Chemistry, asked by nitingarg7586, 10 months ago

For the reaction N₂ + 3H₂ → 2NH₃
if ∆[NH ]/∆t = 2 × 10⁻⁴ mol l⁻¹ s⁻¹, the value of ∆[H₂]/∆t
would be
(a) 1 × 10⁻⁴ mol L⁻¹ s⁻¹ (b) 3 × 10⁻⁴ mol L⁻¹ s⁻¹
(c) 4 × 10⁻⁴ mol L⁻¹ s⁻¹ (d) 6 × 10⁻⁴ mol L⁻¹ s⁻¹

Answers

Answered by HStar6389
5

Answer:

Here is your answer..

hope it helps you

Attachments:
Answered by abhi178
1

answer : option (b) 3 × 10-⁴ mol l-¹ s-¹

for chemical reaction N₂ + 3H₂ → 2NH₃

-d[N₂]/dt = -1/3 d[H₂]/dt = 1/2 d[NH₃]/dt ......(1)

given, d[NH₃]/dt = 2 × 10-⁴ mol l-¹ s-¹

we have to find d[H₂]/dt

applying equation (1)

-1/3 d[H₂]/dt = 1/2 d[NH₃]/dt

⇒-1/3 d[H₂]/dt = 1/2 × 2 × 10-⁴ = 10-⁴

⇒d[H₂]/dt = -3 × 10-⁴ mol l-¹ s-¹

hence magnitude of d[H₂]/dt = 3 × 10-⁴ mol l-¹ s-¹

hence, option (b) is correct choice.

also read similar questions : the rate of a first order reaction is 0.04 mol/L/s at 10 min and 0.03 mol/L/s at 20 min after initiation. Find the half ...

https://brainly.in/question/8658108

The Ksp for a sparingly soluble Ag2Cro4, is

4 * 10-12. The molar solubility of the salt is

(1) 2.0 10-6 mol L-1 (2) 1.0 ...

https://brainly.in/question/12167895

Similar questions