In a first-order reaction, 10% of the reactant is consumed in 25 minutes. Calculate:
(1) The half-life period of the reaction.
(2) The time required for completing 87.5% of the reaction.
Two moles of NH3 are introduced into the one-litre flask in which it dissociates at high temperature as follows: 2NH3(g) ⇌ N2(g) + 3H2(g). Determine Kc, if at equilibrium 1 mole of NH3 remains.
Write the mathematical expression relating to the variation of the rate constant of a reaction with temperature.
How can you graphically find the activation energy of the reaction from the above expression?
The slope of the line in the graph of log k (k = rate constant) versus `1/"T"` is -5841. Calculate the activation energy of the reaction.