Jeopardy Game

Chemical Compounds

100

Identify the type of chemical reaction in the following equation:

2H₂+O₂→2H₂O

This is a synthesis reaction because two elements combine to form a compound.

200

Classify the following reaction as either synthesis, decomposition, single replacement, double replacement, or combustion:

C₃H₈+5O₂→3CO₂+4H₂O  

This is a combustion reaction because a hydrocarbon reacts with oxygen to produce carbon dioxide and water.

300

Balance the following chemical equation for the decomposition of potassium chlorate (KClO3) when it decomposes to form potassium chloride (KCl) and oxygen gas (O2). Then, identify the type of reaction.

KClO₃→KCl+O₂  

• 2KClO₃→2KCl+3O₂

• This is a decomposition reaction, as potassium chlorate breaks down into two simpler substances: potassium chloride and oxygen gas.

400

How many moles of H₂ are required to fully react with 0.75 moles of N₂ in the reaction below? Also, balance the equation.

4. N2+3H2→2NH3

   Using stoichiometry, 0.75 moles of N₂ require 0.75×3=2.25 moles of H2.

500

Calculate the mass of CO₂ produced when 5.0 grams of C₂H₅OH (ethanol) undergoes complete combustion. Molar mass: C₂H₅OH=46.07 g/mol, CO₂=44.01 g/mol

C₂H₅OH + O₂ → CO₂ +H₂O

1. C₂H₅OH + 3O₂ → 2CO₂ +3H₂O

2. 5.0g/ 46.07 g/mol = 0.1085 mol C₂H₅OH

3. Using the molar ratio C₂H₅OH: CO₂ =1:2, moles of CO₂ produced: 0.1085 x 2=0.217 mol CO₂ 

4. Mass of CO₂: 0.217 mol x 44.01 g/mol= 9.55 g CO₂ 

Reactions and Stoichiometry

100

If you have the balanced chemical equation for the combustion of propane (C₃H₈):

C₃H₈ + 5O₂ → 3CO₂ + 4H₂O

How many moles of CO₂ are produced when 2 moles of C₃H₈ are completely combusted?

6 moles of CO₂

200

If the reaction between sodium bicarbonate and acetic acid, the following balanced eqaution applies:

NaHCO₃ +CH₃COOH → CH₃COONa + H₂O +CO₂

If you start with 4 moles of sodium bicarbonate,how many moles of carbon dioxide (CO₂) will be produced?

4 moles of CO₂

300

In the reaction between nitrogen gass and hydrogen gas to form ammonia:

N₂ +H₂ → NH₃

If you start with 10 moles of H₂ and excess N₂, how many moles of NH₃ can be produced?

NH₃= (2 moles NH₃/ 3 moles H₂₎ x 10 moles H₂

= 20/3

=6.67 moles NH₃

400

Ammonium sulfate can be formed from the reaction of ammonia and sulfuric acid. Write the balanced equation for this reaction and calculate the mass of ammonium sulfate produced if you react 34 grams of ammonia with excess sulfuric acid"

2NH₃ + H₂SO₄→ (NH₄)₂SO₄

132.14 g (NH₄)₂SO₄

500

Given the reaction between iron (III) chloride (FeCl₃) and sodium hydroxide (NaOH) to form iron (III) hydroxide (Fe(OH)₃) and sodium chloride (NaCl)

FeCl₃ + 3NaOH → Fe(OH)₃ + 3NaCl

If you have 30 grams of FeCl₃ and an excess of NaOH, how many grams of Fe(OH)₃ can be produced?

49.38 grams of Fe(OH)₃

Chemical Equilibrium

100

Define chemical equilibrium

Chemical equilibrium is the state in a reversible reaction where the forward and reverse reaction rates are equal, resulting in no net change in the concentrations of reactants and products.

200

What is the equilibrium constant (K) for the reaction of aA +bB⇌ cC + dD

K=[C]c[D]d/[A]a[B]b

300

Explain what the reaction quotient (Q) represents and how it can be used to predict the direction in which a reaction will proceed to reach equilibrium.

The reaction quotient Q has the same expression as the equilibrium constant but is calculated using initial (not necessarily equilibrium) concentrations of reactants and products. If Q<K, the reaction will proceed forward to form more products. If Q>K, the reaction will shift in the reverse direction to produce more reactants. If Q=K, the system is at equilibrium.

400

For the reaction 2NO₂ ⇌ N₂O_4, the equilibrium constant K_c is 170 at a certain temperature. If the concentration of NO₂ is 0.30 M at equilibrium, calculate the concentration of N₂O_4.

K_c= [N₂O₄]/[NO₂]²

[N₂O_4]=K_c x [NO₂]²

=170 x (0.30)²

=170 x 0.09

=15.3 M

500

In a closed 5.0 L container, dinitrogen tetroxide decompises at high temperatures into nitrogen gas. The reaction is as follows: N₂O_4⇌ 2NO₂

If at equilibrium, the concentration of NO₂ is found to be 0.60 mol/L, calculate the equilibrium constant K_c for the reaction at this temperature. What will happen to the equilibrium position if more N₂O₄ gas is added to the system?

K_c= (0.60)²/0.30

=1.20

Reactions in Aqueous solutions and Oxidation-reduction reaction

100

Explain the significance of oxidation and reduction in terms of electron transfer and its importance in chemical reactions.

Oxidation and reduction are processes involving the transfer of electrons between chemical species. Oxidation is the loss of electrons, while reduction is the gain of electrons. These reactions are crucial in energy production, metabolism, and various industrial processes. They drive processes in electrochemical cells, where electrons are transferred to generate electric current.

200

Identify the oxidizing and reducing agents in the following redox reaction and explain your reasoning:

Zn +Cu²⁺ →  Zn ²⁺ + Cu

1. The oxidizing agent is Cu²⁺ because it gains electrons to form Cu.

2. The reducing agent is Zn because it loses electrons to form Zn ²⁺

300

Determine whether the following reaction is a redox reaction. If it is, identify the species being oxidized and reduced, and explain your reasoning: 

2H₂+O₂ → 2H₂O

1. Yes, this is a redox reaction.

2. H₂ is oxidized as it goes from an oxidation state of ) in H₂ to +1 in H₂O, losing electrons.

3. O₂ is reduced as it goes from an oxidation state of O in O₂ to -2 in H₂O, gaining electrons.

400

Write the net ionic equation for the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH\) in aqueous solution.

HCl + NaOH → NaCl + H₂O

H⁺ + OH →  H₂O

500

Write the net ionic equation for the reaction that occurs when sulfuric acid (H₂SO₄) is mixed with barium hydroxide (Ba(OH)₂) in aqueous solution.

Ba²⁺ + SO₄^2- → BaSO₄

Chemical Safety

100

Explain the proper steps to take when a chemical spill occurs in the laboratory. Include specific procedures for different types of spills (e.g., acid, base, solvent) and how to ensure the safety of yourself and others during the response.

When a chemical spill occurs, the following steps should be taken:

• Assess the situation: Determine the type and quantity of the spilled chemical. If it is a hazardous material, evacuate the area and inform others.
• Activate the emergency alarm if necessary and call for help.
• Personal protective equipment (PPE): Ensure you are wearing appropriate PPE, such as gloves, goggles, and lab coats.
• Contain the spill: For small spills, use absorbent materials specific to the chemical type (e.g., neutralizing agents for acids or bases). For large spills, cordon off the area to prevent exposure.
• Notify a supervisor or lab manager: Report the spill immediately and follow institutional protocols for spill management.
• Follow disposal procedures: Collect the materials used for cleanup and dispose of them according to your institution's waste disposal guidelines.

200

Describe the emergency preparedness and response procedures you should follow in the event of a fire in the laboratory. Include details on the use of fire extinguishers and evacuation routes.

In the event of a fire in the laboratory, follow these emergency preparedness and response procedures:

• Alert: Immediately notify everyone in the lab of the fire and activate the fire alarm.
• Evacuate: Follow the designated evacuation routes to exit the building safely. Do not use elevators.
• Extinguish: If the fire is small and manageable, use the appropriate fire extinguisher (e.g., Class B for flammable liquids) to extinguish it. Remember the PASS method: Pull the pin, Aim at the base, Squeeze the handle, and Sweep side to side.
• Close doors as you leave to contain the fire.
• Call 911 or your emergency response number once you are in a safe location. Provide details about the fire and any hazardous materials involved.
• Do not re-enter the building until it is deemed safe by emergency personnel.

300

When handling chemicals, why is it essential to wear personal protective equipment (PPE) such as goggles and gloves? Discuss the specific hazards that each type of PPE protects against and the consequences of neglecting to use them.

Wearing PPE such as goggles and gloves is crucial for several reasons:

• Goggles protect the eyes from chemical splashes, airborne particles, and intense light that can cause severe eye injuries or blindness. Neglecting to wear goggles can lead to irreversible damage from exposure.
• Gloves safeguard the skin from direct contact with hazardous substances, which can cause burns, allergic reactions, or absorption of toxic chemicals. Failure to wear gloves can result in chemical burns or systemic toxicity if harmful substances penetrate the skin.
• Proper PPE use significantly reduces the risk of injuries and promotes a safer laboratory environment. Neglecting to use appropriate PPE may lead to accidents that compromise the health and safety of individuals and the laboratory.

400

Explain the significance of following chemical safety protocols during laboratory work. How do these protocols help prevent accidents and ensure a safe working environment?

• Accident Prevention: Protocols provide guidelines for safe handling, storage, and disposal of chemicals, minimizing the risk of spills, exposures, and accidents.
• Consistent Training: Adhering to safety protocols fosters a culture of safety and ensures that all personnel are trained and aware of potential hazards and emergency procedures.
• Legal Compliance: Compliance with safety regulations protects individuals and institutions from legal liabilities and penalties associated with unsafe practices.
• Incident Preparedness: Established protocols ensure that all personnel know how to respond appropriately in emergencies, which can significantly mitigate injury and damage.

500

When working with strong acids in the laboratory, what specific safety measures should be implemented to protect personnel from exposure and potential accidents? Include measures for both handling and disposal of acids.

• Personal Protective Equipment (PPE): All personnel must wear appropriate PPE, including acid-resistant gloves, safety goggles or face shields, and lab coats. Additionally, face shields should be used when there is a risk of splashing.

• Ventilation: Ensure that the laboratory is well-ventilated, preferably with a fume hood in use, to prevent the accumulation of harmful vapors. Always conduct acid handling and transfers inside the fume hood.

• Proper Storage: Store acids in designated acid cabinets made of compatible materials that can withstand corrosion. Ensure that containers are labeled correctly and kept tightly closed when not in use.

• Dilution Protocol: Always add acid to water (never water to acid) to minimize the risk of exothermic reactions that can cause splattering or boiling. Use a graduated cylinder for precise measurements and slow addition.

• Emergency Equipment: Have access to an eyewash station and safety shower within the immediate area. Ensure that neutralizing agents (e.g., sodium bicarbonate for acid spills) are available and that personnel know how to use them.

• Spill Response: Implement a clear protocol for dealing with acid spills. This includes evacuating the area, containing the spill with absorbent materials suitable for acids, and notifying appropriate personnel for cleanup.

• Disposal Protocols: Follow institutional and regulatory guidelines for acid disposal. Use designated waste containers for acidic waste, and ensure they are clearly labeled. Never pour acids down the sink unless specifically allowed by local regulations.

• Training: Ensure all personnel are trained in the properties of the acids being used, the associated risks, safe handling techniques, and emergency response procedures.