Q: If you have $$5.0\ \mathrm{Q}/\mathrm{B}^3$$, how many $$\mathrm{M}/\mathrm{Z}^3 do $$you have? (Given: $$1\ \mathrm{Q} = 3.0\ \mathrm{R}$$, $$2.0\ \mathrm{B} = 1\ \mathrm{Z}$$, $$6.0\ \mathrm{R} = 1\ \mathrm{M})$$

$$2.0 \times 10^1$\ \mathrm{M}/\mathrm{Z}^3$$

Question 1

Which of the following temperatures is the hottest?

Accepted Answer

$$-80\ ^\circ\mathrm{F}$$

Question 2

Perform the following calculation and report your answer to the correct number of significant figures: $$\left( \dfrac{7.20 	imes 10$$^{-2}$$}{0.049} ight) - 0.383$$

Accepted Answer

$$1.1$$

Question 3

Convert $$1.187 	imes 10$$^{-2}$$\ \mathrm{m}^3 to$$ $$\mathrm{in}^3$$. ($$1\ \mathrm{in} = 2.54\ \mathrm{cm})$$

Accepted Answer

$$724.4\ \mathrm{in}^3$$

Question 4

A metal has a density of $$2.70\ \mathrm{g/mL}. An $$electrical wire with a diameter of $$0.5\ \mathrm{mm} is $$made of that metal and has a volume of $$3.00 	imes 10$$^{-3}$$\ \mathrm{mL}. $$What is the mass of the wire in mg?

Accepted Answer

$$8.10\ \mathrm{mg}$$

Question 5

An atom has an atomic number of $$16$$, an atomic mass of $$34$$, and contains $$18$$ electrons. What is the charge of the atom and what is its element symbol?

Accepted Answer

Charge: $$-2$$, Symbol: $$\mathrm{S}$$

Question 6

Which pair of atoms are isotopes of each other?

Accepted Answer

I and II

Question 7

What is the formula mass of dinitrogen pentoxide ($$\mathrm{N}_2\mathrm{O}_5$$)?

Accepted Answer

$$108.0\ \mathrm{amu}$$

Question 8

If you have $$5.0\ \mathrm{Q}/\mathrm{B}^3$$, how many $$\mathrm{M}/\mathrm{Z}^3 do $$you have? (Given: $$1\ \mathrm{Q} = 3.0\ \mathrm{R}$$, $$2.0\ \mathrm{B} = 1\ \mathrm{Z}$$, $$6.0\ \mathrm{R} = 1\ \mathrm{M})$$

Accepted Answer

$$2.0 	imes 10^1$\ \mathrm{M}/\mathrm{Z}^3$$

Question 9

Infants are to be given a medication at a dosage no higher than $$15.0\ \mathrm{mg/kg} of $$body mass every $$6$$ hours. What is the maximum total dosage a child weighing $$18.0\ \mathrm{lb}$$ should receive in a $$12-$$hour period? ($$1\ \mathrm{kg} = 2.205\ \mathrm{lb})$$

Accepted Answer

$$245\ \mathrm{mg}$$

Question 10

What is the formula of ammonium phosphate, and how many hydrogen atoms are in it?

Accepted Answer

$$(\mathrm{NH}_4)_3\mathrm{PO}_4$$, $$12$$ hydrogen atoms

Question 11

Which pair of name and formula does NOT match?

Accepted Answer

chromium(III) sulfide: $$\mathrm{CrS}$$

Question 12

Which of the following is the correct equation for the ionization of aluminum?

Accepted Answer

$$\mathrm{Al} \rightarrow \mathrm{Al}^{3+} + e$$^{3-}$$

Question 13

Chlorine has two naturally occurring isotopes: $$\mathrm{Cl}-35$$ ($$34.97\ \mathrm{amu}) $$and $$\mathrm{Cl}-37$$ ($$36.97\ \mathrm{amu}). $$The atomic mass of chlorine is $$35.45\ \mathrm{amu}. $$What is the relative abundance of each isotope in a naturally occurring sample?

Accepted Answer

$$76.0\%$$ $$\mathrm{Cl}-35$$; $$24.0\%$$ $$\mathrm{Cl}-37$$

Question 14

How many protons, neutrons, and electrons are in the ion $$^{56}\mathrm{Fe}^{3+}$$?

Accepted Answer

$$26$$ protons, $$30$$ neutrons, $$23$$ electrons

Question 15

A sample of metal is either zinc or titanium. Fully submerged, it displaces $$0.450\ \mathrm{gal} of $$water and weighs $$16.85\ \mathrm{lb}. $$Which is it? (Density of zinc $$= 7.13\ \mathrm{g/cm}^3$$; density of titanium $$= 4.51\ \mathrm{g/cm}^3$$; $$1\ \mathrm{gal} = 3.785\ \mathrm{L}$$; $$1\ \mathrm{lb} = 453.6\ \mathrm{g})$$

Accepted Answer

titanium

Question 16

Which of the following statements about isotopes is correct?

Accepted Answer

Isotopes of an element have the same number of protons but different numbers of neutrons.

Question 17

A patient is prescribed a solution containing $$0.50\ \mathrm{g} of $$sodium chloride ($$\mathrm{NaCl}) $$per $$100\ \mathrm{mL} of $$solution. How many moles of $$\mathrm{NaCl}$$ are present in $$250\ \mathrm{mL} of $$this solution? ($$\mathrm{Molar\ mass\ of\ NaCl} = 58.44\ \mathrm{g/mol})$$

Accepted Answer

$$0.0214\ \mathrm{mol}$$

Question 18

Which of the following best describes the process of determining the empirical formula from percent composition data?

Accepted Answer

Convert percent to grams, convert grams to moles, divide by the smallest number of moles, and round to the nearest whole number.

Introduction to Chemistry Practice Midterm 1 – Step-by-Step Guidance

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