5.6g of an organic compound on burning with excess oxygen gave 17.6g of carbon dioxide nd 7.2g of water what is the organic compound
find the moles of C in the CO2 , and the moles of H in the H2O
that is the C/H ratio in the compound
To determine the organic compound from the given data, you need to consider the balanced chemical equation for the combustion of organic compounds.
The general equation for the combustion of an organic compound can be represented as follows:
CₓHᵧ + O₂ → CO₂ + H₂O
Here, the organic compound is represented by the formula CₓHᵧ, which contains unknown values of x and y. We need to find the specific combination of x and y.
To find the value of x, compare the number of carbon atoms on both sides of the equation. In this case, 1 carbon atom can be found in each molecule of carbon dioxide (CO₂). Since 17.6g of CO₂ are produced, the mass of carbon dioxide corresponds to the mass of carbon in the organic compound.
Using the molar mass of carbon dioxide (44 g/mol), we can calculate the moles of carbon:
moles of carbon = mass of CO₂ / molar mass of CO₂
= 17.6 g / 44 g/mol
≈ 0.4 mol
Since 1 mole of CₓHᵧ contains 1 mole of carbon, we can conclude that x = 0.4.
To find the value of y, compare the number of hydrogen atoms on both sides of the equation. Each molecule of water (H₂O) contains two hydrogen atoms. Thus, the mass of water produced corresponds to the mass of hydrogen in the organic compound.
Using the molar mass of water (18 g/mol), we can calculate the moles of hydrogen:
moles of hydrogen = mass of H₂O / molar mass of H₂O
= 7.2 g / 18 g/mol
≈ 0.4 mol
Since 1 mole of CₓHᵧ contains 2 moles of hydrogen, we can conclude that y = 0.8.
Thus, the organic compound can be represented as C₀.₄H₀.₈, which simplifies to CH₂.
Therefore, the organic compound is Methane (CH₄).