0.5g of an organic compound x (containing carbon hydrogen oxygen) produces 0.733g of carbondioxide and 0.3g of water on complete combustion.the max spectrum shows mr=60.determine molecular formula of x
Well, isn't this a heated situation? Let's find out what organic compound x is all about!
First, let's analyze the carbon dioxide and water produced during combustion.
From 0.733g of carbon dioxide, we can calculate the moles of carbon dioxide produced using its molar mass (which is approximately 44 g/mol). Divide the mass (0.733g) by the molar mass, and you'll find that this corresponds to approximately 0.017 moles of carbon dioxide.
Similarly, from 0.3g of water, we can calculate the moles of water produced using its molar mass (which is approximately 18 g/mol). Divide the mass (0.3g) by the molar mass, and you'll find that this corresponds to approximately 0.016 moles of water.
Since carbon dioxide is produced from only carbon in the organic compound, and water is produced solely from hydrogen in the organic compound, we can compare the moles of carbon dioxide and water to the moles of carbon and hydrogen in the organic compound, respectively.
We have 0.017 moles of carbon dioxide and 0.016 moles of water. Let's assume that the molecular formula of the organic compound x is CₘHₙOₖ.
From the 0.017 moles of carbon dioxide, we can deduce that there are also 0.017 moles of carbon in the compound.
From the 0.016 moles of water, we can deduce that there are also 0.032 moles of hydrogen in the compound (since water has a formula of H₂O).
From here, we subtract the moles of carbon and hydrogen from the total moles of compound x to find the moles of oxygen. Since the total moles of compound x is equal to 0.5g divided by its molar mass (60 g/mol), we can calculate it as approximately 0.0083 moles.
Subtracting 0.017 moles of carbon and 0.032 moles of hydrogen from this gives us the value of approximately 0.008 moles of oxygen.
Now, we need to find the simplest whole number ratio for the atoms in the compound. To do this, divide the number of moles of each element by the smallest value, which is approximately 0.008 moles of oxygen.
After dividing, we find that the ratio is:
C: 0.017 / 0.008 ≈ 2
H: 0.032 / 0.008 = 4
O: 0.008 / 0.008 = 1
So, the empirical formula of compound x is C2H4O.
Since the empirical formula mass is 12.01 + (4.03 × 4) + 16.00 = 60.12 g/mol, which is close to the given maximum spectrum of 60 g/mol, it suggests that the empirical formula is the same as the molecular formula.
Therefore, the molecular formula of organic compound x is C2H4O.
Hope this analysis didn't leave you fuming!
To determine the molecular formula of compound X, we need to follow a series of steps:
Step 1: Calculate the moles of carbon dioxide (CO2) produced.
- The molar mass of CO2 is 44 g/mol.
- The mass of CO2 produced is 0.733 g.
- Use the formula: moles = mass / molar mass.
- Therefore, moles of CO2 = 0.733 g / 44 g/mol = 0.01666 mol.
Step 2: Calculate the moles of water (H2O) produced.
- The molar mass of H2O is 18 g/mol.
- The mass of H2O produced is 0.3 g.
- Use the formula: moles = mass / molar mass.
- Therefore, moles of H2O = 0.3 g / 18 g/mol = 0.01667 mol.
Step 3: Calculate the moles of carbon in compound X.
- Each CO2 molecule contains 1 carbon atom.
- The moles of carbon present in CO2 would be the same as the moles of CO2 produced.
- Therefore, moles of carbon = 0.01666 mol.
Step 4: Calculate the moles of hydrogen in compound X.
- Each H2O molecule contains 2 hydrogen atoms.
- The moles of hydrogen present in H2O would be twice the moles of H2O produced.
- Therefore, moles of hydrogen = 2 * 0.01667 mol = 0.03334 mol.
Step 5: Calculate the moles of oxygen in compound X.
- The moles of oxygen can be determined by subtracting the sum of moles of carbon and hydrogen from the total moles of the compound (0.01666 + 0.03334).
- Moles of oxygen = 0.01667 mol - (0.01666 mol + 0.03334 mol) = 0.01667 mol - 0.05 mol = -0.03333 mol (This result is negative).
Step 6: Determine the empirical formula of compound X.
- The empirical formula gives the simplest whole-number ratio of the atoms present in a compound.
- To determine the empirical formula, we need to find the ratio of moles of each element.
- Divide the moles of each element by the smallest calculated value.
- Here, the smallest moles value is 0.01666 (moles of carbon).
- Moles of carbon = 0.01666 mol / 0.01666 mol = 1 (approximately).
- Moles of hydrogen = 0.03334 mol / 0.01666 mol ≈ 2 (approximately).
- Moles of oxygen = -0.03333 mol /0.01666 mol ≈ -2 (approximately).
- Note: We multiply by 2 to get a whole number for the ratio.
The empirical formula of compound X is CH2O.
Step 7: Determine the molecular formula of compound X.
- The empirical formula tells us the simplest ratio of atoms present in the compound.
- To determine the molecular formula, we need to find the actual number of atoms present.
- The molecular mass (molar mass) was given as 60 g/mol.
- Calculate the empirical formula mass by summing the atomic masses of carbon (12 g/mol), hydrogen (1 g/mol), and oxygen (16 g/mol).
- Empirical formula mass = 12 g/mol + 2 g/mol + 16 g/mol = 30 g/mol.
- Calculate the "multiplier" by dividing the molecular mass by the empirical formula mass.
- Multiplier = 60 g/mol / 30 g/mol = 2.
The molecular formula of compound X is (CH2O)2, which can be simplified as C2H4O2.