iCON Education - Some Basic Concepts of Chemistry AP-EAPCET Test

The mass of a mixture containing NaCl and NaBr is 4.0 g . If Na is $30 \%$ of the total mixture, the composition of NaCl in the mixture is $(\mathrm{Na}=23 \mathrm{u}, \mathrm{Cl}=35.5 \mathrm{u}, \mathrm{Br}=80 \mathrm{u})$

Two acids $A$ and $B$ are titrated separately, 25 mL of $0.5 \mathrm{M} \mathrm{Na}_2 \mathrm{CO}_3$ solution requires 10 mL of $A$ and 40 mL of $B$ for complete neutralisation. The volume (in L ) of $A$ and $B$ required to produce 1 L of 1 N acid solution respectively are

An ideal gas mixture of $\mathrm{C}_2 \mathrm{H}_6$ and $\mathrm{C}_2 \mathrm{H}_4$ occupies a volume of 28 L at 1 atm and 273 K . This mixture reacts completely with 128 g of $\mathrm{O}_2$ to produce $\mathrm{CO}_2$ and $\mathrm{H}_2 \mathrm{O}(l)$. What is the mole fraction of $\mathrm{C}_2 \mathrm{H}_4$ in the mixture ?

Complete combustion of ethane gives only gaseous products. In a closed vessel, 15 g of ethane and 112 g of $\mathrm{O}_2$ were allowed to completely react. What is the total number of moles of gaseous substances present in the vessel at the end of the reaction?

The composition of a sample of wustite is $\mathrm{Fe}_{0.93} \mathrm{O}_{1.00}$. Percentage of iron in the form of $\mathrm{Fe}^{3+}$ ion is nearly

Consider the following

(A) 0.0025

(B) 500.0

Number of significant figures in $A, B$ and $C$ respectively, are

1.84 g of a mixture of $\mathrm{CaCO}_3$ and $\mathrm{MgCO}_3$ is strongly heated to get a residue of 0.96 g . The percentage of $\mathrm{CaCO}_3$ in the mixture is

209 g of an element reacts with chlorine to form 315.5 g of its chloride. What is the weight (in g ) of oxygen that reacts with 418 g of same element ?

$ (\mathrm{Cl}=35.5 \mathrm{u} ; \mathrm{O}=16 \mathrm{u}) $

Observe the following

I. 0.0063

II. 132.00

III. 1004

The number of significant figures in I, II and III is respectively.

Identify the correct statements from the following.

I. Reaction of hydrogen with fluorine occurs even in dark.

II. Manufacture of ammonia by Haber process is an endothermic reaction.

III. HF is electron rich hydride.

10 g of a metal $(M)$ reacts with oxygen to form 11.6 got oxide. What is the equivalent weight of $M$ ?

A flask contains 98 mg of $\mathrm{H}_2 \mathrm{SO}_4$. If $3.01 \times 10^{20}$ molecules of $\mathrm{H}_2 \mathrm{SO}_4$ are removed from the flask. The number of moles of $\mathrm{H}_2 \mathrm{SO}_4$ remained in flask is

$ \left(N_A=6.02 \times 10^{23}\right) $

$1.66 \times 10^{-3}$

$9.95 \times 10^{-3}$

0.1 mole of potassium permanganate was heated at $300^{\circ} \mathrm{C}$. What is weight (ing) of the residue? $ (\mathrm{Mn}=55 \mathrm{u}, \mathrm{~K}=39 \mathrm{u}, \mathrm{O}=16 \mathrm{u}) $

100 mL of $\frac{M}{10} \mathrm{Ca}\left(\mathrm{NO}_3\right)_2$ and 200 mL of $\frac{M}{10} \mathrm{KNO}_3$ solutions are mixed. What is the normality of resulted solution with respect to $\mathrm{NO}_3^{-}$?

At STP ' $x$ ' $g$ of a metal hydrogen carbonate $\left(M \mathrm{HCO}_3\right)$ (molar mass $84 \mathrm{~g} \mathrm{~mol}^{-1}$ ) on heating gives $\mathrm{CO}_2$, which can completely react with 0.2 moles of MOH (molar mass $40 \mathrm{~g} \mathrm{~mol}^{-1}$ ) to give $\mathrm{MHCO}_3$. The value of ' $x^{\prime}$ is

The mass % of urea solution is 6 . The total weight of the solution is 1000 g . What is its concentration in $\mathrm{mol} \mathrm{L}^{-1}$ ? (Density of water $=1.0 \mathrm{~g} \mathrm{~mL}^{-1}$ )

( $\mathrm{C}=12 \mathrm{u}, \mathrm{N}=14 \mathrm{u}, \mathrm{O}=16 \mathrm{u}, \mathrm{H}=1 \mathrm{u}$ )

$\mathrm{Xe}(g)+2 \mathrm{~F}_2(g) \xrightarrow[7 \text { bar }]{873 \mathrm{~K}} \mathrm{XeF}_4(\mathrm{~s})$

The ratio of $\mathrm{Xe}: \mathrm{F}_2$ required in the above reaction is

The density of nitric acid solution is $1.5 \mathrm{~g} \mathrm{~mL}^{-1}$. Its weight percentage is 68 . What is the approximate concentration (in $\mathrm{mol} \mathrm{L}^{-1}$ ) of nitric acid ?

$ (\mathrm{N}=14 \mathrm{u} ; \mathrm{O}=16 \mathrm{u} ; \mathrm{H}=1 \mathrm{u}) $

A hydrocarbon containing C and H has $92.3 \% \mathrm{C}$ When 39 g of hydrocarbon was completely burnt in 0 $X$ moles of water and $Y$ moles of $\mathrm{CO}_2$ were formed $\mathrm{H}_2$ with Na metal, What is the weight (in g) of ounp ${ }^{\circ}$ consumed $)(\mathrm{C}=12 \mathrm{u}: \mathrm{H}=1 \mathrm{f})$

The concentration of 1 L of $\mathrm{CaCO}_3$ solution is 1000 ppm . What is its concentration in mol $\mathrm{L}^{-1}$ ?

$ (\mathrm{Ca}=40 \mathrm{u}, \mathrm{O}=16 \mathrm{u}, \mathrm{C}=12 \mathrm{u}) $

50 g of a substance is dissolved in 1 kg of water at $+90^{\circ} \mathrm{C}$. The temperature is reduced to $+10^{\circ} \mathrm{C}$. The density is increased from 1.1 to $1.15 \mathrm{~g} \mathrm{~cc}^{-1}$. What is the % change of molarity of the solution?

The empirical formula of calgon is

$\mathrm{Na}_2 \mathrm{PO}_3$

$\mathrm{NaP}_2 \mathrm{O}_3$

$\mathrm{Na}_3 \mathrm{PO}_3$

The statement related to law of definite proportions is

the ratio of oxygen in $\mathrm{H}_2 \mathrm{O}$ and $\mathrm{H}_2 \mathrm{O}_2$ with respect to fixed mass of hydrogen atom is a whole number.

% of oxygen in $\mathrm{H}_2 \mathrm{O}$ is constant irrespective of the source.

equal volume of all gases at the same temperature and pressure should contain equal number of molecules.

matter can neither be created nor destroyed.

What are $x$ and $y$ in the following reaction?

$x \mathrm{~Pb}_3 \mathrm{O}_4 \longrightarrow y \mathrm{PbO}+\mathrm{O}_2$

If the volume of $15.9 \mathrm{~g}$ of carbon tetrachloride is $10 \mathrm{~mL}$, calculate its density.

$31.8 \mathrm{~g} \mathrm{~mL}^{-1}$

$1.59 \mathrm{~g} \mathrm{~mL}^{-1}$

$0.159 \mathrm{~g} \mathrm{~mL}^{-1}$

$15.9 \mathrm{~g} \mathrm{~mL}^{-1}$

$0.63 \mathrm{~g}$ of oxalic acid is dissolved in order to obtain $250 \mathrm{~cm}^3$ of its solution. Find the normality of this solution. [oxalic acid $\left.(\mathrm{COOH})_2 \cdot 2 \mathrm{H}_2 \mathrm{O}\right]$

$7.8 \mathrm{~g}$ of a compound having molecular formula $\mathrm{C}_6 \mathrm{H}_6$, on reacting with $\mathrm{CH}_3 \mathrm{COCl} / \mathrm{AlCl}_3$ gives $8.4 \mathrm{~g}$ of a product which has molecular formula $\mathrm{C}_8 \mathrm{H}_8 \mathrm{O}$. Calculate the percentage yield of the product $\mathrm{C}_8 \mathrm{H}_8 \mathrm{O}$. (Given, atomic weights of $\mathrm{H}, \mathrm{C}$ and $\mathrm{O}$ respectively are 1, 12 and 16)

The complete combustion of one mole of benzene produces .......... grams of carbon dioxide.

An alloy of metals X and Y weighs 12 g and contains atoms X and Y in the ratio of 2 : 5. The percentage of metal X in the alloy is 20 by mass. If the atomic mass of X is 40 amu what is the atomic mass of metal Y ?

If 0.2 moles of sulphuric acid is poured into 250 mL of water, calculate the concentration of the solution.

When 20 g of CaCO$_3$ is treated with 20 g of HCl, the mass of CO$_2$ formed would be