${\mathrm{x}}_1$ ml solution having normality ${\mathrm{y}}_1$ is diluted to get a solution Of normality ${\mathrm{y}}_2$what would be volume required for dilution?

1.  $x_1(\frac{y_1}{y_2}-1)$

2.    $x_1(1-\frac{y_1}{y_2})$

3.  $x_1(\frac{y_2}{y_1}-1)$

4.  $x_1(1+\frac{y_1}{y_2})$

What volume of ammonia gas at N TP will be required to be passed into 30 mL of 1 $\mathrm{N} {\mathrm{H}}_2{\mathrm{SO}}_4$ to bring down the acid normality to 0.2 N?

1.  480.5 mL

2.  537.6 mL

3.   438.4 mL

4.  556.5 mL

A and B are two elements that form ${\mathrm{A}}_2{\mathrm{B}}_3$and ${\mathrm{AB}}_2$. If 0.30 mole of  ${\mathrm{A}}_2{\mathrm{B}}_3$ weighs 31.8 g and 0.30 mole of  ${\mathrm{AB}}_2$ weighs 18.6 g. What are the atomic weights of A and B respectively?

1.   18, 26

2.  9, 13

3.  26, 18

4.  26, 52

A mixture of ${\mathrm{MgCl}}_2$ and ${\mathrm{MgSO}}_4$ contains 0.6 moles of chloride ions and 0.2 moles of sulphate ions. The equivalent fraction of ${\mathrm{Mg}}^{2+}$ present in the mixture is

1.   0.3

2.  $\frac{5}{13}$

3.  0.5

4.  $\frac{1}{3}$

x L of 1 M HCI is mixed With 2 L of 2 M HCI in order to prepare y L of 1.5 M HCI. The values 01 x and y are respectively

1.  6, 4

2.  2, 4

3.  3, 4

4.  4, 2

On passing 1.8 L of oxygen through ozonizer gives 1.6 L of a mixture of ozone and oxygen. What is the mole fraction of ozone in the resultant mixture?

1.   015

2.   025

3.   040

4.   050

A 10.0 g Of sample Of mixture of calcium chloride and sodium chloride is treated with ${\mathrm{Na}}_2{\mathrm{CO}}_3$ to precipitate the calcium as calcium carbonate. This ${\mathrm{CaCO}}_3$ is heated to convert all calcium to Cao and the final mass of Cao is 1.62 gms. The % by mass of CaC12 in the original mixture is

1.   15.2%

2.   32.1%

3.   21.8%

4.   11.07%

1.625 g of an interhalogen compound ${\mathrm{ICI}}_{\mathrm{x}}$ was subjected to electric discharge which split it into constituents and brought to STP It occupied 224 ml. The interhalogen compound is

1.  ICl

2.  ${\mathrm{lCl}}_3$

3.  ${\mathrm{lCl}}_5$

4.  ${\mathrm{lCl}}_7$

A 2 g sample of xenon reacts with fluorine. The mass Of compound produced is 3.158 g. The empirical formula of the compound is

1.  ${\mathrm{XeF}}_2$

2.  ${\mathrm{XeF}}_4$

3.  ${\mathrm{XeF}}_5$

4.  ${\mathrm{XeF}}_6$

Volume strength of 1 M solution of ${\mathrm{H}}_2{\mathrm{O}}_2$ is: