Chemical Equilibrium and Thermodynamics Worksheet

Chemical Equilibrium and Thermodynamics Worksheet

11th Grade

79 Qs

quiz-placeholder

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Chemical Equilibrium and Thermodynamics Worksheet

Chemical Equilibrium and Thermodynamics Worksheet

Assessment

Quiz

Chemistry

11th Grade

Hard

NGSS
HS-PS1-5, HS-PS1-6, HS-PS1-4

+7

Standards-aligned

Created by

Mr. Poyser

Used 1+ times

FREE Resource

79 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Umar and Louis are observing a chemical reaction in their science class. Which statement is true if the free energy (ΔG) of the reaction they are studying is zero?

The rate of the forward reaction is zero.

The rate of the reverse reaction is zero.

The reaction is approaching equilibrium.

The reaction is at equilibrium.

Answer explanation

When the free energy (ΔG) of a reaction is zero, it indicates that the forward and reverse reactions occur at the same rate, meaning the system is at equilibrium.

2.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

During a chemistry experiment, Danny and Damilola add a catalyst to a reaction mixture that has reached equilibrium. The value of the equilibrium constant

decreases

increases

remains the same

Answer explanation

A catalyst speeds up the rate of reaching equilibrium but does not change the position of equilibrium or the value of the equilibrium constant. Therefore, the equilibrium constant remains the same.

3.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Jaeda and Umar are conducting an experiment. If they increase the temperature of a chemical system at constant pressure, the rate of the forward reaction will

decrease

increase

remain the same

Answer explanation

Increasing the temperature at constant pressure typically favors the endothermic direction of a reaction. If the forward reaction is endothermic, its rate will increase with temperature, making 'increase' the correct choice.

Tags

NGSS.HS-PS1-5

4.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

During a chemistry experiment, Deshaun and Jaeda are observing a reaction in a closed container. If O2 is added to the system at constant pressure and temperature, what will happen to the number of moles of HCl?

decrease

increase

remain the same

Answer explanation

Adding O2 shifts the equilibrium of the reaction involving HCl, leading to a decrease in the concentration of HCl as it reacts to form products. Therefore, the number of moles of HCl will decrease.

5.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Jaeda and Damilola are conducting an experiment with a chemical reaction at constant temperature. If they increase the pressure on the system, the value of the equilibrium constant for the reaction will

decrease

increase

remain the same

Answer explanation

Increasing pressure shifts the equilibrium towards the side with fewer moles of gas. If the reaction produces more moles of gas, the equilibrium constant will increase, making the correct answer 'increase'.

Tags

NGSS.HS-PS1-6

6.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

During a science experiment, Umar and Jaeda are investigating phase changes at 1 atmosphere of pressure. Which equilibrium is correctly associated with the Kelvin temperature at which it occurs?

ice-water equilibrium at 0 K

ice-water equilibrium at 32 K

steam-water equilibrium at 212 K

steam-water equilibrium at 373 K

Answer explanation

The steam-water equilibrium occurs at 373 K (100°C) at 1 atmosphere pressure, which is the boiling point of water. The other options incorrectly associate temperatures with their respective equilibria.

7.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Jaeda and Danny place a sealed flask of water at 298 K on their classroom desk. After some time, the water is in equilibrium with its vapor inside the flask. This is an example of:

chemical equilibrium

phase equilibrium

solution equilibrium

static equilibrium

Answer explanation

This scenario illustrates phase equilibrium, where liquid water and its vapor coexist in a sealed environment at a constant temperature. The system is balanced between the liquid and vapor phases.

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