Allie De la Llana
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Basic Chemistry 1 Final Exam Review, based off lecture and labs 6-9.

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Allie De la Llana
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Chemistry I Final Exam Review

Chemistry I Final Exam Review

Question 1 of 19

1

A piece of metal weighing 59.047 g was heated to 100ºC and then put into 100 mL of water (initially at 23.7ºC). The metal and water were allowed to an equilibrium temperature, determined to be 27.8ºC. Assuming no heat lost to the environment, calculate the specific heat of the metal. Specific Heat of water = 4.18J/gºC Density of water = 1.00g/mL

Select one of the following:

  • 0.623 J/gºC

  • 1.79 J/gºC

  • 0.402 J/gºC

  • 0.721 J/gºC

Explanation

Question 2 of 19

1

In an experiment, 700 mL of 0.5 M hydrochloride acid (HCl) is added to 600 mL of of 0.5 M sodium hydroxide (NaOH) solution. The acid and base neutralize each other according to the equation: HCl + NaOH --> NaCl + H2O
How many moles of acid and base were there originally?

Select one of the following:

  • 0.35 mole of HCl and 0.3 mole of NaOH

  • 0.08 mole of HCl and 0.18 mole of NaOH

  • 0.035 mole of HCl and 0.05 mole of NaOH

  • 0.05 mole of HCl and 0.03 mole of NaOH

Explanation

Question 3 of 19

1

A chemist wants to determine the enthalpy of neutralization for the following reaction: HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O (l)

The chemist uses a coffee-cup calorimeter to neutralize completely 70.5 mL of 2.56 M HCl (aq) with 30.5 mL of 2.56 M NaOH (aq). The initial temperature of both solutions is 16.8ºC. After neutralization, the highest recorded temperature is 22.6ºC. Calculate the enthalpy of neutralization in kJ/mol of H2O.
Assume that the density of the solution is 1.00 g/mL and specific heat is 4.18 J/gºC

Select one of the following:

  • -29.2 kJ/mol

  • 29.2 kJ/mol

  • -31.4 kJ/mol

  • 31.4 kJ/mol

Explanation

Question 4 of 19

1

Use the periodic table to predict which element has the largest ionization energy.

Select one of the following:

  • H

  • He

  • Fr

  • Rn

  • Rh

Explanation

Question 5 of 19

1

Use the periodic table to predict which element has the largest atomic radius.

Select one of the following:

  • H

  • He

  • Fr

  • Rn

  • Rh

Explanation

Question 6 of 19

1

Which of the following is a transition element?

Select one of the following:

  • H

  • He

  • Fr

  • Rn

  • Rh

Explanation

Question 7 of 19

1

The element germanium (Ge) is used in the manufacture of some transistors. What other element might be used for such a purpose?

Select one of the following:

  • Ga

  • Se

  • Si

  • Pb

  • Tl

Explanation

Question 8 of 19

1

When the excess of calcium carbonate is added to dilute HCl, the reaction gradually becomes slower and finally stops. Which statement best explains why this happens?

Select one of the following:

  • An insoluble layer of calcium chloride is formed on the calcium carbonate.

  • The concentration of HCl gradually reduces to zero.

  • The pieces of calcium carbonate gradually become smaller.

  • The calcium carbonate is covered by bubbles of carbon dioxide.

Explanation

Question 9 of 19

1

The molar volume of a gas-

Select one of the following:

  • is commonly used in calculations as 22.4 L/mol at STP

  • of 22.4 L/mol at STP is considered to be absolutely true only for ideal gases

  • will change if the temperature and/or pressure change

  • All of the above are true

Explanation

Question 10 of 19

1

In the reaction CH4 (g) + 2O2 (g) --> CO2 (g) + 2H2O (g)
18 L of oxygen would produce how many L of CO2 at STP?
(Hint: You must first balance the equation.)

Select one of the following:

  • 0.40 L

  • 9 L

  • 18 L

  • 36 L

Explanation

Question 11 of 19

1

A metal was found to release -1246 J of energy in a calorimeter. Initial temperature was 40.0ºC and the final temperature was 2.00ºC. The specific heat of the metal is 3.14 J/gºC, what is the mass of the metal used?

Select one of the following:

  • 4.40 g

  • 16.5 g

  • 9.44 g

  • 10.4 g

Explanation

Question 12 of 19

1

What is the mass in grams of 17.0 liters of methane gas (CH4) at STP?
MM of CH4 = 16.04 g/mol

Select one of the following:

  • 0.0473 g

  • 23.7 g

  • 6100 g

  • 12.2 g

Explanation

Question 13 of 19

1

During a Carbonate Analysis experiment, a 0.306 g sample of a CaCO3 "mixture" was used to collect 0.061 g CO2. Determine the mass of CaCo3 in the original mixture.
CaCO3 (g) + 2H3O+ (aq) --> Ca2+ (aq) + 2H2O (l) + CO2 (g)
MM of CaCO3 = 100.09 g/mol
MM of Co2 = 44.01 g/mol

Select one of the following:

  • 43.8 %

  • 75.6%

  • 45.4 %

  • 78.4 %

Explanation

Question 14 of 19

1

A 3 M HCl solution was used to generate the CO2 from the CaCO3 mixture. What would be the effect on the calculations if 6 M HCl was substituted for the 3 M HCl?

Select one of the following:

  • no affect as long as the 3 M HCl is in access

  • calculations would be too low

  • calculations would be too high

  • calculations can not be completed

Explanation

Question 15 of 19

1

Electrons are lost by the-

Select one of the following:

  • reducing agent as it undergoes oxidation

  • reducing agent as it undergoes reduction

  • oxidizing agent as it undergoes oxidation

  • oxidizing agent as it undergoes reduction

Explanation

Question 16 of 19

1

Phenolphthalein is ______ in basic solutions but _____ in acidic solutions.

Select one of the following:

  • pink; colorless

  • blue; colorless

  • colorless; blue

  • colorless; pink

Explanation

Question 17 of 19

1

In a titration, 34.12 mL of HCl required 42.03 mL of a 0.9981 M NaOH solution to reach the endpoint. Calculate moles of NaOH dispensed.

Select one of the following:

  • 0.03406 mol

  • 1.229 mol

  • 0.04195 mol

  • 41.95 mol

Explanation

Question 18 of 19

1

What is the difference between the endpoint and stoichiometric point in a strong acid/base titration?

Select one of the following:

  • The endpoint is when the pH is exactly 7

  • The stoichiometric point is when the pH is exactly 7

  • The endpoint and the equivalence point are the same thing

  • None of these answers are correct

Explanation

Question 19 of 19

1

At 16.7 mL volume of a 0.0861 M NaOH solution neutralizes 20.0 mL of HCl acid. What is the molar concentration of the HCl solution?

Select one of the following:

  • 0.0710 M

  • 0.0625 M

  • 0.0725 M

  • 0.0719 M

Explanation

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