Unit 9 - Kinetics and Equilibrium: Quizziz

For a reaction system at equilibrium, LeChatelier’s principle can be used to predict the

• activation energy for the system

• type of bonds in the reactants

• effect of a stress on the system

• polarity of the product molecules

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In terms of entropy and energy, systems in nature tend to undergo changes toward

• lower entropy and lower energy

• lower entropy and higher energy

• higher entropy and lower energy

• higher entropy and higher energy

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Based on Table I, what is the ΔH value for the production of 1.00 mole of NO₂(g) from its elements at 101.3 kPa and 298 K?

• 33.2 kJ

• -33.2 kJ

• 132.8 kJ

• -132.8 kJ

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Systems in nature tend to undergo changes toward

• lower energy and lower entropy

• lower energy and higher entropy

• higher energy and lower entropy

• higher energy and higher entropy

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A chemical reaction occurs when reactant particles

• are separated by great distances

• have no attractive forces between them

• collide with proper energy and proper orientation

• convert chemical energy into nuclear energy

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Given the balanced equation representing a reaction:

CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g) + energy

Which change in reaction conditions will increase the frequency of effective collisions between reactant molecules?

• decreasing the pressure of the reactants

• decreasing the temperature of the reactants

• increasing the concentration of the reactants

• increasing the volume of the reactants

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The energy absorbed and the energy released during a chemical reaction are best represented by a

• cooling curve

• heating curve

• kinetic energy diagram

• potential energy diagram

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The amount of randomness of the atoms in a system is an indication of the

• entropy of the system

• polarity of the system

• excited state of the atoms

• ground state of the atoms

A reaction is most likely to occur when the colliding particles have proper orientation and

• mass

• volume

• half-life

• energy

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Given the equation representing a chemical reaction at equilibrium in a sealed, rigid container:

When the concentration of H₂(g) is increased by adding more hydrogen gas to the container at constant temperature, the equilibrium shifts

• to the right, and the concentration of HI(g) decreases

• to the right, and the concentration of HI(g) increases

• to the left, and the concentration of HI(g) decreases

• to the left, and the concentration of HI(g) increases

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