The empirical formula of a compound is the simplest ratio of components making up the compound.
In 100 g of compound,there's <span>66.6 g of C, 11.2 g of H and 22.2 g of O
lets calculate for 100 g of compound
C H O
mass </span> 66.6 g 11.2 g 22.2 g
number of moles 66.6/12 g/mol 11.2/1 g/mol 22.2/ 16 g/mol
= 5.55 mol =11.2 mol =1.3875 mol
divide by the least number of moles
5.55/1.3875 11.2/1.3875 1.3875/1.3875
= 4 = 8.08 = 1
round them off to the nearest whole number
C - 4
H - 8
O - 1
Therefore empirical formula of compound is C₄H₈O
Chemical equilibrium is the state in which both reactants and products are present in concentrations which have no further tendency to change with time. Usually, this state results when the forward reaction proceeds at the same rate as the reverse reaction.
Answer:
Ionization Energy increases from left to right on the periodic table. Atomic radius decreases moving left to right on the periodic table.
Atomic size gradually decreases from left to right across a period of elements. This is because, within a period or family of elements, all electrons are added to the same shell.
Answer:
So, weight per litre (1.25g/l) times 22.4 l/mole equals the mole weight (28 g/mole).
Answer:
0.0196
Explanation:
The Total volume of the solution = Volume of 
= 10 mL + 10 mL + 10 mL+ 10 mL + 1 mL + 10 mL
= 51 mL
The concentration of ![[H^+] = \dfrac{ mL \ used \times 0.1 \ M}{total \ volume}](https://tex.z-dn.net/?f=%5BH%5E%2B%5D%20%3D%20%5Cdfrac%7B%20mL%20%5C%20used%20%5Ctimes%200.1%20%5C%20M%7D%7Btotal%20%5C%20volume%7D)
= 0.0196
