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

$$\text{Percent Yield} = \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\%$$

Q: Which of the following is the correct formula for calculating the enthalpy change ($$\Delta H) of a $$reaction using bond energies?

$$\Delta H = \text{Sum of bond energies of bonds broken} - \text{Sum of bond energies of bonds formed}$$

Question 1

Which of the following best describes a chemical change, as opposed to a physical change?

Accepted Answer

Iron rusting when exposed to air

Question 2

A student mixes 0.50 mol of NaCl with 0.30 mol of AgNO$$_3 in $$water. What is the limiting reactant in the reaction: $$\mathrm{NaCl(aq) + $$AgNO_3$$(aq) \rightarrow AgCl(s) + $$NaNO_3$$(aq)}$$?

Accepted Answer

AgNO$$_3$$

Question 3

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

Accepted Answer

$$	ext{Percent Yield} = \frac{	ext{Actual Yield}}{	ext{Theoretical Yield}} 	imes 100\%$$

Question 4

A solution is prepared by dissolving 0.25 mol of KBr in enough water to make 500 mL of solution. What is the molarity of the solution?

Accepted Answer

$$0.50\ \mathrm{mol/L}$$

Question 5

Which of the following ions will NOT form a precipitate when mixed with Cl$$^- in $$aqueous solution?

Accepted Answer

Na$$^+$$

Question 6

Which of the following best describes an exothermic reaction?

Accepted Answer

A reaction that releases heat to the surroundings

Question 7

Calculate the heat ($$q) $$absorbed by 200 g of water when its temperature increases from 20°C to 40°C. (Specific heat capacity of water $$c = 4.18\ \mathrm{J/g\cdot ^\circ C})$$

Accepted Answer

$$q = 16,720\ \mathrm{J}$$

Question 8

Which of the following is the correct balanced equation for the reaction between aluminum and hydrochloric acid?

Accepted Answer

$$\mathrm{2Al(s) + 6HCl(aq) \rightarrow 2AlCl_3(aq) + 3H_2(g)}$$

Question 9

Which of the following statements about solubility rules is correct?

Accepted Answer

All sodium (Na$$^+) $$salts are soluble in water

Question 10

Which of the following is the correct formula for calculating the enthalpy change ($$\Delta H) of a $$reaction using bond energies?

Accepted Answer

$$\Delta H = 	ext{Sum of bond energies of bonds broken} - 	ext{Sum of bond energies of bonds formed}$$

Question 11

A 1.0 L solution contains 0.10 mol of Na$$_2SO$_4. $$What is the concentration of SO$$_4$$^{2-}$$ ions in the solution?

Accepted Answer

$$0.20\ \mathrm{M}$$

Question 12

Which of the following best describes the role of a spectator ion in a chemical reaction?

Accepted Answer

It is unchanged and does not participate in the reaction

Question 13

Which of the following is a redox reaction?

Accepted Answer

$$\mathrm{Zn(s) + Cu$$^{2+}$$(aq) \rightarrow Zn$$^{2+}$$(aq) + Cu(s)}$$

Question 14

Which of the following is the correct net ionic equation for the reaction between aqueous solutions of Na$$_2SO$_4$$ and BaCl$$_2$$?

Accepted Answer

$$\mathrm{Ba$$^{2+}$$(aq) + SO_4$^{2-}(aq) \rightarrow $$BaSO_4$$(s)}$$

Question 15

Which of the following is the correct formula for the dilution equation?

Accepted Answer

$$M_1V_1 = M_2V_2$$

Question 16

Which of the following is a correct statement about the enthalpy of formation ($$\Delta H_f$$)?

Accepted Answer

It is the enthalpy change when 1 mol of a compound is formed from its elements in their standard states

Question 17

A reaction has $$\Delta H = -150\ \mathrm{kJ}. $$Which statement is true about this reaction?

Accepted Answer

The reaction is exothermic and releases heat

Question 18

Which of the following is the correct formula for calculating the molarity ($$M) of a $$solution?

Accepted Answer

$$M = \frac{	ext{moles of solute}}{	ext{volume of solution in liters}}$$

Question 19

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

Accepted Answer

Calculate the amount of product formed from each reactant and identify the one that produces the least

General Chemistry Study Guide: Chemical Reactions, Solutions, and Thermochemistry (Chapters 7-9)

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