (Assume a density of 1.00 g>mL.)

TH

Timothy H.

Chemistry 102

2 days, 3 hours ago

A solution is made 1.1 * 10-3 M in Zn(NO3)2 and 0.150 M in NH3. After the solution reaches equilibrium, what concentration of Zn2+(aq) remains?

NC

Nabriya C.

Chemistry 102

2 days, 4 hours ago

Because the reaction free energy change (DG ) and cell potential (Ecell ) are related, instead of using DG to determine the reaction spontaneity, we can also use Ecell to determine the cell reaction spontaneity. Which of the following can predict a non-spontaneous cell reaction?

NC

Nabriya C.

Chemistry 102

2 days, 4 hours ago

Because the reaction free energy change (DG ) and cell potential (Ecell ) are related, instead of using DG to determine the reaction spontaneity, we can also use Ecell to determine the cell reaction spontaneity. Which of the following can predict a cell reaction at equilibrium?

NC

Nabriya C.

Chemistry 102

2 days, 4 hours ago

Which one is the Nernst equation, that shows the concentration effect on cell potential ?

NC

Nabriya C.

Chemistry 102

2 days, 4 hours ago

Which of the following is not an application of electrochemistry?

SB

Stephanie B.

Chemistry 102

2 days, 16 hours ago

O2(g)+2H2O(l)+2Cu(s)?4OH?(aq)+2Cu2+(aq)

BG

Brady G.

Chemistry 102

3 days, 3 hours ago

Explain why it is not possible to prepare a ketone that contains only two carbon atoms.

Cc

Canary C.

Chemistry 102

3 days, 3 hours ago

Write two complete, balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures. (a) 2-butene reacts with chlorine. (b) benzene burns in air

JC

Jason C.

Chemistry 102

3 days, 3 hours ago

On a microscopic level, how does the reaction of bromine with a saturated hydrocarbon differ from its reaction with an unsaturated hydrocarbon? How are they similar?

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