Answer:
The correct answer is 10.939 mol ≅ 10.94 mol
Explanation:
According to Avogadro's gases law, the number of moles of an ideal gas (n) at constant pressure and temperature, is directly proportional to the volume (V).
For the initial gas (1), we have:
n₁= 1.59 mol
V₁= 641 mL= 0.641 L
For the final gas (2), we have:
V₂: 4.41 L
The relation between 1 and 2 is given by:
n₁/V₁ = n₂/V₂
We calculate n₂ as follows:
n₂= (n₁/V₁) x V₂ = (1.59 mol/0.641 L) x 4.41 L = 10.939 mol ≅ 10.94 mol
Answer:
R.F.M of Iron (II) oxide :
Moles :
Molecules :
Answer:
4
Explanation:
it will share its valence electrons with other elements to acquire noble gas confriguration of the nearest inert element.
6-(2+4)
6-6
=0 Formal charge of O atoms a and b is 0
6-(1+6)
6-7
= -1 Formal charge for O atoms c is -1
Answer 0,0,-1
