Second Review: Acids, bases, redox, thermo, equilibrium,

If the enthalpy of formation of 1 mol of liquid water is –285.8 kJ, what is the standard enthalpy for the reaction 2H₂O(l) → 2H₂(g) + O₂(g)?

• –571.6 kJ

• –285.8 kJ

• 285.8 kJ

• 571.6 kJ

Tags

NGSS.HS-PS1-4

Hydrogen gas reacts explosively with chlorine gas to form gaseous hydrogen chloride. The chemical equation is shown. H₂(g) + Cl₂(g) → 2HCl(g) The standard enthalpy of formation of HCl gas is –92.3 kJ/mol. Based on the chemical equation, what are the respective values for the standard enthalpy of the reaction and the standard enthalpy of formation of the reactants?

• –184.6 kJ; 0 kJ

• –92.3 kJ; 0 kJ

• 0 kJ; –92.3 kJ

• 0 kJ; –46.15 kJ

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

What statement best compares the energy change during the formation of solvation shells and the energy change during the breaking of ionic bonds and intermolecular forces for the given reaction?

• energy released during formation of solvation shells < energy absorbed during breaking of bonds and intermolecular forces

• energy released during formation of solvation shells > energy absorbed during breaking of bonds and intermolecular forces

• energy absorbed during formation of solvation shells < energy released during breaking of bonds and intermolecular forces

Tags

NGSS.HS-PS1-4

The conversion of liquid water to water vapor is ____.

• endothermic

• exothermic

• both endothermic and exothermic

• neither endothermic or exothermic

Tags

NGSS.MS-PS1-4

The enthalpy of reaction for the combustion of butane is: ΔH = –2876 kJ/mol If the Bunsen burner burns 4.00 moles of butane, what is the amount of energy produced?

• 1329 kJ

• 2657 kJ

• 11,500 kJ

• 13,290 kJ

Tags

NGSS.HS-PS3-1

Magnesium metal reacts with hydrochloric acid to form magnesium chloride and hydrogen gas. Which set of conditions will raise the rate of the reaction between the metal and acid by the greatest magnitude?

• reacting magnesium metal cube and 6.0M HCl solution

• reacting magnesium metal cube and 1.0M HCl solution

• reacting magnesium metal dust and 6.0M HCl solution

• reacting magnesium metal dust and 1.0M HCl solution

Tags

NGSS.HS-PS1-5

Which letter represents the activation energy of the reaction?

• A

• B

• C

• D

Tags

NGSS.HS-PS1-4

A chemical engineer working at the ammonia synthesis plant is asked to increase the yield of ammonia by varying the temperature, pressure, and concentration conditions of the reaction. In order to achieve the desired outcome, the engineer tries to shift the equilibrium of the given reaction. What should the engineer do in order to achieve the desired outcome?

• The engineer should shift the equilibrium to the right by increasing both the concentration of nitrogen gas and the overall temperature.

• The engineer should shift the equilibrium to the right by increasing both the concentration of nitrogen gas and the overall pressure.

• The engineer should shift the equilibrium to the left by increasing both the concentration of hydrogen gas and the overall temperature.

• The engineer should shift the equilibrium to the left by increasing both the concentration of hydrogen gas and the overall pressure.

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

During one of the shifts at the plant, the shift supervisor finds that the valve of the condenser is malfunctioning. The malfunction prevents the valve from opening while the reaction is in process. This leads to an increase in volume of ammonia in the condenser. When the valve is fixed and the volume of ammonia produced is measured, it is found to be unusual. What is the most likely reason for the unusual yield of ammonia?

• As the ammonia was not withdrawn, the equilibrium to the left led to a high yield of ammonia.

• As the ammonia was not withdrawn, the equilibrium to the left led to a low yield of ammonia.

• As the ammonia was not withdrawn, the equilibrium to the right led to a high yield of ammonia.

• As the ammonia was not withdrawn, the equilibrium to the right led to a low yield of ammonia.

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

A student performs a laboratory experiment. The experiment involves dissolving ammonium nitrate in water. The chemical reaction is as follows: NH₄NO₃(s) ⇌ NH₄⁺(aq) + NO₃⁻(aq). The student measures the temperature of the solution at the start of the reaction and notices that the temperature decreases over time. The ΔH and ΔS of the reaction are both positive. Choose the correct option that indicates the type of chemical reaction occurring and the shift in equilibrium that occurs when heat is added.

• exothermic reaction; shifts to the reactants

• exothermic reaction; shifts to the products

• endothermic reaction; shifts to the reactants

• endothermic reaction; shifts to the products

Tags

NGSS.HS-PS1-4