CHM 1100 RC General Chemistry Questions

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CHM 1100 RC General Chemistry Questions

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Practice questions week 4

Answer and Explain the following practice questions.

  1. Practice questions

Top of Form What is the difference between the heat capacity and specific heat of a substance? Bottom of Form

Top of Form Question 22 Points

How does Gibbs energy, enthalpy, and entropy determine whether a process will be a spontaneous or nonspontaneous reaction?”

Bottom of Form

Top of Form Question 32 Points

Describe the differences between the first, second and third law of thermodynamics.

Bottom of Form

Top of Form Question 42 Points

Explain the difference between the 3 energy systems and provide a real-world example of a system of energy.

Bottom of Form

Top of Form Question 52 Points

Describe the difference between an exothermic and endothermic process in terms of a chemical compound or reaction.

Bottom of Form

Top of Form Question 61 Point

If the energy of the system is the sum of the energy and work, identify the following: What would be the sign of energy (Q) if the system was absorbing heat?

+Q

-Q Bottom of Form

Top of Form Question 71 Point

If the energy of the system is the sum of the energy and work, identify the following: What happens to the volume if work was done by the system?

Volume increases

Volume decreases Bottom of Form

Top of Form Question 81 Point

Solve the following thermochemical reactions:

2 HCl + Pb

eq_e5e8c0.gif

PbCl 2 + H 2

eq_e5e8ce.gif

H = -1861 J/mole

What is the enthalpy if there was 4.5 x 10 -3 g of HCl?

-1.1 x 10 J

8.375 J

-8.375 J

3.05 x 102 J Bottom of Form

Top of Form Question 91 Point

Solve the following thermochemical reactions:

2 HCl + Pb

eq_e5e84e.gif

PbCl2 + H2

eq_e5e860.gif

H = -1861 J/mole

What is the enthalpy if there was 3.86g of PbCl2?

-25.8 J

10.73 x 10-1 J

-0.577 J

1.153 J Bottom of Form

Top of Form Question 101 Point

Calculate the amount of heat absorbed or released by the following substances: 98.53g of carbon dioxide, final temperature = 30°C, initial temperature = 15°C

1.2 x 103 J

-1.2 x 10-5 J

1.2 x 108 J

1.0 x 103 J Bottom of Form

Top of Form Question 111 Point

Calculate the amount of heat absorbed or released by the following substances: 34.6g of water, final temperature = 60°C, initial temperature = 44°C

2.3 x 103 J

2.0 x 103 J

2.3 J

-2.0 x 103 J Bottom of Form

Top of Form Question 121 Point

Describe if the following reaction is spontaneous or non-spontaneous based on enthalpy, entropy and Gibbs energy:

eq_e5eab7.gif

H = 345J/mol

eq_e5eac2.gif

S = -6345J/K*mol and

eq_e5ead7.gif

G = 2355J at room temperature

Spontaneous

Not spontaneous Bottom of Form

Top of Form Question 131 Point

Describe if the following reaction is spontaneous or non-spontaneous based on enthalpy, entropy and Gibbs energy:

eq_e5ea7f.gif

H = -35J/mol,

eq_e5ea94.gif

S = 562J/K*mol, and

eq_e5eaa1.gif

G = -425J at room temperature

Spontaneous

Not spontaneous Bottom of Form

Top of Form Question 141 Point

Predict the trend of entropy in the following scenario: Freezing of water

Entropy increases

Entropy decreases

No change Bottom of Form

Top of Form Question 151 Point

Predict the trend of entropy in the following scenario: Melting of ice

Entropy increases

Entropy decreases

No change Bottom of Form

Top of Form Question 161 Point

Predict the trend of entropy in the following scenario: Entropy of vinegar v. salt

Entropy is higher

Entropy is lower

No change in entropy Bottom of Form

Top of Form Question 171 Point

Predict the trend of entropy in the following scenario: Water as ice compared to liquid

Entropy is higher

Entropy is lower

No change in entropy Bottom of Form

Top of Form Question 181 Point

Calculate the reaction entropy (S°rxn) for the following reaction: Si + 2 Cl2SiCl4

-133.84 J/mol K

126.56 J/mol K

253.12 J/mol K

794.7 J/mol K Bottom of Form

Top of Form Question 191 Point

Calculate the reaction entropy (S°rxn) for the following reaction: 4 NH+ 5 O24 NO + 6 H2O

-208.4 J/mol K

842.4 J/mol K

-419.4 J/mol K

374.2 J/mol K Bottom of Form

Top of Form Question 201 Point

If a solid substance needs 3425J of energy to increase its temperature from 24C to 98C and it has a mass of 243g, what is the specific heat of the substance?

Bottom of Form

Top of Form Question 211 Point

Calculate the Gibbs energy for the following condition K = 8.2 x 10-11, T = 35˚C

Bottom of Form

Top of Form Question 221 Point

Write out the equilibrium constant expressions for the following reaction: 2 KClO3 (s) → 2 KCl (s) + 3 O2 (g)

Bottom of Form

Top of Form Question 231 Point

Write out the equilibrium constant expressions for the following reaction: H2O (l) → H+ (aq) + OH (aq)

Bottom of Form

Top of Form Question 241 Point

Consider an exothermic reaction. How does the following action affect an equilibrium reaction by driving the reaction? Increasing the temperature of the system

Forward reaction

Reverse reaction Bottom of Form

Top of Form Question 251 Point

How does the following action affect an equilibrium reaction by driving the reaction? Removal of products

Forward reaction

Reverse reaction No 25 is multiple choice is either

  • Forward reaction
  • Reverse reaction

Bottom of Form Top of Form

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