In the sulphur estimation, 0.20 g of a pure organic compound gave 0.40 g of barium sulphate. The percentage of sulphur in the compound is
Show Hint
Correct Answer: 27.5
Approach Solution - 1
Given that the molar mass of sulphur (S) is 32 g/mol and that of barium sulphate (BaSO\(_4\)) is 233 g/mol, the mass of sulphur in the compound can be calculated from the mass of barium sulphate produced:
The moles of barium sulphate formed: \[ \text{Moles of BaSO}_4 = \frac{0.40 \, \text{g}}{233 \, \text{g/mol}} = 0.00172 \, \text{mol} \]
The moles of sulphur in the compound are equal to the moles of BaSO\(_4\) because of the 1:1 stoichiometry of BaSO\(_4\) and sulphur.
The mass of sulphur is: \[ \text{Mass of S} = 0.00172 \, \text{mol} \times 32 \, \text{g/mol} = 0.05504 \, \text{g} \]
The percentage of sulphur in the compound is: \[ % \text{S} = \frac{0.05504 \, \text{g}}{0.20 \, \text{g}} \times 100 = 27.5% \] Thus, the correct percentage of sulphur is \(27.5\%.\)
Approach Solution -2
Mass of the organic compound = 0.20 g
Mass of barium sulphate (\( \text{BaSO}_4 \)) formed = 0.40 g
Step 2: Recall the relationship between sulphur and barium sulphate.
In the estimation of sulphur, all the sulphur in the organic compound is converted into \( \text{BaSO}_4 \).
1 mole of \( \text{BaSO}_4 \) contains 1 mole of sulphur.
Molar mass of \( \text{BaSO}_4 \):
\[ \text{Ba} = 137, \quad \text{S} = 32, \quad \text{O}_4 = 64 \] \[ \text{Total molar mass of BaSO}_4 = 233 \, \text{g mol}^{-1} \] Thus, 233 g of \( \text{BaSO}_4 \) contain 32 g of sulphur.
Step 3: Calculate the mass of sulphur in 0.40 g of \( \text{BaSO}_4 \).
\[ \text{Mass of S} = \frac{32}{233} \times 0.40 = 0.0549 \, \text{g} \]
Step 4: Calculate the percentage of sulphur in the compound.
\[ \text{Percentage of S} = \frac{0.0549}{0.20} \times 100 = 27.45 \approx 27.5\% \]
Final Answer:
\[ \boxed{27.5\%} \]
Top JEE Main Chemistry Questions
What will be the equilibrium constant of the given reaction carried out in a \(5 \,L\) vessel and having equilibrium amounts of \(A_2\) and \(A\) as \(0.5\) mole and \(2 \times 10^{-6}\) mole respectively?
The reaction : \(A_2 \rightleftharpoons 2A\)- At equilibrium the concentrations of and in a sealed vessel at . What will be for the reaction
- Find out the major products from the following reactions
Cobalt chloride when dissolved in water forms pink colored complex $X$ which has octahedral geometry. This solution on treating with cone $HCl$ forms deep blue complex, $\underline{Y}$ which has a $\underline{Z}$ geometry $X, Y$ and $Z$, respectively, are
- The correct order of atomic radii is:
Top JEE Main Stoichiometry and Stoichiometric Calculations Questions
- If 50 mL of 0.5 M oxalic acid is required to neutralise 25 mL of NaOH solution, the amount of NaOH in 50 mL of given NaOH solution is _____g.
- Consider the following reaction:\[3\text{PbCl}_2 + 2(\text{NH}_4)_3\text{PO}_4 \rightarrow \text{Pb}_3(\text{PO}_4)_2 + 6\text{NH}_4\text{Cl}\]If 72 mmol of PbCl\(_2\) is mixed with 50 mmol of (\(\text{NH}_4\))\(_3\)PO\(_4\), then the amount of \(\text{Pb}_3(\text{PO}_4)_2\) formed is ______ mmol (nearest integer).
- \( X \, \text{g} \) of ethylamine is subjected to reaction with \( \text{NaNO}_2/\text{HCl} \) followed by water; evolved dinitrogen gas which occupied \( 2.24 \, \text{L} \) volume at STP. \( X \) is ______ \( \times 10^{-1} \, \text{g} \).
- 9.3 g of pure aniline is treated with bromine water at room temperature to give a white precipitate of the product 'P'. The mass of product 'P' obtained is 26.4 g. The percentage yield is ......... %.
- Combustion of glucose (\(C_6H_{12}O_6\)) produces \(CO_2\) and water. The amount of oxygen (in g) required for the complete combustion of \(900 \, \text{g}\) of glucose is:
\([ \text{Molar mass of glucose in g mol}^{-1} = 180 ]\)
Top JEE Main Questions
- In a hydrogen like atom, when an electron jumps from the $M$ - shell to the $L$ - shell, the wavelength of emitted radiation is $\lambda$. If an electron jumps from $N$-shell to the $L$-shell, the wavelength of emitted radiation will be :
- Two masses $m$ and $\frac{m}{2}$ are connected at the two ends of a massless rigid rod of length $l$. The rod is suspended by a thin wire of torsional constant $k$ at the centre of mass of the rod-mass system(see figure). Because of torsional constant $k$, the restoring torque is $\tau =k\theta$ for angular displacement $\theta$. If the rod is rota ted by $\theta_0$ and released, the tension in it when it passes through its mean position will be:
What will be the equilibrium constant of the given reaction carried out in a \(5 \,L\) vessel and having equilibrium amounts of \(A_2\) and \(A\) as \(0.5\) mole and \(2 \times 10^{-6}\) mole respectively?
The reaction : \(A_2 \rightleftharpoons 2A\)- The value of is
- The number of terms of an is even. The sum of the odd terms is and of the even terms is . The last term exceeds the first by . Then the number of terms in the series is ______.