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 a solution is a measure of its concentration. It is defined as the number of moles of solute dissolved in one liter of solution.
To determine the molarity of the products in a chemical reaction, you need to know the balanced chemical equation for the reaction. The molarity of a product is the concentration of that specific product in the solution, measured in mol/L.
For example, if you have a chemical reaction where you react A + B to form C + D, the molarity of the products would be the concentration of C and D in the solution, measured in mol/L.
4. Pressure can indeed affect reaction rates, but its influence depends on the nature of the reaction.
In general, for reactions involving gases, an increase in pressure can increase the rate of reaction. This is due to the fact that higher pressure increases the number of collisions between gas molecules, and thus the chance of successful collisions leading to a reaction. So, option A is more accurate, pressure is particularly important for gas-phase reactions.
However, it's important to note that pressure does not always necessarily increase reaction rates. For reactions not involving gases, such as reactions occurring in a solution or in the solid state, pressure does not have a significant effect on the reaction rate.
6. The statement "Reaction rate decreases as pressure increases" is not universally true. It is valid for gas-phase reactions but does not apply to reactions occurring in solutions or in solids. In gas-phase reactions, increasing pressure can indeed decrease the reaction rate due to increased intermolecular collisions, leading to more frequent collisions resulting in unsuccessful reactions.
Keep in mind that the effect of pressure on reaction rates can vary depending on the specific reaction conditions, reactants, and other factors. It is always recommended to consider the particular context of the reaction when assessing the impact of pressure on reaction rates.