1 L ---------- 1000 mL
274 L ------- ??
274 x 1000 / 1 => 2,740 mL
hope this helps!
Answer:
Explanation:
2K + Cl₂ ⟶ 2KCl
n/mol: 2.00
2 mol of KCl are formed from 2 mol of K
Answer:
The sample obtained from the environment has a higher mass
Explanation:
A simple way to put the answer is that the element carbon -as found in nature- has a molar mass of 12.0107 g/mol, because there are a few isotopes of 14C and 13C; and <em>the molar mass is an expression of the isotopes' natural abundance</em>.
So 1 mole of carbon obtained from the environment would weigh 12.0107 g, while a sample of isotopically pure carbon would weigh 12.0000 g.
For a) [Ru(NH₃)₅Cl]SO₄
Ru configuration = d⁶s²
In this complex Ru oxidation number is +3
Ru³⁺ configuration = d⁵
number of
electrons = 5
For b) Na₂[Os(CN)₆]
Os configuration = d⁶s²
In this complex Os oxidation number is +4
Os⁴⁺ configuration = d⁴
number of
electrons = 4
The first dissociation for H2X:
H2X +H2O ↔ HX + H3O
initial 0.15 0 0
change -X +X +X
at equlibrium 0.15-X X X
because Ka1 is small we can assume neglect x in H2X concentration
Ka1 = [HX][H3O]/[H2X]
4.5x10^-6 =( X )(X) / (0.15)
X = √(4.5x10^-6*0.15)
∴X = 8.2 x 10-4 m
∴[HX] & [H3O] = 8.2x10^-4
the second dissociation of H2X
HX + H2O↔ X^2 + H3O
8.2x10^-4 Y 8.2x10^-4
Ka2 for Hx = 1.2x10^-11
Ka2 = [X2][H3O]/[HX]
1.2x10^-11= y (8.2x10^-4)*(8.2x10^-4)
∴y = 1.78x10^-5
∴[X^2] = 1.78x10^-5 m