Question 1

When the equation $\mathrm{AlCl_3(aq) + Ba_3(PO_4)_2(aq) \rightarrow AlPO_4(s) + BaCl_2(aq)}$ is properly balanced, what is the coefficient of barium chloride ($\mathrm{BaCl_2}$)?

Accepted Answer

3

Question 2

A certain element has four naturally occurring isotopes with the following data:

Mass (amu): 49.946 (4.35%), 51.941 (83.79%), 52.941 (9.50%), 53.939 (2.36%).

Calculate the average atomic mass of the element.

Accepted Answer

$51.32$

Question 3

Which of the following matched pairs of name and formula has an error?

Accepted Answer

Tetraantimony hexoxide, Sb_4O_6

Question 4

Which of the following does NOT exist as a diatomic molecule at room temperature?

Accepted Answer

Argon

Question 5

Express $39.34\ \mathrm{yd^2}$ in $\mathrm{cm^2}$ given that $1\ \mathrm{m} = 1.0936\ \mathrm{yd}$.

Accepted Answer

$3.24 	imes 10^4$

Question 6

Which of the following pairs is correct?

Accepted Answer

Nitrite ion, NO$_2^-$

Question 7

What is the percentage by mass of Cl in $\mathrm{Mn(ClO_4)_2}$?

Accepted Answer

$16.44\%$

Question 8

Which of the following is NOT an empirical formula?

Accepted Answer

C$_2$H$_4$O$_2$

Question 9

When $22.34\ \mathrm{g}$ iron is consumed in the following unbalanced reaction, how many grams of hydrogen gas will be produced?

$\mathrm{HNO_3(aq) + Fe(s) \rightarrow H_2(g) + Fe(NO_3)_3(aq)}$

Accepted Answer

$1.210\ \mathrm{g}$

Question 10

How many moles of hydrogen atoms are in $2.0158\ \mathrm{g}$ of molecular hydrogen?

Accepted Answer

$1.0\ \mathrm{mol}$

Question 11

A sample of gas is contained in a sealed container with flexible walls. Which will result in the volume of the container being reduced to $\frac{1}{2}$ of the original volume?

Accepted Answer

Increase pressure by 2 and constant T

Question 12

A $4.50\ \mathrm{L}$ sample of neon occupies $4.50\ \mathrm{L}$ at $30.0\ ^\circ\mathrm{C}$ and $2.50\ \mathrm{atm}$. What volume will it occupy at $1000.0\ \mathrm{torr}$ and $300.\ ^\circ\mathrm{C}$?

Accepted Answer

$1620\ \mathrm{mL}$

Question 13

Volume is proportional to temperature at fixed pressure. This is:

Accepted Answer

Charles's Law

Question 14

An $11.2\ \mathrm{L}$ flask contains $0.25\ \mathrm{mol}$ hydrogen and $0.25\ \mathrm{mol}$ radon gas at $273\ ^\circ\mathrm{C}$. What is the pressure in the flask?

Accepted Answer

$1.0\ \mathrm{atm}$

Question 15

If a gas absorbs heat, which of the following is always true?

Accepted Answer

None of the above are necessarily true.

Question 16

A substance has the empirical formula $\mathrm{C_2H_4O}$. If its molar mass is $88\ \mathrm{g/mol}$, its true formula is:

Accepted Answer

$\mathrm{C_4H_8O_2}$

Question 17

What is the molarity of $175\ \mathrm{mL}$ of a solution when $2.18\ \mathrm{g}$ of $\mathrm{Na_2SO_4 \cdot 10H_2O}$ is dissolved in just enough water?

Accepted Answer

$0.00678\ \mathrm{M}$

Question 18

Which of the following is NOT a chemical change?

Accepted Answer

Some pulp shows up in a bottle of previously well-mixed orange juice.

Question 19

How many grams of $\mathrm{AgNO_3}$ are required to make $750\ \mathrm{mL}$ of a $0.100\ \mathrm{M}$ solution?

Accepted Answer

$12.7\ \mathrm{g}$

Question 20

A compound contains $40.0\%$ C, $6.67\%$ H, and the rest is O. If this compound has a molar mass of $120\ \mathrm{g/mol}$, what is the molecular formula of this compound?

Accepted Answer

$\mathrm{C_4H_8O_2}$

General Chemistry I: Practice Exam 1 Study Guide

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