Honors Chemistry 1 Semester Exam (Part 2)

What is the molarity of a solution containing 20 grams of NaOH in 500 mL of solution? : A. 1 M B. 2M C. .04 M D. 0.5 M

A. 1 M

What is the molarity of a solution that contains 0.25 mole of solute in 250 mL of solution? : A. 1.0 M B. 0.025 M C. 0.50 M D. 0.75

A. 1.0 M

A 2.00-gram sample of helium at STP will occupy : A. 11.2l B. 22.4l C. 33.6l D. 44.8l

A. 11.2l

The volume of 16.0 grams of SO2(g) at STP is closest to : A. 5.60l B. 11.2l C. 22.4l D. 44.8l

A. 5.60l

Which formula represents a mixture? : A. HCl(aq) B. HCl(g) C. HCl(s) D. HCl(l)

A. HCl(aq)

What is the correct formula of potassium hydride? : A. KH B. KH2 C. KOH D. K(OH)2

A. KH

Which of the following represents a mixture? : A. NaCl(aq) B. NaCl(s) C. NH3(g) D. NH3(l)

A. NaCl(aq)

Which of these elements has an atom with the most stable outer electron configuration? : A. Ne B. Cl C. Ca D. Na

A. Ne

Which atom in the ground state has three half-filled orbitals? : A. P B. Si C. Al D. Li

A. P

Which of the following electron configurations represents the LEAST active metal? : A. [Ne]3s^2 B. [Ar]4s^2 C. [Kr]5s^2 D. [Xe]6s^2

A. [Ne]3s^2

Which is an example of a compound? : A. ammonia B. calcium C. diamond D. uranium

A. ammonia

When sugar is dissolved in water, the resulting solution is classified as a : A. homogeneous mixture B. heterogeneous mixture C. homogeneous compound D. heterogeneous compound

A. homogeneous mixture

An example of a heterogeneous mixture is : A. soil B. sugar C. carbon monoxide D. carbon dioxide

A. soil

How many moles of H2SO4 are needed to prepare 5.0 L of a 2.0 M solution of H2SO4? : A. 2.5 B. 5.0 C. 10 D. 20

C. 10

Which quantity of N2 gas has a volume of 11.2 liters at STP? : A. 1.0 mole B. 2.0 moles C. 14.0 grams D. 28.0 grams

C. 14.0 grams

A 3.0 M HCl(aq) solution contains a total of : A. 3.0 grams of HCl per liter of water B. 3.0 grams of HCl per mole of solution C. 3.0 moles of HCl per liter of solution D. 3.0 moles of HCl per mole of water

C. 3.0 moles of HCl per liter of solution

Given the balanced equation : Mg(s) + 2HCl(aq) -> MgCl2(aq) + H2(g) At STP, what is the total number of liters of hydrogen gas produced when 3.00 moles of hydrochloric acid solution is completely consumed? : A. 11.2L B. 22.4L C. 33.6L D. 44.8L

C. 33.6L

What is the volume of 1.50 moles of an ideal gas at STP? : A. 11.2L B. 22.4L C. 33.6L D. 44.8L

C. 33.6L

What is the total number of valence electrons in an atom of xenon? : A. 0 B. 2 C. 8 D. 18

C. 8

Which is the formula of a binary compound? : A. KOH B. NaClO3 C. Al2S3 D. Bi(NO3)3

C. Al2S3

Which ion has the electron configuration of a noble gas?: A. Cu2+ B. Fe2+ C. Ca2+ D. Hg2+

C. Ca2+

An atom that has an electron configuration of 1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 4s^2 is classified as : A. an alkali metal B. an alkaline earth metal C. a transition metal D. a noble gas element

C. a transition metal

Which unit can be used to express solution concentration? : A. J/mol B. L/mol C. mol/L D. mol/s

C. mol/L

The volume of a 1.00-mole sample of an ideal gas will decrease when the : A. pressure decreases and the temperature decreases B. pressure decreases and the temperature increases C. pressure increases and the temperature decreases D. pressure increases and the temperature increases

C. pressure increases and the temperature decreases

What is the name of the compound whose formula is H2SO4? : A. hydrosulfuric acid B. hydrosulfurous acid C. sulfuric acid D. sulfurous acid

C. sulfuric acid

The molarity (M) of a solution is equal to the : A. # of grams of solute/liter of solvent B. # of grams of solute/liter of solution C. # of moles of solute/liter of solvent D. # of moles of solute/liter of solution

D. # of moles of solute/liter of solution

What is the gram formula mass of Mg(ClO3)2? : A. 107 g B. 142 g C. 174 g D. 191 g

D. 191 g

Given the reaction at STP : N2(g) + 3H2(g) -> 2NH3(g) What is the total number of liters of NH3 formed when 20 liters of N2 reacts completely? : A. 10L B. 20L C. 30L D. 40L

D. 40L

What is the total number of carbon atoms contained in 22.4 liters of CO gas at STP? : A. 1.00 B. 0.500 C. 3.01 x 10^23 D. 6.02 x 10^23

D. 6.02 x 10^23

The correct formula for calcium phosphate is : A. CaPO4 B. Ca2(PO4)3 C. Ca3P2 D. Ca3(PO4)2

D. Ca3(PO4)2

Which substance is classified as a salt? : A. Ca(OH)2 B. C2H4(OH)2 C. CCl4 D. CaCl2

D. CaCl2

Which is the formula for sodium perchlorate? : A. NaClO B. NaClO2 C. NaClO3 D. NaClO4

D. NaClO4

Which species does not have a noble gas electron configuration? : A. Na B. Mg C. Ar D. S

D. S

Which particle has the same electron configuration as a potassium ion? : A. fluoride ion B. sodium ion C. neon atom D. argon atom

D. argon atom

What halogen is a solid at STP? : A. fluorine B. chlorine C. bromine D. iodine

D. iodine

Show a correct numerical setup for determining how many liters of a 1.2 M solution can be prepared with 0.50 mole of C6H12O6.

1.2 = 0.50/x

What is the volume, in liters, of 576 grams of SO2 gas at STP? : A. 101 B. 202 C. 216 D. 788

B. 202

If .50 L of a 12-molar solution is diluted to 1.0 liter, the molarity of the new solution is : A. 2.4 B. 6.0 C. 12 D. 24

B. 6.0

Which material is a mixture? : A. water B. air C. methane D. magnesium

B. air

What is the correct name of the compound with the formula NH4NO2? : A. ammonia nitrite B. ammonium nitrite C. ammonia nitrate D. ammonium nitrate

B. ammonium nitrite

At constant temperature, which line best shows the relationship between the volume of an ideal gas and its pressure? : A. curved up B. curved down C. line with positive slope D. straight line

B. curved down

Which temperature change would cause a sample of an ideal gas to double in volume while the pressure is held constant? : A. from 400.K to 200 B. from 200.K to 400.K C. from 400. (degrees C) to 200. (degrees C) D. from 200. (degrees C) to 400. (degrees C)

B. from 200.K to 400.K

The pH of a 0.1 M CH3COOH solution is : A. less than 1 B. greater than 1 but less than 7 C. equal to 7 D. greater than 7

B. greater than 1 but less than 7

Molarity is defined as the : A. moles of solute per kilogram of solvent B. moles of solute per liter of solution C. mass of a solution D. volume of a solvent

B. moles of solute per liter of solution

Which gas is monatomic at STP? : A. nitrogen B. neon C. fluorine D. chlorine

B. neon