A redox reaction has an equilibrium constant of K = 0.055. What is true of $\Delta G_{\mathrm{rxn}}^{\mathrm{o}}$ and $E_{\mathrm{cell}}^{\circ}$ for this reaction?

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. a. $4 \mathrm{Li}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Li}_{2} \mathrm{O}(s)$ b. $\mathrm{Mg}(s)+\mathrm{Fe}^{2+}(a q) \longrightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Fe}(s)$ c. $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{PbSO}_{4}(s)+2 \mathrm{NaNO}_{3}(a q)$ d. $\mathrm{HBr}(a q)+\mathrm{KOH}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{KBr}(a q)$

Two biology instructors set out to evaluate the effects of discovery-based teaching compared to the standard lecture-based teaching approach in the laboratory. The standard lecture-based approach provided a list of instructions to follow at each step of the laboratory exercise, whereas the discovery-based approach asked questions rather than providing directions, and used small group reports to decide the best way to proceed in reaching the laboratory objective. One evaluation of the techniques involved written appraisals of both techniques by students at the end of the course. The comparison of the number of positive and negative responses for both techniques is given in the following table.

Group, Positive Evaluations, Negative Evaluations, Total Discovery, 37, 11, 48 Control, 31, 17, 48

a. Is there a significant difference in the proportion of positive responses for each of the teaching methods? Use $\alpha$=.05. If so, how would you describe this difference? b. What is the approximate p-value for the test in part a?

Which metal cation is the best oxidizing agent? a. $Pb^{2+}$ b. $Cr ^{3+}$ c. $Fe^{2+}$ d. $Sn^{2+}$

The anode of an electrolytic cell must be connected to which terminal - positive or negative-of the power source?

For the phrase in the first column, write the letter of the synonymous phrase in the second column.

$$\begin{matrix} \text{direct balefully} & \text{a. spoil the toil}\\ & \text{b. naturally matchable}\\ & \text{c. an iniquity from antiquity }\\ & \text{d. born to adorn}\\ & \text{e. usin' a euphemism}\\ & \text{f. sickening chicken}\\ & \text{g. intense defense}\\ & \text{h. administer sinisterly}\\ & \text{i. a diabolical frolic}\\ & \text{j. an inexorable force}\\ \end{matrix}$$

What is the oxidation state of Cl in each ion? a. $ClO^-$ b. $ClO_2^-$ c. $ClO_3 ^-$

Briefly explain its connection to East Asia between 600 and 1350. 6.Shinto

The molar mass of a metal (M) is 50.9 g/mol; it forms a chloride of unknown composition. Electrolysis of a sample of the molten chloride with a current of 6.42 A for 23.6 minutes produces 1.20 g of M at the cathode. Determine the empirical formula of the chloride.

Balance each redox reaction occurring in acidic aqueous solution. a. $\mathrm{I}^{-}(a q)+\mathrm{NO}_{2}^{-}(a q) \longrightarrow \mathrm{I}_{2}(s)+\mathrm{NO}(g)$ b. $\mathrm{ClO}_{4}^{-}(a q)+\mathrm{Cl}(a q) \longrightarrow \mathrm{ClO}_{3}^{-}(a q)+\mathrm{Cl}_{2}(g)$ c. $\mathrm{NO}_{3}^{-}(a q)+\mathrm{Sn}^{2+}(a q) \longrightarrow \mathrm{Sn}^{4+}(a q)+\mathrm{NO}(g)$

Express your answer as a chemical equation. Enter NOREACTION if no reaction occurs. Identify all of the phases in your answer.

Part A. sodium nitrate and lead (II) acetate

Part B. aluminum iodide and lead(II) acetate

Part C. barium nitrate and sodium sulfide

Part D. strontium nitrate and sodium sulfide

After all foreign and U.S. taxes, a U.S. corporation expects to receive 2 pounds of dividends per share from a British subsidiary this year. The exchange rate at the end of the year is expected to be $1.53 per pound, and the pound is expected to depreciate 5% against the dollar each year for an indefinite period. The dividend (in pounds) is expected to grow at 10% a year indefinitely. The parent U.S. corporation owns 10 million shares of the subsidiary. What is the present value in dollars of its equity ownership of the subsidiary? Assume a cost of equity capital of 11% for the subsidiary.

The Henry's law constant for helium gas in water at

$$30 ^ { \circ } \mathrm { C }$$

is

$$3.7 \times 10 ^ { - 4 } M / a t m$$

and the constant for

$$N_2$$

at

$$30 ^ { \circ } \mathrm { C }$$

is

$$6.0 \times 10 ^ { - 4 } M / atm$$

If the two gases are each present at 1.5 atm pressure, calculate the solubility of each gas.

Which metal could you use to reduce $Mn^{2+}$ ions but not $Mg^{2+}$ ions?