Chemical Kinetics and Nuclear ChemistryMedium
Question
Consider the chemical reaction N2(g) + 3H2(g) → 2NH3(g). The rate of this reaction can be expressed in terms of time derivative of concentration of N2(g), H2(g) or NH3(g). Identify the correct relationship amongst the rate expressions.
Options
A.Rate $= - \frac{d\left\lbrack N_{2} \right\rbrack}{dt} = - \frac{1}{3}\frac{d\left\lbrack H_{2} \right\rbrack}{dt} = + \frac{1}{2}\frac{d\left\lbrack NH_{3} \right\rbrack}{dt}$
B.$= - \frac{d\left\lbrack N_{2} \right\rbrack}{dt} = - 3\frac{d\left\lbrack H_{2} \right\rbrack}{dt} = + 2\frac{d\left\lbrack NH_{3} \right\rbrack}{dt}$
C.$= - \frac{d\left\lbrack N_{2} \right\rbrack}{dt} = \frac{1}{3}\frac{d\left\lbrack H_{2} \right\rbrack}{dt} = + \frac{1}{2}\frac{d\left\lbrack NH_{3} \right\rbrack}{dt}$
D.$= - \frac{d\left\lbrack N_{2} \right\rbrack}{dt} = - \frac{d\left\lbrack H_{2} \right\rbrack}{dt} = + \frac{d\left\lbrack NH_{3} \right\rbrack}{dt}$
Solution
$r = - \frac{d\left\lbrack N_{2} \right\rbrack}{dt} = - \frac{1}{3}.\frac{d\left\lbrack H_{2} \right\rbrack}{dt} = + \frac{1}{2}\frac{d\left\lbrack NH_{3} \right\rbrack}{dt}$
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