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Which has maximum number of atoms at NTP?
1. 1 ml ${\mathrm{CH}}_4$
2. 1 ml ${\mathrm{N}}_2$
3. 1 ml ${\mathrm{H}}_2$
4. 1 ml ${\mathrm{H}}_2\mathrm{O}$

1 gm butane $\left({\mathrm{C}}_4{\mathrm{H}}_{10}\right)$ is burnt with excess of ${\mathrm{O}}_2$ to form ${\mathrm{CO}}_2$. The approximate mass of ${\mathrm{CO}}_2$ produced is
1. 1gm
2. 2gm
3. 3gm
4. 4gm

2 gm Iron pyrite $\left(Fe{S}_2\right)$ is burnt with $O_2$to form ${\mathrm{Fe}}_2{\mathrm{O}}_{3 }\mathrm{and} {\mathrm{SO}}_2$. THe mass of $S{O}_2$produced is
(Fe = 56, S = 32, O = 16)
1.  2 gm
2.  2.13 gm
3.  4 gm
4.  4.26 gm 

800 ml of a mixture of ${\mathrm{O}}_2 \mathrm{and} {\mathrm{O}}_3$ weighs 1.2 gm at NTP. The volume of ${\mathrm{O}}_3$ in the mixture will be
1. 80 ml
2. 160 ml
3. 200 ml
4. 400 ml

9.8 gm ${\mathrm{KCIO}}_3$ is decomposed and the weight loss was found to be 0.384 gm. The percentage of ${\mathrm{KCIO}}_3$ decomposed is:
1. 10%
2. 20%
3. 40%
4. 100%

The molarity of ${\mathrm{NaNO}}_3$ solution is 1 M. The density of solution is 1.25 gm/ml. The molality of the solution will be
1. 1 M
2. 0.86 M
3. 1.25 M
4. 0.625 M

After 50 g of the solute precipitated from a 400 g solution containing 20% solute, what is the new concentration (in percentage) of the remaining solution?
1. 7.5%
2. 8.57%
3. 10%
4. 12%

10 g of a mixture of $C{u}_{2}S$ and CuS is reacted with 150 ml 1M $KMn{O}_4$ producing ${\mathrm{Cu}}^{2+}, {\mathrm{Mn}}^{2+} \mathrm{and} {\mathrm{SO}}_2$. The excess of $KMn{O}_4$ is completely reacted with 175 ml 1M $F{e}^{2+}$ in acidic medium. Percentage of CuS in hte mixture will be
1.  37%
2.  47%
3.  57%
4.  67%

In Haber processes, 30 L  of dihydrogen and 30L of dinitrogen were taken for the reaction which yielded only 50% of the expected product. What will be the composition of the gaseous mixture under the aforesaid conditions in the end?
1. 20L of ammonia, 25L of nitrogen, 15L of hydrogen
2. 20L of ammonia, 20L of nitrogen, 20L of hydrogen
3. 10L of ammonia, 25L of nitrogen, 15L of hydrogen
4. 20L of ammonia, 10L of nitrogen, 30L of hydrogen

25 ml of a mixture of NaOH and ${\mathrm{N}}_2{\mathrm{CO}}_3$ is titrated against N/10 HCI using phenolphthalin as an indicator then the volume of HCI used was 20 ml. Now, the same 25 ml of the same mixture is titrated against N/10 HCI using methyl orange indicator then the volume of HCI used was 25 ml. Weight of NaOH is the mixture will be
1. 0.02 gm
2. 0.04 gm
3. 0.06 gm
4. 0.08 gm

Dehydration of cyclohexanol yields cyclohexene in 75% yield. How much of cyclohexene will be obtained from 100g of cyclohexanol?
1. 75.0g
2. 61.5g
3. 82.0g
4. 41.0g

The maximum volume at STP is occupied by
1.  12.8g of $S{O}_2$
2.  $6.02 \times {10}^{22} \mathrm{molecules} \mathrm{of} {\mathrm{CH}}_4$
3.  0.5 mol of $N{O}_2$
4.  1 gm-molecule of $C{O}_2$

5.6L of a gas at STP weighs equal to 8g.
The vapour density of gas is:
1. 32
2. 16
3. 8
4. 40

What will be the molarity 20% (by mass) NaOH solution, if the density of the solution is 1.2 gm/cc?
1. 6 M
2. 3 M
3. 0.5M
4. 5 M

0.16g of dibasic acid requires 25 ml decimolar NaOH solution for complete neutralization. The molecular mass of the acid is
1. 256
2. 64
3. 32
4. 128

A metal nitride ${\mathrm{M}}_3 {\mathrm{N}}_2$ contains 28% of nitrogen. The atomic mass of metal M is:
1. 24
2. 54
3. 9
4. 87.62

The volume of water to be added to 100 ${\mathrm{cm}}^3 \mathrm{of} 0.5 {\mathrm{NH}}_2{\mathrm{SO}}_4$ to get decinormal concentration is
1. 400 ${\mathrm{cm}}^3$
2. 500 ${\mathrm{cm}}^3$
3. 450 ${\mathrm{cm}}^3$
4. 100 ${\mathrm{cm}}^3$

The equivalent weight of ${\mathrm{H}}_3{\mathrm{PO}}_4$ in the following reaction is,
${\mathrm{H}}_3{\mathrm{PO}}_4+\mathrm{Ca}{\left(\mathrm{OH}\right)}_2\to {\mathrm{CaHPO}}_4+2{\mathrm{H}}_2\mathrm{O}$
1. 98
2. 49
3. 32.66
4. 40

The law of multiple proportions is illustrated by:
1. Carbon monoxide and carbon dioxide
2. Potassium bromide and potassium chloride
3. Water and heavy water
4. Calcium hydroxide and barium hydroxide