Exams › NEET › Chemistry

For a first-order reaction with an initial concentration of 2.00 M, a time duration of 200 minutes, and a final concentration of 0.15 M, the rate constant (k) is calculated using which expression?

1. k = 2.303/t log (a/(a-x))
2. k = 2.303 log (a/(a-x))
3. k = 2.303/t log (2.00/0.15)
4. k = 2.303 log (2.00/0.15)

Correct answer: k = 2.303/t log (2.00/0.15)

Solution

The formula for the rate constant of a first-order reaction is k = (2.303/t) log (a/(a-x)). Substituting the given values (a = 2.00 M, a-x = 0.15 M, t = 200 min), the correct expression is k = 2.303/t log 2.00/0.15.

Related NEET Chemistry questions

• Why is catalyst added while preparing oxygen from decomposition of \( K C l O_{3} ? \)
• In the Arrhenius equation \( k=A e^{E / R T} \) rate will be constant at:
• As the concentration of reactants increases:
• Assertion The rate of reaction can also increase w.r.t its product if one of the product act as catalyst. Reason A catalyst lowers the activation energy of reactions. Read the above assertion and reason and choose the correct option regarding ¡t.
• Assertion Chlorine reacts more rapidly with \( \boldsymbol{H}_{2}, \) in comparision to \( \boldsymbol{O}_{\mathbf{2}} \) Reason \( D-C l \) bond is stronger in comparison to \( H-C l \) bond
• In the Haber process for the industrial manufacturing of ammonia involving the reaction \( N_{2}(g)+3 H_{2}(g) \rightleftharpoons 2 N H_{3}(g) \) at 200atm pressure in the presence of a catalyst, a temperature of about \( 500^{\circ} \mathrm{C} \) is used. This is considered as optimum temperature for the process because:

⚔️ Practice NEET Chemistry free + battle 1v1 →