Q: Which of the following is the correct formula for calculating percent yield?

$$\displaystyle \%\ \mathrm{yield} = \frac{\text{actual yield}}{\text{theoretical yield}} \times 100$$

Question 1

Which of the following best describes the role of the limiting reactant in a chemical reaction?

Accepted Answer

It is the reactant that determines the amount of product formed.

Question 2

A student is asked to prepare 500.0 mL of 1.00 M $$(\mathrm{NH}_4)_3\mathrm{PO}_4$$ solution. What mass of $$(\mathrm{NH}_4)_3\mathrm{PO}_4 is $$required? (Molar mass = 149.09 g/mol)

Accepted Answer

$$74.5\ \mathrm{g}$$

Question 3

Which of the following is the correct balanced equation for the reaction between silver nitrate and potassium iodide in aqueous solution?

Accepted Answer

$$\mathrm{AgNO}_3 (aq) + \mathrm{KI} (aq) \rightarrow \mathrm{AgI} (s) + \mathrm{KNO}_3 (aq)$$

Question 4

A 1.154 g sample of sulfur reacts with fluorine to form a compound with the formula $$SF_x. If 5.722 g of$$ $$F_2 is $$used, what is the value of $$x$$?

Accepted Answer

$$6$$

Question 5

Which of the following statements about strong and weak electrolytes is correct?

Accepted Answer

Strong electrolytes dissociate completely in water, while weak electrolytes dissociate only partially.

Question 6

Given the reaction: $$2\mathrm{NaOH} (aq) + \mathrm{Pb(NO}_3)_2 (aq) \rightarrow 2\mathrm{NaNO}_3 (aq) + \mathrm{Pb(OH)}_2 (s)$$, if 0.200 mol $$\mathrm{NaOH} is $$mixed with 0.100 mol $$\mathrm{Pb(NO}_3)_2$$, how many moles of $$\mathrm{Pb(OH)}_2$$ will precipitate?

Accepted Answer

$$0.100\ \mathrm{mol}$$

Question 7

Which of the following is the correct net ionic equation for the reaction between $$\mathrm{Na}_2\mathrm{SO}_4$$ and $$\mathrm{BaCl}_2 in $$aqueous solution?

Accepted Answer

$$\mathrm{Ba}^{2+} (aq) + \mathrm{SO}_4$$^{2-}$$ (aq) \rightarrow \mathrm{BaSO}_4 (s)$$

Question 8

A solution is prepared by dissolving 10.0 g of $$\mathrm{NaCl} in $$enough water to make 500.0 mL of solution. What is the molarity of the solution? (Molar mass of $$\mathrm{NaCl} = 58.44 g/$$mol)

Accepted Answer

$$0.342\ \mathrm{M}$$

Question 9

Which of the following is the correct sequence of steps for balancing a redox reaction in acidic solution?

Accepted Answer

Assign oxidation states, separate into half-reactions, balance all elements except H and O, balance O with $$\mathrm{H}_2\mathrm{O}$$, balance H with $$\mathrm{H}^+$$, balance charge with electrons, combine and simplify.

Question 10

A combustion analysis of a hydrocarbon yields 2.20 g of $$\mathrm{CO}_2$$ and 0.90 g of $$\mathrm{H}_2\mathrm{O}. $$What is the empirical formula of the hydrocarbon?

Accepted Answer

$$\mathrm{CH}_2$$

Question 11

Which of the following solutions has the highest total ion concentration?

Accepted Answer

$$0.10\ \mathrm{M}\ \mathrm{BaCl}_2$$

Question 12

Which of the following acids is a strong acid?

Accepted Answer

$$\mathrm{HNO}_3$$

Question 13

What is the percent yield if 27.0 g of $$\mathrm{PCl}_3 is $$produced from a reaction with a theoretical yield of 30.0 g?

Accepted Answer

$$90\%$$

Question 14

Which of the following best describes a spectator ion?

Accepted Answer

An ion that does not participate in the chemical reaction and remains unchanged in solution.

Question 15

If 100.0 mL of 12 M HCl is diluted to a final volume of 1.00 L, what is the final concentration?

Accepted Answer

$$1.2\ \mathrm{M}$$

Question 16

Which of the following is the correct formula for calculating percent yield?

Accepted Answer

$$\displaystyle \%\ \mathrm{yield} = \frac{	ext{actual yield}}{	ext{theoretical yield}} 	imes 100$$

Question 17

Which of the following is a correct net ionic equation for the reaction of hydrochloric acid with sodium hydroxide?

Accepted Answer

$$\mathrm{H}^+ (aq) + \mathrm{OH}^- (aq) \rightarrow \mathrm{H}_2\mathrm{O} (l)$$

Question 18

A solution contains $$0.10\ \mathrm{M}\ \mathrm{K}_3\mathrm{PO}_4. $$What is the total ion concentration in the solution?

Accepted Answer

$$0.40\ \mathrm{M}$$

Question 19

Which of the following is the correct order of steps for preparing a standard solution in a volumetric flask?

Accepted Answer

Dissolve solute in less than the final volume, swirl to mix, add water to the calibration line, stopper and invert to mix.

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