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Practice Exam for General Chemistry I - Fall 2008 | CHM 2045, Papers of Chemistry

Material Type: Paper; Professor: Alegria; Class: General Chemistry I; Subject: Chemistry; University: University of South Florida; Term: Fall 2008;

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Uploaded on 10/02/2008

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CHM 2045
1)
Which of the following statements about mass spectrometry is false?
A)
Mass spectrometry can be used to determine the molecular weight of a compound.
B)
The curvature of the path in a magnetic field is determined by the mass of the ion.
C)
The paths of heavier ions are deflected more strongly than the paths of lighter ions.
D)
The sample is changed into positively charged ion
2)
If the density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are
needed to produce 15.0 g of CO2 according to the following chemical equation?
C2H5OH(l) + 3 O2(g) 2 CO2(g) + 3 H2O(l)
A)
6.19 mL
B)
9.95 mL
C)
19.9 mL
D)
39.8 mL
3)
If the percent yield for the following reaction is 75.0%, and 45.0 g of NO2 are consumed in
the reaction, how many grams of nitric acid, HNO3(aq) are produced?
3 NO2(g) + H2O(l) 2 HNO3(aq) + NO(g)
A)
30.8 g
B)
41.1 g
C)
1
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CHM 2045

Which of the following statements about mass spectrometry is false?

A)

Mass spectrometry can be used to determine the molecular weight of a compound.

B)

The curvature of the path in a magnetic field is determined by the mass of the ion.

C)

The paths of heavier ions are deflected more strongly than the paths of lighter ions.

D)

The sample is changed into positively charged ion

If the density of ethanol, C 2

H

OH, is 0.789 g/mL. How many milliliters of ethanol are

needed to produce 15.0 g of CO 2

according to the following chemical equation?

C

H

OH( l ) + 3 O 2

( g ) 2 CO 2

( g ) + 3 H 2

O( l )

A)

6.19 mL

B)

9.95 mL

C)

19.9 mL

D)

39.8 mL

If the percent yield for the following reaction is 75.0%, and 45.0 g of NO 2

are consumed in

the reaction, how many grams of nitric acid, HNO 3

( aq ) are produced?

3 NO

( g ) + H 2

O( l ) 2 HNO 3

( aq ) + NO( g )

A)

30.8 g

B)

41.1 g

C)

54.8 g

D)

69.3 g

Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen

and 4.0 g of sodium hydroxide according to the following chemical equation:

2 S( s ) + 3 O 2

( g ) + 4 NaOH( aq ) 2 Na 2

SO

( aq ) + 2 H 2

O( l )

A)

S( s )

B)

What is the concentration of NO 3

ions in a solution prepared by dissolving 25.0 g of

Ca(NO 3

in enough water to produce 300. mL of solution?

A)

0. 254 M

B)

0. 508 M

C)

0. 672 M

D)

1.02 M

How many milliliters of a 9.0 M H 2

SO

solution are needed to make 0. 35 L of a 3.5 M

solution?

A)

  1. 14 mL

B)

0.90 mL

C)

140 mL

D)

900 mL

A FeCl 3

solution is 0.175 M. How many mL of a 0.175 M FeCl 3

solution are needed to

make 450. mL of a solution that is 0.300 M in Cl

ion?

A)

0.771 mL

B)

257 mL

C)

771 mL

D)

It is not possible to make a more concentrated solution from a less concentrated solution.

A student prepared a stock solution by dissolving 10.0 g of KOH in enough water to make

  1. mL of solution. She then took 15.0 mL of the stock solution and diluted it with enough

water to make water to make 65.0 mL of a final solution. What is the concentration of KOH

for the final solution?

A)

0. 274 M

B)

0. 356 M

C)

2.81 M

D)

3.65 M

How many grams of CaCl 2

are formed when 15.00 mL of 0.00237 M Ca(OH) 2

reacts with

excess Cl 2

gas?

2 Ca(OH) 2

( aq ) + 2 Cl 2

( g ) Ca(OCl) 2

( aq ) + CaCl 2

( s ) + 2 H 2

O( l )

A)

0.00 197 g

B)

0.00 394 g

C)

0.00789 g

D)

0.0507 g

How many milliliters of 0.200 M FeCl 3

are needed to react with an excess of Na 2

S to

produce 1.38 g of Fe 2

S

if the percent yield for the reaction is 65.0%?

3 Na 2

S( aq ) + 2 FeCl 3

( aq ) Fe 2

S

( s ) + 6 NaCl( aq )

A)

33.8 mL

When 280. mL of 1.50 × 10

M hydrochloric acid is added to 125 mL of 1.75 × 10

M

Mg(OH) 2

, the resulting solution will be

A)

acidic.

B)

basic

C)

neutral.

D)

It is impossible to tell from the information given.

Combustion analysis of 1.200 g of an unknown compound containing carbon, hydrogen,

and oxygen produced 2.086 g of CO 2

and 1.134 g of H 2

O. What is the empirical formula

of the compound?

A)

C

H

O

B)

C

H

O

C)

C

H

O

D)

C

H

O

Based on the balanced chemical equation shown below, determine the mass percent of

Fe

in a 0.7450 g sample of iron ore, if 22.40 mL of a 0.1000 M stannous chloride,

SnCl 2

( aq ), solution is required to completely react with the Fe

present in the ore

sample. The chemical equation for the reaction is

2 Fe

( aq ) + Sn

( aq ) 2 Fe

( aq ) + Sn

( aq ).

A)

B)

C)

D)

  1. Based on the balanced chemical equation shown below, determine the molarity of a

solution containing Fe

( aq ), if 40.00 mL of the Fe

( aq ) solution is required to

completely react with 30.00 mL of a 0. 250 M potassium bromate, KBrO 3

( aq ), solution. The

chemical equation for the reaction is

6 Fe

( aq ) + BrO 3

( aq ) + 6 H

( aq ) 6 Fe

( aq ) + Br

( aq ) + 3 H 2

O( l ).

A)

0. 0312 M

B)

  1. According to the balanced chemical equation

5 H

C

O

( aq ) + 2 MnO 4

( aq ) + 6 H

( aq ) 10 CO 2

( g ) + 2 Mn

( aq ) + 8 H 2

O( l )

0.3500 grams of oxalic acid, H 2

C

O

will react with ________ mL of 0.100 M potassium

permanganate, KMnO 4

solution.

A) 15.5 mL B) 38.9 mL C) 77.7 mL D) 97.2 mL

What is the reduction half reaction for the chemical reaction in a basic solution

Mn

( aq ) + 2 ClO 3

( aq ) + OH

( aq ) MnO 2

( s ) + 2 ClO 2

( aq ) + H 2

O( l )?

A)

Mn

( aq ) + 4 OH

( aq ) MnO 2

( s ) + 2 H 2

O( l ) + 2e

B)

Mn

( aq ) + 2 H 2

O( l ) MnO 2

( s ) + 4 H

( aq ) + 2e

C)

ClO 3

( aq ) + H 2

O( l ) + e

ClO 2

( aq ) + 2 OH

( aq )

D)

ClO 3

( aq ) + 2 H

( aq ) + e

ClO 2

( aq ) + H 2

O( l )

  1. Determine the number of water molecules necessary to balance the reduction half

reaction of ( )

2

( ) ___Mn

4

___MnO aq aq

  that occurs in an acidic solution.

A)

B)

C)

D)

In the unbalanced equation shown below how many moles of electrons are transferred per

mole of reducing agent?

C

O

2– ( aq ) + MnO 4

( aq ) CO 2

( aq ) + Mn

( aq )

A)

B)

C)

D)