At a given temperature T, gases Ne, Ar, Xe and Kr are found to deviate from ideal gas behavior. Their equation of state is given as P = (RT)/(V-b) at T. Here, b is the van der Waals constant. Which gas will exhibit steepest increase in the plot of Z (compression factor) vs P?
At constant temperature of 273 K, (1)/(V) vs P are plotted for two ideal gases A and B as given below. Ratio of number of moles of A and B are:
The rate constant of most of the reaction increases with increase in temperature. According to the Arrhenius equation, k = Ae^(-E_(a)//RT) . The curve of rate constant 'k' against temperature 'T' will be.
