Question
Why does water covered with excessive algal growth become polluted?

Answer

Water containing algae have a very less amount of oxygen as the algae consume most of the oxygen dissolved in the water, and thus deprive aquatic plants and oxygen of it, and hence kill them. This results in eventual loss of biodiversity and thus, the balance of nature is broke. This is a kind of pollution it makes happen.
This condition is called- Eutrophication.
Some algae even produce toxins that are harmful to higher forms of life.
P.S.- Algae are formed mostly by addition of chemical fertilisers containing phosphates, which enhance algae growth)

Need a full question paper?

Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.

Start Generating Free

Similar questions

i. Arrange $\mathrm{NH}_3, \mathrm{PH}_3, \mathrm{AsH}_3, \mathrm{SbH}_3$ in increasing order of boiling point.
ii. Identify complex, interstitial, covalent and polymeric hydrides from the following.
$\mathrm{BeH}_2, \mathrm{AsH}{ }_3, \mathrm{LaH}_3, \mathrm{LiAlH}_4$.
Write a relation between $\Delta\text{G}$ and Q and define the meaning of each term and answer the following:
  1. Why a reaction proceeds forward when Q < K and no net reaction occurs when Q = K.
  2. Explain the effect of increase in pressure in terms of reaction quotient Q. for the reaction: $\text{CO(g)}+\text{3H}_2\text{(g)}\rightleftharpoons\text{CH}_4\text{(g)}+\text{H}_2\text{O(g)}$
Energy of an electron in the ground state of the hydrogen atom is –2.18×10–18J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol–1.
Hint: Apply the idea of mole concept to derive the answer.
From where does ozone come in the photochemical smog?
  1. What are the reactions involved in removing $\text{SO}_2$ from the atmosphere by passing it through a solution containing citrate ions?
  2. What is the most important sink of CO pollutant?
  3. How are fuel gases from industries freed from oxides of nitrogen and sulphur?
Complete the following reactions:
  1. $\text{SO}_3+\text{D}_2\text{O}\xrightarrow{\ \ \ \ \ \ \ \ \ }$
  2. $2\text{Na}+2\text{D}_2\text{O}\xrightarrow{\ \ \ \ \ \ \ \ }$
  3. $\text{P}_2\text{O}_5+\text{D}_2\text{O}\xrightarrow{\ \ \ \ \ \ \ \ \ }$
Find:
  1. The total number and.
  2. The total mass of neutrons in 7 mg of 14C.
(Assume that mass of a neutron = 1.675 × 10–27kg).
Fluorine reacts with ice and results in the change:
$H_2O(s) + F_2(g) → HF(g) + HOF(g)$
Justify that this reaction is a redox reaction.
Account for the following.
  1. CO is used in the extraction of metals.
  2. CO is poisonous.
  3. $\mathrm{CO}_2$ is used in referigeration.
What do you understand by:
  1. Electron-deficient.
  2. Electron-precise, and
  3. Electron-rich compounds of hydrogen? Provide justification with suitable examples.