Some basic concepts of chemistry practice · Mixed difficulty

Statement I: Combustion of $16 \mathrm{~g} {\text { of }} \mathrm{CH}_4$ gives $18 \mathrm{~g}$ of $\mathrm{H}_2 \mathrm{O}$.

Statement II: In the combustion of $\mathrm{CH}_4, \mathrm{H}_2 \mathrm{O}$ is one of the products.

Dulong and Petit’s law is valid only for

In the following change, $3\mathrm{Fe} + 4{\mathrm{H}_2}\mathrm{O} \to \mathrm{F}{\mathrm{e}_3}{\mathrm{O}_4} + 4{\mathrm{H}_2}$. If the atomic weight of iron is 56, then its equivalent weight will be :

Number of $\mathrm{Zn}$ atoms present in $122 \mathrm{~g}$ of $\mathrm{ZnO}$ is (Atomic wt. of $\mathrm{Zn}=65$)

Statement I: $\mathrm{SO}_2$ formed by the oxidation of sulphur or hydrogen sulphide contains sulphur and oxygen in $1: 2$ mass ratio.

Statement II: Different samples of a pure chemical substance always contain the same proportions of elements by mass.

2.4 kg of carbon is made to react with 1.35 kg of aluminium to form $Al_4C_3.$ The maximum amount (in kg) of aluminium carbide formed is

20.0 kg of $H_2(g)$ and 32 kg of $O_2(g)$ are reacted to produce $H_2O(l).$ The amount of $H_2O(l)$ formed after completion of reaction is

The amount of ${BaSO}_4$ formed upon mixing $100 {~mL}$ of $20.8 \% \,{BaCl}_2$ solution with $50 {~mL}$ of $9.8 \% {H}_2 {SO}_4$ solution with $50 {~mL}$ of $9.8 \%\,$ ${H}_2 {SO}_4$ solution will be:

$({Ba}=137, {Cl}=35.5, {~S}=32, {H}=1 \text { and } {O}=16 \text { ) }$

Statement I: When $10 \mathrm{~g}$ of $\mathrm{CaCO}_3$ is decomposed $5.6 \mathrm{~g}$ of $\mathrm{CaO}$ and $4.4 \mathrm{~g}$ of $\mathrm{CO}_2$ are formed.

Statement II: Law of conservation of mass is followed.

The number of moles of $\mathrm{CaCl}_2$ needed to react with excess of $\mathrm{AgNO}_3$ to produce $4.31 \mathrm{gm}$ of $\mathrm{AgCl}$

The volume of air needed for complete combustion of 1 kg carbon at STP is:

Assertion:- $44 \mathrm{~g}$ of $\mathrm{CO}_2, 28 \mathrm{~g}$ of $\mathrm{CO}$ have same volume at STP.

Reason:- Both $\mathrm{CO}_2$ and $\mathrm{CO}$ are formed by $\mathrm{C}$ and oxygen.

One mole of molecules of dioxygen represents

Which property of an element is not variable?

6.90 grams of metal carbonate was completely decomposed by 50 ml of 2N HCl. The equivalent weight of metal is

Choose the correct option based on following statements. Here ‘T’ stands for true and ‘F’ stands for false statement.
(i) Molecular mass of cane sugar $(C_{12}H_{22}O_{11})$ is 182 amu.
(ii) 1 mole of cane sugar contains $6.022 \times 10^{23}$ molecules of cane sugar.
(iii) 34.20 g of cane sugar contains $6.022 \times 10^{21}$ molecules of cane sugar.

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

Complete combustion of $0.858 \mathrm{~g}$ of compound $X$ gives $2.64 \mathrm{~g}$ of $\mathrm{CO}_2$ and $1.26 \mathrm{~g}_{\text {of }} \mathrm{H}_2 \mathrm{O}$. The lowest molecular mass $X$ can have :

The following sequence of reaction occurs in commercial production of aqueous nitric acid.

$\begin{array}{cc} 4 \mathrm{NH}_3(\mathrm{~g})+5 \mathrm{O}_2(\mathrm{~g}) \longrightarrow 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_2 \mathrm{O}(\mathrm{l}) & \Delta \mathrm{H}=-904 \mathrm{~kJ}.........(i) \\ 2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{NO}_2(\mathrm{~g}) & \Delta \mathrm{H}=-112 \mathrm{~kJ}.........(ii) \\ 3 \mathrm{NO}_2(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\mathrm{l}) \longrightarrow 2 \mathrm{HNO}_3(\mathrm{aq})+\mathrm{NO}(\mathrm{g}) & \Delta \mathrm{H}=-140 \mathrm{~kJ}.........(iii) \end{array}$

Determine the total heat (in $\mathrm{kJ} / \mathrm{mole}$ ) liberated at constant pressure for the production of exactly 1 mole of aqueous nitric acid by this process.

The mass of 11.2 L of ammonia gas at STP is

The mole fraction of solute in one molal aqueous solution is:

40 milligram diatomic volatile substance $\left(X_2\right)$ is converted to vapour that displaced $4.92 \mathrm{~mL}$ of air at $1 \mathrm{~atm}$ and $300 \mathrm{~K}$. Atomic weight of element $X$ is nearly:

Max. no. of gram molecules are present in:

$45.4 \mathrm{~L}$ of dinitrogen reacted with $22.7 \mathrm{~L}$ of dioxygen and $45.4 \mathrm{~L}$ of nitrous oxide was formed. The reaction is given below.
$2 \mathrm{~N}_2(\mathrm{g})+\mathrm{O}_2(\mathrm{g}) \longrightarrow 2 \mathrm{~N}_2 \mathrm{O}(\mathrm{g})$
Which law is being obeyed in this experiment?

10 g of hydrogen and 64 of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be:

Assertion: 1 equivalent of $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ has 1 equivalent of $\mathrm{K}, \mathrm{Cr}$ and $\mathrm{O}$ each.
Reason: Equivalent and milliequivalent reacts in equal number to give same equivalent of product.

Maximum number of atoms are present in

A $4 \mathrm{~g}$ mixture of $\mathrm{Na}_2 \mathrm{O}$ and $\mathrm{NaCl}$ was dissolved in $400 \mathrm{~mL}$ of $0.3 \mathrm{~M} \mathrm{~HCl}$. After complete reaction, the resulting solution required $200 \mathrm{~mL}$ of $0.2 \mathrm{~M} \mathrm{~NaOH}$ for complete neutralization of the excess $\mathrm{HCl}$. What mass $\%$ of $\mathrm{Na}_2 \mathrm{O}$ is present in the mixture?

2 g of metal carbonate is neutralised completely by 100mL of 0.1 (N) HCl. The equivalent weight of metal carbonate is

Out of $1.0 \mathrm{~g}$ dioxygen, $1.0 \mathrm{~g}$ atomic oxygen and $1.0 \mathrm{~g}$ ozone, the maximum number of oxygen atoms are contained in