Some basic concepts of chemistry practice · Mixed difficulty

Assertion: Equivalent weight of $\mathrm{NH}_3$ in the reaction $\mathrm{N}_2 \rightarrow \mathrm{NH}_3$ is $17 / 3$ while that of $\mathrm{N}_2$ is $28/6.$

Reason: Equivalent weight = $\frac{\text {Molecular weight}}{\text {number of } e^- \text{ lost or gained }}$.

The weight of lime obtained by heating $200 \mathrm{~kg}$ of $95 \%$ pure lime stone is:

The sulphate of an element contains $42.2 \%$ element. The equivalent weight of the metal would be

The law of definite proportions is not applicable to nitrogen oxide because

At NTP, $5.6\,\,\mathrm{litre}$ of a gas weighs $8\mathrm{g}$. The vapour density of the gas is

One litre of ${\mathrm{C}{\mathrm{O}_2}}$ is passed over hot coke. The volume becomes 1.4 litre. The per cent composition of products is:

An aqueous solution of oxalic acid dihydrate contains its $6.3 \mathrm{~g}$ in $250 \mathrm{~mL}$. The volume of $0.1 \mathrm{~N} \mathrm{~NaOH}$ required to completely neutralize $10 \mathrm{~mL}$ of this solution

Arsenic forms two oxides, one of which contains 65.2% and the other 75.5% of the element. Hence, equivalent masses of arsenic are in the ratio

20.0 g of a magnesium carbonate sample decomposes on heating to give carbon dioxide and 8.0 g magnesium oxide. What will be the percentage purity of magnesium carbonate in the sample?
(Atomic weight: $Mg = 24$)

Dissolving 120 g of urea (mol.wt.60) in 1000 g of water gave a solution of density 1.15 g/mL. The molarity of the solution is:

S.I. unit of molarity will be?

Mass of ${10^{21}}$ molecules of Cu (at. Wt = 63.5)

Two elements $X$ and $Y$ have atomic weights of 14 and 16. They form a serics of compounds $A, B, C, D$ and $E$ in which the same amount of element ${X},{Y}$ is present in the ratio $1: 2: 3: 4: 5.$ If the compound $A$ has 28 parts by weight of $X$ and 16 parts by weight of ${Y},$ then the compound of ${C}$ will have 28 parts weight of ${X}$ and

Mole fraction of solute in aqueous solution of $30 \% \,{NaOH}$.

A compound has molar mass of $147 \mathrm{~g}$. It contains $49 \%\mathrm{C}$ and $2.72 \% \mathrm{H}$. On Carius estimation $2.561 \mathrm{~mg}$ of the compound gave $5 \mathrm{~mg}$ of $\mathrm{AgCl}$. Find the empirical and molecular formula.

The number of $\mathrm{F}{\mathrm{e}^{2 + }}$ ion oxidised by one mole of $\mathrm{MnO}_4^ -$ ions is :

An organic compound has an empirical formula $\mathrm{(C}{\mathrm{H}_2}\mathrm{O)}$ its vapour density is 45. The molecular formula of the compound is

$12 \mathrm{gm}$ of $\mathrm{Mg}$ (At mass $=24$ ) will react with an acid to give

$0.40 \mathrm{~g}$ of helium in a bulb at a temperature of $T \mathrm{~K}$ had a pressure of $p$ atm. When the bulb was immersed in water bath at temperature $50 \mathrm{~K}$ more than the first one, $0.08 \mathrm{~g}$ of gas had to be removed to restore the original pressure. $T$ is

Calculate the molality of 1 litre solution of $93 \% \, \mathrm{H}_2 \mathrm{SO}_4$ (weight/volume). The density of the solution is $1.84 \mathrm{~g} / \mathrm{mL}$.

Iron forms two oxides. If for the same mass of iron, the mass of oxygen combined in the first oxide is two-third of the mass of oxygen combined in the second oxide, then the ratio of valency of iron in first and second oxide is

$10^{21}$ molecules areramoved from $200 {mg}$ of ${CO}_2$. The moles of ${CO}_2$ left are :

In the reaction

$\mathrm{Br}_2+\mathrm{Na}_2 \mathrm{CO}_3 \rightarrow \mathrm{NaBr}+\mathrm{NaBrO}_3+\mathrm{CO}_2$

The equivalent weight of $\mathrm{NaBrO}_3$ is

For $\mathrm{CuSO}_4 \cdot 5 \mathrm{H}_2 \mathrm{O},$ which is the correct mole relationship?

The total number of electrons in 18 ml of water (density = 1/gml

How many moles of $\mathrm{A}{\mathrm{l}_2}{\left( {\mathrm{S}{\mathrm{O}_4}} \right)_3}$ would be in 50 g of the substance?

One litre of a gas at STP weight $1.16 \, g$ it can possible be

Which is correct for $\mathrm{N}{\mathrm{a}_2}\mathrm{HP}{\mathrm{O}_3}$?

At 300 K and 1 atm, 15 mL of a gaseous hydrocarbon requires 375 mL air containing 20% ${O_2}$ by volume for complete combustion. After combustion, the gases occupy 330 mL. Assuming that the water formed is in liquid form and the volumes were measured at the same temperature and pressure, the formula of the hydrocarbon is

For the reaction,

$\mathrm{FeS}_2+\mathrm{KMnO}_4+\mathrm{H}^* \longrightarrow \mathrm{Fe}^{3+}+\mathrm{H}_2 \mathrm{SO}_4+\mathrm{Mn}^{2+}+\mathrm{H}_2 \mathrm{O}$

if the molar mass of $\mathrm{FeS}_2$ is $\mathrm{M}$, then equivalent mass of $\mathrm{FeS}_2$ would be equal to