To answer this item, our basis is 100g. We solve for the masses of the given elements in this item,
carbon: (0.18)(100 g) = 18 g
hydrogen: (0.0226)(100 g) = 2.26 g
chlorine: (0.797)(100 g) = 17.7 g
Then, we calculate for the number of moles by dividing the masses by the molar masses of the given elements.
Number of moles:
carbon = (18 g) x (1 mol / 12 g) = 1.5 moles
hydrogen = (2.26 g) x (1 mol/ 1.01 g) = 2.23 moles
chlorine = (79.7 g) x (1 mol / 35.45 g) = 2.25 moles
We get the ratio of the number of moles by dividing them with the lowest value, 1.5.
Carbon = 1.5 moles / 1.5 = 1
Hydrogen = 2.23 moles / 1.5 = 1.48
Chlorine = 2.25 / 1.5 = 1.5
The empirical formula is,
C1H1.5CL1.5
Simplifying,
<em> C2H3Cl3</em>
The answer is letter b. from the sunlight. Plants are also referred as producers. Typically, plants gets their energy from the sun, wherein it helps them produce their own food, through the sunlight, the carbon dioxide present, the process wherein the producers undergo is known as photosynthesis.
Answer:
b. 4.4
Explanation:
pH is related to the concentration of H₃O⁺ through the following equation:
pH = -log([H₃O⁺]) = -log(4 x 10⁻⁵)
pH = 4.4
Answer : The oxidation state of nitrogen in
is, (+5)
Explanation :
Rules for the oxidation numbers :
- The oxidation number of a free element is always be zero.
- The oxidation number of a monatomic ion equal to the charge of the ion.
- The oxidation number of Hydrogen (H) is +1.
- The oxidation number of oxygen (O) in compounds is usually -2, but it is -1 in the peroxides.
- The oxidation number of a Group 1 element in a compound is +1.
- The oxidation number of a Group 2 element in a compound is +2.
- The oxidation number of a Group 17 element in a binary compound is -1.
- The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.
- The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.
The given compound is,
Let the oxidation state of 'N' be, 'x'
Hence, the oxidation state of N is, (+5)