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Molality of \( 0.8 \, \text{M} \, \mathrm{H_2SO_4} \) solution (density \( 1.06 \, \text{g cm}^{-3} \)) is ______ \( \times 10^{-3} \, \text{m} \).

\( 10 \, \text{mL} \) of gaseous hydrocarbon on combustion gives \( 40 \, \text{mL} \) of \( \text{CO}_2 (g) \) and \( 50 \, \text{mL} \) of water vapour. Total number of carbon and hydrogen atoms in the hydrocarbon is __________.

Given below are two statements:
Statement I: \( \mathrm{S}_8 \) solid undergoes disproportionation reaction under alkaline conditions to form \( \mathrm{S}^{2-} \) and \( \mathrm{S}_2\mathrm{O}_3^{2-} \).
Statement II: \( \mathrm{ClO}_4^{-} \) can undergo disproportionation reaction under acidic condition.
In the light of the above statements, choose the most appropriate answer from the options given below:

A solution of \( \mathrm{H_2SO_4} \) is \( 31.4\% \) \( \mathrm{H_2SO_4} \) by mass and has a density of \( 1.25 \, \mathrm{g/mL} \).
The molarity of the \( \mathrm{H_2SO_4} \) solution is __________ \( \mathrm{M} \) (nearest integer)
[Given molar mass of \( \mathrm{H_2SO_4} = 98 \, \mathrm{g \, mol^{-1}} \) ]

The number of moles of methane required to produce \( 11 \, \text{g} \) \( \mathrm{CO_2(g)} \) after complete combustion is:
(Given molar mass of methane in \( \mathrm{g \, mol^{-1}} : 16 \))

The mass of sodium acetate \( \mathrm{(CH_3COONa)} \) required to prepare \( 250 \, \text{mL} \) of \( 0.35 \, \text{M} \) aqueous solution is _______ \( \text{g} \). (Molar mass of \( \mathrm{CH_3COONa} \) is \( 82.02 \, \text{g} \, \text{mol}^{-1} \) )

A sample of \( \mathrm{CaCO_3} \) and \( \mathrm{MgCO_3} \) weighed \( 2.21 \, \text{g} \) is ignited to constant weight of \( 1.152 \, \text{g} \). The composition of mixture is:
(Given molar mass in \( \text{g mol}^{-1} \) \( \mathrm{CaCO_3} : 100, \; \mathrm{MgCO_3} : 84 \))

Mass of methane required to produce \( 22 \, \text{g} \) of \( \mathrm{CO_2} \) after complete combustion is ________ \( \text{g} \). (Given Molar mass in \( \text{g mol}^{-1} \), \( \mathrm{C} = 12.0 \), \( \mathrm{H} = 1.0 \), \( \mathrm{O} = 16.0 \))

An organic compound has \( 42.1\% \) carbon, \( 6.4\% \) hydrogen and remainder is oxygen. If its molecular weight is \( 342 \), then its molecular formula is:

Molality \( (m) \) of \( 3 \, \mathrm{M} \) aqueous solution of \( \mathrm{NaCl} \) is:
(Given: Density of solution \( = 1.25 \, \mathrm{g \, mL^{-1}} \), Molar mass in \( \mathrm{g \, mol^{-1}} \): \( \mathrm{Na\!-\!23, \, Cl\!-\!35.5} \))

The incorrect postulates of the Dalton’s atomic theory are:
(A) Atoms of different elements differ in mass
(B) Matter consists of divisible atoms
(C) Compounds are formed when atoms of different element combine in a fixed ratio
(D) All the atoms of given element have different properties including mass
(E) Chemical reaction involve reorganisation of atoms
Choose the correct answer from the options given below:

Volume of \( 3 \, \text{M} \) NaOH (formula weight \( 40 \, \text{g mol}^{-1} \)) which can be prepared from \( 84 \, \text{g} \) of NaOH is __________ × \( 10^{-1} \, \text{dm}^3 \).

If a substance ‘A’ dissolves in solution of a mixture of ‘B’ and ‘C’ with their respective number of moles as \( n_A \), \( n_B \) and \( n_C \), Mole fraction of C in the solution is:

The Molarity \( (M) \) of an aqueous solution containing \( 5.85 \, \mathrm{g} \) of \( \mathrm{NaCl} \) in \( 500 \, \mathrm{mL} \) water is:
(Given: Molar Mass Na : \( 23 \) and Cl : \( 35.5 \, \mathrm{g \, mol^{-1}} \) )

Molality of an aqueous solution of urea is \( 4.44 \, \text{m} \). Mole fraction of urea in solution is \( x \times 10^{-3} \). Value of \( x \) is _____________. (Integer answer)

Combustion of glucose \( (\mathrm{C_6H_{12}O_6}) \) produces \( \mathrm{CO_2} \) and water. The amount of oxygen (in \( \mathrm{g} \)) required for the complete combustion of \( 900 \) \( \mathrm{g} \) of glucose is: [Molar mass of glucose in \( \mathrm{g\,mol^{-1}} \) = \( 180 \)]

Consider the following reaction:
\( 3\mathrm{PbCl_2} + 2(\mathrm{NH_4})_3\mathrm{PO_4} \rightarrow \mathrm{Pb_3(PO_4)_2} + 6\mathrm{NH_4Cl} \)
If \( 72 \) mmol of \( \mathrm{PbCl_2} \) is mixed with \( 50 \) mmol of \( (\mathrm{NH_4})_3\mathrm{PO_4} \), then the amount of \( \mathrm{Pb_3(PO_4)_2} \) formed is ______ mmol. (Nearest integer)