The ionization constant equation is:
=1.0 × 
at 25°C
the option is 1.
Explanation:
Sometimes in pure water one proton of the water molecule(hydrogen ion) will get attracted to the lone pairs present in another water molecule.This causes the hydrogen ion to leave the present water(leaving the 
behind) molecule ad gets attached to another water molecule leading to the formation of the hydronium ion(
,hydronium ion).
This process is called auto-ionization of water because the water molecule ionizes into 
and ions.
<h2>
<u>
+</u>
<u>
→</u>
<u>
+ </u>
</h2>
As such the equilibrium constant,which is measure of concentration of products to concentration of reactants,will be very slow.
∴the ionization constant of water at 25°C is 1.0 × .
(i.e.)option<u> c</u> is correct answer []=[]
Answer:
Explanation:
2Al(s) + 3 2 O2(g) → Al2O3(s) And given the stoichiometry ...and EXCESS dioxygen gas...we would get 6.25⋅ mol of alumina. the which represents a mass... ...6.25 ⋅ mol ×101.96 ⋅ g ⋅ mol−1 molar mass of alumina ≡ 637.25 ⋅ g.
Answer:
Heat, energy that is transferred from one body to another as the result of a difference in temperature.
Explanation:
The molar mass of Na₂SO₄ -
2 x Na - 2 x23 = 46
1 x S - 1 x 32 = 32
4 x O - 4 x 16 = 64
total = 46 + 32 + 64 = 142 g/mol
the molarity of solution - 2.0 M
in 1 L of solution , 2.0 moles
Therefore in 2.5 L - 2 mol/L x 2.5 L = 5 mol
then the mass of Na₂SO₄ required = 142 g/mol x 5 mol = 710 g
Answer:
5.34 moles of 
are required to produce 3.56 mol of 
.
0.83 moles of water react with 2.5 moles of .
Explanation:
i) 
Moles of we want to produce = 3.56 moles
According to reaction, 2 moles of are obtained from 3 moles of
Then 3.56 moles of will be obtained from :
of
5.34 moles of are required to produce 3.56 mol of .
ii)
Moles of = 2.5 moles
According to reaction,3 moles of reacts with 1 mole of 
,then 2.5 moles of will react with :
of
0.83 moles of water react with 2.5 moles of .
