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Explanation
The factors that affect the reaction rate include the physical state of the reactants, the presence of a catalyst, and the reactant concentration. The physical state of the reactants can affect the surface area available for the reaction to occur, with greater surface area leading to a faster reaction rate. Catalysts can increase the rate of reaction by providing an alternative pathway with lower activation energy. The reactant concentration affects the frequency of collisions between reactant particles, with higher concentration leading to more collisions and a faster reaction rate. Therefore, all of these factors play a role in determining the reaction rate.

Explanation
The rate of appearance of NO2 is given as 6 molar/sec. Since the balanced chemical equation for the reaction is not provided, we cannot determine the stoichiometry of the reaction. Therefore, we cannot directly calculate the rate of appearance of O2. Without further information, it is not possible to determine the rate of appearance of O2.

Explanation
The rate of appearance of NO2 is given as 6 molar/sec. Since the reaction involves the disappearance of N2O5, the rate of disappearance of N2O5 can be assumed to be equal to the rate of appearance of NO2. Therefore, the rate of disappearance of N2O5 is also 6 molar/sec.

Explanation
The given equation shows that the disappearance of N2O5 is directly proportional to the appearance of O2. This means that as the amount of N2O5 decreases over time, the amount of O2 increases at the same rate. The negative sign in front of the 1/2 indicates that the two quantities have an inverse relationship, meaning that as one increases, the other decreases. Therefore, the correct answer is -1/2(N2O5/t) = O2/t.

Explanation
The overall order of a reaction is determined by the sum of the exponents (x and y) in the rate equation. In this case, since X=1 and Y=2, the sum of the exponents is 1+2=3. Therefore, the overall order of the reaction is 3.

Explanation
The correct answer is 1 because it is the second number in the given data set.

Explanation
The rate law is given as 27k[A]^x, which means the rate of the reaction is directly proportional to the concentration of A raised to the power of x. Since k is raised to the power of 3A, it can be inferred that x must be equal to 3 in order for the rate law to be consistent. Therefore, the order of x is 3.

Explanation
The rate constant of a reaction represents the speed at which the reaction occurs. It is a constant that relates the concentrations of the reactants to the rate of the reaction. In this case, the correct answer is 1.2*10^4 M^-2.s^-1. This means that the rate of the reaction is proportional to the square of the concentration of the reactants. The units M^-2.s^-1 indicate that the concentration is in moles per liter and the time is in seconds.

Explanation
The equation ln[A]t=-kt+ln[A]0 is a first order equation because it is a linear equation in the form y=mx+c, where y is ln[A]t, x is t, m is -k, and c is ln[A]0. First order equations have a linear relationship between the dependent variable (ln[A]t) and the independent variable (t), with a constant rate of change (-k).

Explanation
The given question asks to find the order of A in the reaction 2A=B. The rate constant of the reaction is given as 2.8*10^-2 s^-1 at 80°C. To find the order of A, we need to determine the relationship between the rate of the reaction and the concentration of A. Since the reaction is first order with respect to A, it means that the rate of the reaction is directly proportional to the concentration of A. Therefore, as A decreases from 0.88M to 0.14M, it will take 66 seconds for the concentration to decrease. Hence, the answer is "66s, 1st order".

Explanation
The statement is true because activation energy is the minimum amount of energy required for a chemical reaction to occur. If the activation energy is high, it means that more energy is needed for the reactants to overcome the energy barrier and form products. This results in a slower reaction rate as fewer reactant molecules possess the required energy. Conversely, if the activation energy is low, more reactant molecules have enough energy to react, leading to a faster reaction rate. Therefore, the higher the activation energy, the slower the reaction gets.

Explanation
According to the Arrhenius equation, the rate of a reaction is directly proportional to the temperature (T) and the value of the pre-exponential factor (A), and inversely proportional to the activation energy (Ea). Therefore, as the temperature increases, the rate of the reaction also increases. Similarly, as the value of the pre-exponential factor increases, the rate of the reaction increases. On the other hand, as the activation energy decreases, the rate of the reaction decreases.