Some basic concepts of chemistry practice · Mixed difficulty

The equivalent weight of an acid is obtained by dividing its mol. wt. by its:

An amount of 5 moles of $\text{A,}$ 6 moles of $\text{B}$ and excess amount of $\mathrm{C}$ are mixed to produce a final product $\mathrm{D}$, according to the following reactions.

$\begin{aligned} & \mathrm{A}+2 \mathrm{B} \rightarrow \mathrm{I} \\ & \mathrm{I}+\mathrm{C} \rightarrow \mathrm{B}+\mathrm{D} \end{aligned}$

What is the maximum moles of $\mathrm{D},$ which can be produced assuming that the products formed can also be reused in the reactions?

If molecular weight of $\mathrm{KMn}{\mathrm{O}_4}\;\mathrm{is}\;M,$ then its equivalent weight in acidic medium would be

$0.2 \mathrm{~g}$ of an organic compound contains $\mathrm{C}, \mathrm{H}$ and $\mathrm{O}$. On combustion, it yields $0.15 \mathrm{~g}$ $\mathrm{CO}_2$ and $0.12 \mathrm{~g} \,\mathrm{H}_2 \mathrm{O}$. The percentage of $\mathrm{C}, \mathrm{H}$ and $\mathrm{O}$ respectively is

The minimum amount of ${O_2}(g)$ consumed per gram of reactant is for the reaction (Given atomic mass :
$Fe = 56,O = 16,Mg = 24,P = 31,C = 12,H = 1$)

Which of the following has greatest no. of atoms

The number of atoms in n moles of gas can be given by:

On heating $60 \mathrm{~mL}$ of a mixture of equal volumes of chlorine and its gaseous oxide and cooling to atmospheric temperature, the resulting gas measured is $75 \mathrm{~mL}.$ Treatment of this resulting gas mixture with caustic soda (absorbs chlorine) solution resulted in contraction to $15 \mathrm{~mL}.$ Assuming that all measurements were made at the same temperature and pressure, deduce the formula of oxide. (Consider that due to heating entire chlorine oxide is decomposed).

Weight of oxygen in one mole each of $\mathrm{F}{\mathrm{e}_2}{\mathrm{O}_3}\;\mathrm{and }\;\mathrm{FeO}$ is in the simple ratio of:

A quantity of $2.3 \mathrm{~g}$ of a mixture of $\mathrm{NO}_2$ and $\mathrm{N}_2 \mathrm{O}_4$ has a pressure of $0.82 \mathrm{~atm}$, at temperature $\text{T K}$ in a container of volume $\text{V}$ litres such that the ratio, $\text{T : V}$ is $300: 1$ in magnitude. What is the degree of dissociation of $\mathrm{N}_2 \mathrm{O}_4?$

0.0833 mole of carbohydrate of empirical formula $\mathrm{C}{\mathrm{H}_2}\mathrm{O}$ contain 1 g of hydrogen. The molecular formula of the carbohydrate is

The result reported in the following multiplication of significant figures, $2.5 \times 1.25=3.125$ should be

In a reaction $\mathrm{FeS}_2$ is oxidised by $\mathrm{O}_2$ to $\mathrm{Fe}_2 \mathrm{O}_3$ and $\mathrm{SO}_2$. If the equivalent of $\mathrm{O}_2 \mathrm{O}_2$ consumed is $\mathrm{y}$, then the equivalents of $\mathrm{Fe}_2 \mathrm{O}_3$ and $\mathrm{SO}_2$ with respect to $\mathrm{FeS}_2$ are

Number of atoms in 560 g of Fe ($\mathrm{atomic }\;\mathrm{mass}\;56\;\mathrm{g}\;\mathrm{mo}{\mathrm{l}^{ - 1}}$) is

The empirical formula of naphthalene is:

Carbon and oxygen forms two compound. Carbon content in one of them is $42.9 \%$ while in the other is $27.3 \%$. The give data is in support with

A molar solution represents a solution of molarity equal to:

Temperature does not affect :

The charge present on 1 mole electron is

The units $\mathrm{J}\;\mathrm{P}{\mathrm{a}^{ - 1}}$ is equivalent to

$A + 2B + 3C \to A{B_2}{C_3}$ Reaction of 6.0 g of A, $6.0 \times {10^{23}}$ atoms of B, and 0.036 mol of C yields 4.8 g of compound $A{B_2}{C_3}.$ If the atomic mass of A and C are 60 and 80 amu, respectively, the atomic mass of B is (Avogardo no. $= 6 \times {10^{23}}\,mo{l^{ - 1}})$

Assertion: Molar volume of gases changes considerably with temperature and pressure.

Reason: Molar volume of a substance is the volume occupied by 1 mole of that substance.

The pair of species having same percentage of carbon is:

The number of significant figures in $0.0045$ are

The molar ratio of ${H_2}\mathrm{ }and\mathrm{ }{O_2}$ gases in a mixture which contains these two gases in mass ratio of 1 : 4 will be

The number of atoms present in a molecule is called:

How many litre a 0.5 N solution of an oxidising agent are reduced by 2 litre of 2.0 N solution of a reducing agent?

One litre ${\mathrm{N}_2},\frac{7}{8}\mathrm{litre}\;{\mathrm{O}_2}$ and 1 litre $CO$ are taken in a mixture under indentical conditions of P and T. The amount of gases present in mixture is given by:

Empirical formula of glucose is

Which sample contains the largest number of atoms?