Chemistry Reaction Rates Quiz

<p>The concentrations of reactants and products remain constant. (C)</p> Signup and view all the answers

<p>Concentration of reactants. (D)</p> Signup and view all the answers

<p>The equilibrium shifts right to remove excess heat. (B)</p> Signup and view all the answers

<p>By decreasing the reaction rate. (B)</p> Signup and view all the answers

<p>The forward rate decreases while the reverse rate increases. (C)</p> Signup and view all the answers

<p>The equilibrium shifts towards the products side. (D)</p> Signup and view all the answers

<p>It lowers the activation energy, speeding up both forward and reverse reactions. (D)</p> Signup and view all the answers

<p>To lower the activation energy required for the reaction. (C)</p> Signup and view all the answers

<p>Concentrations of products decrease, and the forward reaction rate increases. (A)</p> Signup and view all the answers

<p>The system shifts toward producing the side with fewer moles of gas. (C)</p> Signup and view all the answers

<p>Change in concentration of reactants or products per unit time (D)</p> Signup and view all the answers

<p>The presence of a catalyst (B)</p> Signup and view all the answers

<p>The minimum energy necessary for a reaction to occur (C)</p> Signup and view all the answers

<p>Cl of HCl colliding with O of water (D)</p> Signup and view all the answers

<p>More bonds are breaking and forming in a given time (C)</p> Signup and view all the answers

<p>Reaction rates are always constant throughout a reaction. (B)</p> Signup and view all the answers

<p>The molecules will bounce apart without reacting (D)</p> Signup and view all the answers

<p>Double displacement reaction (B)</p> Signup and view all the answers

<p>Higher activation energy leads to a slower reaction. (B)</p> Signup and view all the answers

<p>The collisions must occur at a specific orientation and energy. (A)</p> Signup and view all the answers

<p>The climb represents the energy required for the reaction to occur. (A)</p> Signup and view all the answers

<p>Each reaction has its own specific activation energy. (B)</p> Signup and view all the answers

<p>Ionic compounds react faster due to lower activation energies. (D)</p> Signup and view all the answers

<p>One or more original bonds must be partially broken while new bonds form. (B)</p> Signup and view all the answers

<p>Activation energy only applies to endothermic reactions. (D)</p> Signup and view all the answers

<p>Covalent reactions have higher activation energies due to bond breaking. (C)</p> Signup and view all the answers

<p>The equilibrium mixture contains more products than reactants. (D)</p> Signup and view all the answers

<p>K increases or decreases depending on the reaction type. (B)</p> Signup and view all the answers

<p>The equilibrium will shift to increase the concentration of products. (C)</p> Signup and view all the answers

<p>The rates temporarily become unequal until equilibrium is reestablished. (C)</p> Signup and view all the answers

<p>The forward reaction will speed up to create more products. (A)</p> Signup and view all the answers

<p>The forward reaction produces a small amount of products. (A)</p> Signup and view all the answers

<p>It speeds up both the forward and reverse reactions equally. (C)</p> Signup and view all the answers

<p>The rates of the forward and reverse reactions are equal and constant. (A)</p> Signup and view all the answers

The change in concentration of a reactant or product over a specific unit of time.

The study of how fast chemical reactions happen.

The minimum energy required for a collision between reacting molecules to result in a successful reaction.

A theory explaining how reactions occur. It states that molecules must collide with sufficient energy and proper orientation to break bonds and form new ones.

The specific arrangement of atoms and molecules during a collision for a reaction to occur.

The amount of energy possessed by molecules during a collision, influencing the possibility of a reaction.

A chemical equation showing only the ions directly involved in the reaction.

A substance that speeds up a reaction without being consumed in the process.

Increasing the concentration of reactants causes more collisions, making a reaction faster.

A higher temperature means molecules move faster, leading to more effective collisions and a faster reaction.

When a catalyst is in a different phase (solid, liquid, gas) than the reactants.

When a catalyst and reactants are in the same phase (solid, liquid, gas).

When a reaction proceeds in both directions, reactants forming products and products forming reactants.

The state where the forward and reverse reaction rates are equal. No net change in concentrations.

Reactions with low activation energies tend to be faster, while reactions with high activation energies are slower.

The activation energy is inversely related to the rate of the reaction, meaning that a lower activation energy results in a faster reaction.

A point at which reactant bonds are partially broken, and new bonds are forming, representing a high-energy, unstable intermediate state.

The energy difference between the reactants and the products. Positive for endothermic reactions, meaning energy is absorbed. Negative for exothermic reactions, where energy is released.

Ionic compounds in aqueous solutions typically react faster than covalent compounds because they have lower activation energies, as they usually don't involve breaking covalent bonds.

The nature of the reactants, specifically their bond strengths, significantly influences the reaction rate. Stronger bonds require more energy to break, resulting in slower reactions.

Factors that affect reaction rate include the nature of the reactants, surface area, temperature, concentration, and the presence of a catalyst.

A state where the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products.

A numerical value that represents the ratio of products to reactants at equilibrium.

A larger K value indicates that the forward reaction is favored, resulting in more products at equilibrium.

A smaller K value indicates that the reverse reaction is favored, resulting in more reactants at equilibrium.

States that when a change is applied to a system at equilibrium, the system will shift in a way that relieves the stress and re-establishes equilibrium.

Adding a reactant shifts the equilibrium towards product formation, while removing it shifts it towards reactant formation. The same applies to adding or removing products.

A change in temperature can alter the equilibrium constant (K), favoring either the forward or reverse reaction depending on whether the reaction is exothermic or endothermic.

The equilibrium position shifts towards the side with fewer moles of gas when pressure increases. This is because the system tries to relieve the stress of increased pressure by minimizing the number of gas molecules.

A catalyst speeds up both the forward and reverse reactions equally. It doesn't change the equilibrium position because it allows reactants and products to reach equilibrium faster.

Adding heat to an endothermic reaction favors the product formation. This is because the system absorbs heat to counteract the added heat.

Adding heat to an exothermic reaction favors the reactant formation. This is because the system releases heat to counteract the added heat.

The equilibrium position shifts towards the side with fewer moles of gas when pressure decreases. This is because the system tries to relieve the stress of decreased pressure by maximizing the number of gas molecules.