NEET Questions - Chemistry - Some Basic Concepts in Chemistry

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A gaseous compound is composed of 85.7% by mass carbon and 14.3% by mass hydrogen. It's density is 2.28 g/litre at 300 K and 1.0 atm pressure. Determine the molecular formula of the compound:

C_{2} H_{2}

C_{2} H_{4}

C_{4} H_{8}

C_{4} H_{10}

Calculate the % of free ${SO}_{3}$ in oleum (a solution of ${SO}_{3}$ in $H_{2} {SO}_{4}$ ) that is labelled 109% $H_{2} {SO}_{4}$ .

40
30
50
None

Suppose two elements X and Y combine to form two compounds ${XY}_{2}$ and $X_{2} Y_{3}$ when 0.05 mole of ${XY}_{2}$ weighs 5 g while 3.011 $\times$ 10²³ molecules of $X_{2} Y_{3}$ weighs 85 g. The atomic masses of x and y are respectively:

20, 30
30, 40
40, 30
80, 60

40 milligram diatomic volatile substance $(X_{2})$ is converted to vapour that displaced 4.92 mL of air at 1 atm and 300 K. Atomic weight of element X is nearly:

400
240
200
100

For the reaction; $2 Fe {({NO}_{3})}_{3} + 3 {Na}_{2} {CO}_{3} \overset{}{\to} {Fe}_{2} {({CO}_{3})}_{3} + 6 {NaNO}_{3}$

Initially if 2.5 mole of $Fe {({NO}_{3})}_{2}$ and 3.6 mole of ${Na}_{2} {CO}_{3}$ is taken. If 6.3 mole of ${NaNO}_{3}$ is obtained then % yield of given reaction is:

50
84
87.5
100

0.8 mole of a mixture of CO and CO₂ requires exactly 40 gram of NaOH in solution for complete conversion of all the CO₂ into Na₂CO₃. How many moles more of NaOH would it require for conversion into Na₂CO₃, if mixture (0.8 mole) is completely oxidised to CO₂?

0.2
0.6
1
1.5

The impure 6 g of $NaCl$ is dissolved in water and then treated with excess of silver nitrate solution. The weight of precipitate of silver chloride is found to be 14 g. The % purity of $NaCl$ solution would be:

95%
85%
75%
65%

25.4 of $I_{2}$ and 14.2 g of ${Cl}_{2}$ are made to react completely to yield a mixture of ICI and ICI₃. Calculate mole of ICI and ICI₃ formed.

0.5 ,02
0.1, 0.1
0.1 ,0.3
0.3,0.4

The vapour density of a mixture containing ${NO}_{2}$ and $N_{2} O_{4}$ is 38.3. Calculate the mole of ${NO}_{2}$ in 100 g mixture.

0.437
0.347
0.557
0.663

Copper forms two oxides. For the same amount of copper, twice as much oxygen was used to form first oxide than to form second one. What is the ratio of the valencies of copper in first and second oxides?

2:5
1:6
2:1
1:2

5 mL of a gaseous hydrocarbon was exposed to 30 mL of $O_{2}$ . The resultant gas, on cooling is found to measure 25 mL of which 10 mL is absorbed by NaOH and the remainder by pyrogallol. Determine molecular formula of hydrocarbon. All measurements are made at constant room temperature.

CH₄
C₂H₂
C₃H₄
C₂H₄

A sample of ${CaCO}_{3}$ and ${MgCO}_{3}$ weighed 2.21 g is ignited to constant mass of 1.152 g. What is the composition of mixture? Also calculate the volume of ${CO}_{2}$ evolved at $0 ° C$ and 76 cm of pressure.

640 ml
540 ml
500 ml
600 ml

The vapour density of a volume chloride of a metal is 95 and the specific heat of the metal is 0.13 cal/g. The equivalent mass of the metal will be:

6
12
18
24

Which mixture is lighter than humid air?

N_{2} + O_{2} + {SO}_{2}

N_{2} + O_{2} + {CO}_{2}

N_{2} + O_{2} + C_{2} H_{6}

N_{2} + O_{2} + He

NEET Chemistry Questions: Some Basic Concepts in Chemistry

Question bank:

A gaseous compound is composed of 85.7% by mass carbon and 14.3% by mass hydrogen. It's density is 2.28 g/litre at 300 K and 1.0 atm pressure. Determine the molecular formula of the compound:

Calculate the % of free ${SO}_{3}$ in oleum (a solution of ${SO}_{3}$ in $H_{2} {SO}_{4}$ ) that is labelled 109% $H_{2} {SO}_{4}$ .

Suppose two elements X and Y combine to form two compounds ${XY}_{2}$ and $X_{2} Y_{3}$ when 0.05 mole of ${XY}_{2}$ weighs 5 g while 3.011 $\times$ 10²³ molecules of $X_{2} Y_{3}$ weighs 85 g. The atomic masses of x and y are respectively:

40 milligram diatomic volatile substance $(X_{2})$ is converted to vapour that displaced 4.92 mL of air at 1 atm and 300 K. Atomic weight of element X is nearly:

For the reaction; $2 Fe {({NO}_{3})}_{3} + 3 {Na}_{2} {CO}_{3} \overset{}{\to} {Fe}_{2} {({CO}_{3})}_{3} + 6 {NaNO}_{3}$

Initially if 2.5 mole of $Fe {({NO}_{3})}_{2}$ and 3.6 mole of ${Na}_{2} {CO}_{3}$ is taken. If 6.3 mole of ${NaNO}_{3}$ is obtained then % yield of given reaction is:

0.8 mole of a mixture of CO and CO₂ requires exactly 40 gram of NaOH in solution for complete conversion of all the CO₂ into Na₂CO₃. How many moles more of NaOH would it require for conversion into Na₂CO₃, if mixture (0.8 mole) is completely oxidised to CO₂?

The impure 6 g of $NaCl$ is dissolved in water and then treated with excess of silver nitrate solution. The weight of precipitate of silver chloride is found to be 14 g. The % purity of $NaCl$ solution would be:

25.4 of $I_{2}$ and 14.2 g of ${Cl}_{2}$ are made to react completely to yield a mixture of ICI and ICI₃. Calculate mole of ICI and ICI₃ formed.

The vapour density of a mixture containing ${NO}_{2}$ and $N_{2} O_{4}$ is 38.3. Calculate the mole of ${NO}_{2}$ in 100 g mixture.

Copper forms two oxides. For the same amount of copper, twice as much oxygen was used to form first oxide than to form second one. What is the ratio of the valencies of copper in first and second oxides?

5 mL of a gaseous hydrocarbon was exposed to 30 mL of $O_{2}$ . The resultant gas, on cooling is found to measure 25 mL of which 10 mL is absorbed by NaOH and the remainder by pyrogallol. Determine molecular formula of hydrocarbon. All measurements are made at constant room temperature.

A sample of ${CaCO}_{3}$ and ${MgCO}_{3}$ weighed 2.21 g is ignited to constant mass of 1.152 g. What is the composition of mixture? Also calculate the volume of ${CO}_{2}$ evolved at $0 ° C$ and 76 cm of pressure.

The vapour density of a volume chloride of a metal is 95 and the specific heat of the metal is 0.13 cal/g. The equivalent mass of the metal will be:

Which mixture is lighter than humid air?

$O_{3}$ is absorbed by:

NEET Chemistry Questions: Some Basic Concepts in Chemistry

Question bank:

A gaseous compound is composed of 85.7% by mass carbon and 14.3% by mass hydrogen. It's density is 2.28 g/litre at 300 K and 1.0 atm pressure. Determine the molecular formula of the compound:

Calculate the % of free SO3 in oleum (a solution of SO3 in H2SO4) that is labelled 109% H2SO4.

Suppose two elements X and Y combine to form two compounds XY2 and X2Y3when 0.05 mole ofXY2 weighs 5 g while 3.011×1023 molecules of X2Y3 weighs 85 g. The atomic masses of x and y are respectively:

40 milligram diatomic volatile substance X2 is converted to vapour that displaced 4.92 mL of air at 1 atm and 300 K. Atomic weight of element X is nearly:

For the reaction; 2FeNO33 + 3Na2CO3 → Fe2CO33+6NaNO3 Initially if 2.5 mole of FeNO32 and 3.6 mole of Na2CO3 is taken. If 6.3 mole of NaNO3 is obtained then % yield of given reaction is:

0.8 mole of a mixture of CO and CO2 requires exactly 40 gram of NaOH in solution for complete conversion of all the CO2 into Na2CO3. How many moles more of NaOH would it require for conversion into Na2CO3, if mixture (0.8 mole) is completely oxidised to CO2?

The impure 6 g of NaCl is dissolved in water and then treated with excess of silver nitrate solution. The weight of precipitate of silver chloride is found to be 14 g. The % purity of NaCl solution would be:

25.4 of I2 and 14.2 g of Cl2 are made to react completely to yield a mixture of ICI and ICI3. Calculate mole of ICI and ICI3 formed.

The vapour density of a mixture containing NO2 and N2O4 is 38.3. Calculate the mole of NO2 in 100 g mixture.

Copper forms two oxides. For the same amount of copper, twice as much oxygen was used to form first oxide than to form second one. What is the ratio of the valencies of copper in first and second oxides?

5 mL of a gaseous hydrocarbon was exposed to 30 mL of O2. The resultant gas, on cooling is found to measure 25 mL of which 10 mL is absorbed by NaOH and the remainder by pyrogallol. Determine molecular formula of hydrocarbon. All measurements are made at constant room temperature.

A sample of CaCO3 and MgCO3 weighed 2.21 g is ignited to constant mass of 1.152 g. What is the composition of mixture? Also calculate the volume of CO2 evolved at 0°C and 76 cm of pressure.

The vapour density of a volume chloride of a metal is 95 and the specific heat of the metal is 0.13 cal/g. The equivalent mass of the metal will be:

Which mixture is lighter than humid air?

O3 is absorbed by:

Calculate the % of free ${SO}_{3}$ in oleum (a solution of ${SO}_{3}$ in $H_{2} {SO}_{4}$ ) that is labelled 109% $H_{2} {SO}_{4}$ .

Suppose two elements X and Y combine to form two compounds ${XY}_{2}$ and $X_{2} Y_{3}$ when 0.05 mole of ${XY}_{2}$ weighs 5 g while 3.011 $\times$ 10²³ molecules of $X_{2} Y_{3}$ weighs 85 g. The atomic masses of x and y are respectively:

40 milligram diatomic volatile substance $(X_{2})$ is converted to vapour that displaced 4.92 mL of air at 1 atm and 300 K. Atomic weight of element X is nearly:

For the reaction; $2 Fe {({NO}_{3})}_{3} + 3 {Na}_{2} {CO}_{3} \overset{}{\to} {Fe}_{2} {({CO}_{3})}_{3} + 6 {NaNO}_{3}$

Initially if 2.5 mole of $Fe {({NO}_{3})}_{2}$ and 3.6 mole of ${Na}_{2} {CO}_{3}$ is taken. If 6.3 mole of ${NaNO}_{3}$ is obtained then % yield of given reaction is:

0.8 mole of a mixture of CO and CO₂ requires exactly 40 gram of NaOH in solution for complete conversion of all the CO₂ into Na₂CO₃. How many moles more of NaOH would it require for conversion into Na₂CO₃, if mixture (0.8 mole) is completely oxidised to CO₂?

The impure 6 g of $NaCl$ is dissolved in water and then treated with excess of silver nitrate solution. The weight of precipitate of silver chloride is found to be 14 g. The % purity of $NaCl$ solution would be:

25.4 of $I_{2}$ and 14.2 g of ${Cl}_{2}$ are made to react completely to yield a mixture of ICI and ICI₃. Calculate mole of ICI and ICI₃ formed.

The vapour density of a mixture containing ${NO}_{2}$ and $N_{2} O_{4}$ is 38.3. Calculate the mole of ${NO}_{2}$ in 100 g mixture.

5 mL of a gaseous hydrocarbon was exposed to 30 mL of $O_{2}$ . The resultant gas, on cooling is found to measure 25 mL of which 10 mL is absorbed by NaOH and the remainder by pyrogallol. Determine molecular formula of hydrocarbon. All measurements are made at constant room temperature.

A sample of ${CaCO}_{3}$ and ${MgCO}_{3}$ weighed 2.21 g is ignited to constant mass of 1.152 g. What is the composition of mixture? Also calculate the volume of ${CO}_{2}$ evolved at $0 ° C$ and 76 cm of pressure.

$O_{3}$ is absorbed by: