What is the initial rate of reaction (in mol-L^-1s^-1) depicted by this graph? 0

Question

What is the initial rate of reaction (in mol-L^-1s^-1) depicted by this graph? 002 0.01 0.008 0.005 Which function of [X]. plotted against time, will give a straight line for a second order reaction? [X] [X]^2 In [X] 1/[X] A change in temperature from 10 degree C to 20 degree C is found to double the rate of a particular chemical reaction. How did the change in temperature affect the reacting molecules? The average velocity of the molecules doubled. The average energy of the molecules doubled. The number of collisions per second doubled. The number of molecules above the reaction energy threshold doubled. The value for the rate constant of a reaction can generally be expected to decrease with increasing temperature. increase with increasing temperature. decrease with increasing temperature only when the reaction is exothermic. increase with increasing temperature only when the reaction is exothermic. A certain reaction has a Delta H = -75 kJ and an activation energy of 40 kJ. A catalyst is found the activation energy of the forward reaction by 15 kJ. What is the activation energy of the reaction in the presence of this same catalyst? 25 kJ 60 kJ 90 kJ 10

Explanation / Answer

18)The initial rate is equal to the negative of the slope of the curve of concentration versus time at t = 0

it is 0.008(C)

19) ln[X] log of concentration vs time gives straight line(C)

20)Raising the reaction temperature by 10 °C can double or triple the reaction rate. This is due to an increase in the number of particles that have the minimum energy required. The reaction rate decreases with a decrease in temperature.(D)

21) rate constant increases with the temperature one can interpretate by arrhenius equation(B)

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