a compound is decomposed In the laboratory and produces 1.40 g N and 0.20g H what is the empirical formula
1 answer:
First, find the number of moles for each element. The molar mass for nitrogen is 14 g/mol and that of hydrogen is 1 g/mol.
1.40 g N / 14 g/mol = 0.1 mol N
0.20 g H / 1 g/mol = 0.2 mol H
Find the mole ratio. Divide both numbers with the much lower value. In this case, it is 0.1 mol N.
For N: 0.1 ÷ 0.1 = 1
For H: 0.2÷0.1 = 2
Thus, the empirical formula is .
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Answer:
Laws governing gas behavior.
Explanation:
Boyle's law:
It relates the pressure and volume of an ideal gas at a constant temperature.
According to this law:
"The volume of a fixed amount of gas at constant temperature is inversely proportional to its pressure".
.
Charle's law:
It relates the volume and absolute temperature of an ideal gas at a constant pressure.
According to this law:
"The volume of a fixed amount of gas at constant pressure is directly proportional to its absolute temperature".
.
Avogadro's law:
According to this law:
equal volumes of all gases under the same conditions of temperature and pressure contain, an equal number of moles.
.
Ideal gas equation:
By combining all the above-stated gas laws, this equation is formed as shown below:
R is called universal gas constant.
It has a value of 0.0821L.atm.mol-1.K-1.