A. Carbon monoxide
b. Phosphorous trichloride
c.
d.nitrogen
e. Water- Hydrogen - Oxygen
f.
Answer: Option (b) is the correct answer.
Explanation:
A spontaneous reaction is defined as the process which tends to occur on its own. It does not require any external factor or force in order to start itself.
For example, when we dissolve KCl in water then potassium chloride being ionic in nature will dissolve on its own. Hence, it will be a spontaneous process.
And, a non-spontaneous reaction is defined as a process for the completion of which we have to provide certain conditions.
Thus, we can conclude that the statement it does not require any external action to begin, is true about a spontaneous process.
Answer:
Explanation:
Single replacement:
It is the reaction in which one elements replace the other element in compound.
General equation:
AB + C → AC + B
1) zinc and Copper sulfate
Zn + CuSO₄ → ZnSO₄ + Cu
Zinc is more reactive than copper it displaces the copper from copper sulfate and form zinc sulfate.
2) Aluminium and Copper sulfate
2Al + 3CuSO₄ → Al₂(SO₄)₃ + 3Cu
Aluminium is more reactive than copper it displaces the copper from copper sulfate and form aluminium sulfate.
3) Zinc and silver nitrate
Zn + 2AgNO₃ → Zn(NO₃)₂ + 2Ag
zinc is more reactive than silver it displaces the silver from silver nitrate and form zinc nitrate.
4) copper and silver nitrate
Cu + 2AgNO₃ → Cu(NO₃)₂ + 2Ag
copper is more reactive than silver it displaces the silver from silver nitrate and form copper nitrate.
Answer: a. BaO
Explanation:
For formation of a neutral ionic compound, the charges on cation and anion must be balanced. The cation is formed by loss of electrons by metals and anions are formed by gain of electrons by non metals.
Here element barium is having an oxidation state of +2 called as 
cation and 
is an anion with oxidation state of -2. Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral 
