1. What is molarity of products? I can't decide if it's a. The concentration of the reactants measured in mol/L of solution or b. The concentration of the products measured in mol/L of solution
4. How does pressure relate to reaction rates? I'm stuck between a. Pressure is only important for gases or b. higher pressure in general reduces reaction rates. I think it might be B?
6. Reaction rate decreases as pressure increases. True?
1. The molarity of products refers to the concentration of the products in a chemical reaction, measured in moles per liter (mol/L) of solution.
To determine the molarity of products, you need to know the balanced chemical equation for the reaction and have the initial concentrations of the reactants. Then, based on the stoichiometry of the reaction, you can determine the amount of products formed and calculate their concentration in the solution.
For example, if the balanced chemical equation is:
A + B → C + D
And the initial concentrations of A and B are known, you can use the stoichiometry of the reaction to determine the amount of C and D formed. Dividing these amounts by the volume of the solution gives you the molarity of the products.
Therefore, the correct answer is b. The molarity of products refers to the concentration of the products measured in mol/L of solution.
4. The effect of pressure on reaction rates depends on the nature of the reaction and the phases of the reactants and products involved. In general, increasing pressure can potentially affect reaction rates for gas-phase reactions.
For gas-phase reactions, increasing pressure may favor a higher concentration of the reactant gases, leading to more frequent collisions and potentially increasing the reaction rate. So, a higher pressure can often enhance reaction rates for gas-phase reactions.
This means that the correct answer is a. Pressure is primarily important for gases when considering its influence on reaction rates.
6. The statement "Reaction rate decreases as pressure increases" is not universally true. As mentioned earlier, the effect of pressure on reaction rates depends on various factors, including the specific reaction and the phases of the reactants and products involved.
While increasing pressure can enhance reaction rates for gas-phase reactions (as explained in the previous answer), it may not necessarily hold true for reactions occurring in different phases or with different reaction mechanisms.
In summary, the effect of pressure on reaction rates can vary, and therefore, the statement that reaction rate decreases as pressure increases is not universally applicable.