Nitrogen monoxide reacts with chlorine at high temperature according to the equation, 2 NO(g) + Cl2(g) → 2 NOCl(g) In a certain reaction mixture the rate of formation of NOCl(g) was found to be 4.50 x 10‑4 mol L‑1 s‑1. What is the rate of consumption of NO(g)?

4.50 × 10⁻⁴ mol L⁻¹ s⁻¹

Explanation:

Step 1: Write the balanced equation

2 NO(g) + Cl₂(g) → 2 NOCl(g)

Step 2: Establish the appropriate molar ratio

The molar ratio of NO(g) to NOCl(g) is 2:2, that is, when 2 moles of NO(g) are consumed, 2 moles of NOCl(g) are formed.

Step 3: Calculate the rate of consumption of NO(g)

The rate of formation of NOCl(g) is 4.50 × 10⁻⁴ mol L⁻¹ s⁻¹. The rate of consumption of NO(g) is:

on passing the small ampere of electric current through the tube made of ar and hg of cfl generates uv rays which excites the fluorescent and thus emits the high radiation by consumption of just 5- 12 w in comparison to incandescent light which requires more power such as around 40 - 55 w to lighten.

moreover the life span of fluorescent or cfl is around 8000 h whereas the life span of incandescent is around 1200 h

hence, the building installed with incandescent lights bears more electricity bill.