What would happen to the reaction rate of a solution if 10 mL or more of water is added? Will the reaction rate increase or decrease?

The following reaction occurs without a change in the color
2A (g) + B2(g) --- 2AB (g)
a) How could you monitor the concentration of the reactants?
b) How would you determine the reaction orders?
c) How would you find the rate constant and the units for the rate constant?

Duplicate post.

What water is added it would cause concentration to go down and therefore lower reaction rate but I am not sure.

however for the second question you can monitor it by collecting gas production and measuring changed in volume/pressure also measure how long it takes for reactants to be consumed or how long it takes for products to be formed.
for b)for reaction orders you require the rate determining step or you shoudl be given a chart with trials and with different rates and concentration you can find out orders.
for c) you require the answer from b

sorry adding water does not do anything to the rate becuase it just affects concentration

To determine what would happen to the reaction rate of the solution if 10 mL or more of water is added, we need to consider the effect of water on the reaction. However, before that, let's understand how the reaction rate is affected by reactant concentrations.

a) Monitoring the concentration of the reactants:
To monitor the reactant concentrations, you can use a variety of techniques, such as spectroscopy or chemical analysis. In this case, since the reaction does not involve a change in color, spectroscopy may not be a suitable method. Instead, you can consider using a technique like titration or measuring the change in pressure if the reaction involves gases.

b) Determining the reaction orders:
To determine the reaction orders, you can use the method of initial rates. The reaction orders define how the rate of the reaction is affected by changes in the concentrations of the reactants. By measuring the initial rates of the reaction with different concentrations of reactants, you can determine the reaction orders.

For example, if the reaction rate doubles when the concentration of A doubles, the reaction is first order with respect to A. Similarly, if doubling the concentration of B quadruples the reaction rate, the reaction is second order with respect to B. By determining the reaction orders for both A and B, you can establish the overall reaction order.

c) Finding the rate constant and its units:
Once you have determined the reaction orders, you can use the rate equation to find the rate constant, which represents the specific rate of the reaction. The rate equation for a reaction can be written in the form:
rate = k[A]^x[B]^y

In this equation, k is the rate constant, [A] and [B] are the concentrations of reactants, and x and y are the reaction orders determined from the initial rate experiments.

The units for the rate constant (k) depend on the overall reaction order. If the reaction is first order, k has units of s^-1 (per second). If the reaction is second order, k has units of M^-1s^-1 (per molar per second). For different reaction orders, the units of k will vary accordingly.

Coming back to the effect of adding 10 mL or more of water, it depends on the role of water in the reaction. If water is a reactant, the increase in its concentration may affect the reaction rate. However, if water is a solvent and not directly involved in the reaction, adding more water may dilute the reactants, resulting in a decrease in the reaction rate. To determine the precise effect, further analysis of the reaction and its mechanism may be required.