List of top Chemistry Questions on Quantitative Analysis

Consider the reaction} \[ 2\text{H}_2\text{S (g)} + 3\text{O}_2\text{(g)} \rightarrow 2\text{H}_2\text{O (l)} + 2\text{SO}_2\text{(g)} \] The magnitude of enthalpy change for the reaction in kJ mol\(^{-1}\) is _______ (Nearest integer).

In a closed flask at 600 K, one mole of \(X_2Y_4(g)\) attains equilibrium as given below :} \[ X_2Y_4(g) \rightleftharpoons 2XY_2(g) \] At equilibrium, 75% \(X_2Y_4(g)\) was dissociated and the total pressure is 1 atm. The magnitude of \(\Delta G^\circ\) (in kJ mol\(^{-1}\)) at this temperature is _____. (Nearest Integer)}

In an estimation of sulphur by Carius method \(0.2 \text{ g}\) of the substance gave \(0.6 \text{ g}\) of \(BaSO_4\). The percentage of sulphur in the substance is ____ %.
(Given molar mass in \(\text{g mol}^{-1}\) S : 32, \(BaSO_4 : 231\))}

For the following reaction at 50 \(^\circ\)C and at 2 atm pressure,
\(2N_2O_5(g) \rightleftharpoons 2N_2O_4(g) + O_2(g)\)
\(N_2O_5\) is 50% dissociated. The magnitude of standard free energy change at this temperature is x.
x = _______ J \(\cdot mol^{-1}\) [Nearest integer].
Given : R = 8.314 J \(mol^{-1} K^{-1}\), \(\log 2 = 0.30, \log 3 = 0.48, \ln 10 = 2.303, ^\circ C + 273 = K\)

An electrochemical cell, consist of the following two redox couples, \(M^{x+}(aq)/M(s) [E_{red}^\circ = +0.15 V]\) and \(Fe^{3+}(aq)/Fe(s) [E_{red}^\circ = -0.036 V]\). The cell EMF (\(E_{cell}\)) is recorded to be 0.2057 V. If the reaction quotient of the electrochemical cell is found to be \(10^{-z}\), then the value of x is _________. (Nearest integer)
[Given : M is a p-block metal and \(\frac{2.303 RT}{F} = 0.059 V\)]

2.0 g of a bromo hydrocarbon (X) was subjected to Carius analysis, gave 3.36 g of AgBr. The percentage of carbon in the compound (X) is 26.7%. Total number of carbon atoms in the empirical formula for compound (X) is ______.

Consider the following sequence of reactions to give the major product (X). P g of the major product (X) formed is reacted with NaHCO₃ solution to liberate a gas which occupied 11.2 dm³ at STP. P = ______ g.

1 gm of organic compound gave 1.32g $\text{CO}_2$, 0.53g of same compound gave 0.75g AgBr. If molecular formula of compound is $\text{C}_x\text{H}_y\text{Br}_z$ then calculate percentage of hydrogen in the given compound.

When $1$ g of compound $(X)$ is subjected to Kjeldahl's method for estimation of nitrogen, $15$ mL of $1$ M $\mathrm{H_2SO_4}$ was neutralized by ammonia evolved. The percentage of nitrogen in compound $(X)$ is:

Sodium extract of organic compound of 0.1 g is treated with chlorine water and \( \text{CCl}_4 \) which dissolves in organic solvent to produce a violet colour. Upon treatment with \( \text{AgNO}_3 \), a yellow ppt. of 0.12 g is produced. Calculate the percentage of halide in the organic compound.

In Carius method of estimation of ‘Br’, 1.53 g of an organic compound gave 1 g AgBr. The % of Br in the organic compound is: (Atomic mass of Ag, Br = 108, 80 u respectively)

1 g of an organic compound produces 1.49 g of \( \text{Mg}_2\text{P}_2\text{O}_7 \). Determine the percentage of phosphorus (P).

Given below are two statements :
Statement (I) : Kjeldahl method is applicable to estimate nitrogen in pyridine.
Statement (II) : The nitrogen present in pyridine can easily be converted into ammonium sulphate in Kjeldahl method.
In the light of the above statements, choose the correct answer from the options given below.

Match List-I with List-II.

List-I (Name of the test)	List-II (Reaction sequence involved) [M is metal]
(A) Borax bead test	I
(B) Charcoal cavity test	II
(C) Cobalt nitrate test	III
(D) Flame test	IV

Choose the correct answer from the options given below:

In Kjeldahl’s method for estimation of nitrogen, CuSO\(_4\) acts as:

When 0.01 mol of an organic compound containing 60% carbon was burnt completely, 4.4 g of $CO_2$ was produced. The molar mass of compound is _______ $gmol^{−1}$. (Nearest integer).

0.25 g of an organic compound containing chlorine gave 0.40 g of silver chloride in Carius estimation. The percentage of chlorine present in the compound is ______. [in nearest integer]
(Given : Molar mass of \(Ag\) is 108 g mol^–1 and that of \(Cl\) is 35.5 g mol^–1