Most Expected Questions of MOLE CONCEPT & STOICHIOMETRY

 

When 5 moles of Ca (OH)2 mixed with 4 Moles of H3PO4 The limiting reagent in.

1) Ca(OH)2 2) H3 PO4 3) both 4)we cannot predict

For the reaction 2A +B→C, 8 moles of A and excess of B will produce

1) 8 moles of C 2) 5 moles of C 3) 4 moles of C 4) 13 moles C

Number of moles of KI required for the preparation of K2Hg I4 from 0.5 moles of 

HgCl2

1). 0.5 2) 1 3) 1.5 4) 2

4g of mixture CaCO3 and MgCO3 upon heating produces 4g of MgO what volume 

of CO2 produced from the mixture at STP (273 K 1 atm)

1) 2.24L 2)3.36L 3) 1.12L 4) 4.48L

When 2 liters of mixture of CO and CO2 passed over red hot coke 3.2 liters of the CO is obtained what volume of CO2 present in the original mixture 

1)0.6 L 2)1.2 L 3)0.8 L 4)1.6 L

2.76g of silver carbonate on strong ignition leaves a residue weighing

1)2.48g 2)2.16g 3)2.32g 4)2.84g

The number of moles of CO2 produced when 3 moles of HCl react with excess of 

CaCO3 is

1)1 2)1.5 3) 2 4)2.5

What volume of H2 at NTP is required to convert 2.8g of N2 into NH3?

1)2240ml 2)22400 ml 3)6.72lit 4)224 lit 

The weight of NaOH in gram that

completely neutralizes 9.8g of phosphoric acid is 

1)120 2)24 3)63 4)12

The volume of CO2 obtained by the complete decomposition of one mole of 

NaHCO3at STP is 

1) 22.4 L 2)11.2L 3)44.8L 4)4.48L

The amount of Mg in gms. to be dissolved in dilute H2SO4 to liberate H2 which is just sufficient to reduce 160g of ferric oxide is.

1)24 2)48 3)72 4)84

x’ grams of calcium carbonate was completely burnt in air The weight of the solid residue formed is 28g .What is the value of ‘x’ (in grams)?

 1) 44 2)200 3)150 4)50

X forms an oxide X2O3, 0.36 grams of X forms 0.56 grams of X2Oyso the atomic 

weight of X is 

1)36 2)565 3)28 4)43.2

The number of moles of Fe2O3 formed when 5.6 lit if O2 reacts with 5.6g of Fe is

 1)0.125 2)0.01 3)0.05 4)0.10

If 0.5 mol of BaCl2 is mixed with 0.2 mol of Na3PO4 the maximum number of moles of Ba3(PO4)2 Formed

1)0.7 2)0.5 3)0.1 4)3

40 ml of a hydrocarbon undergoes combustion in 260ml of oxygen and gives 160ml of CO2 If all volumes are measured under similar conditions of temperature and pressure, the formula of the hydrocarbon is 

1)C3H8 2)C4H8 3)C4H14 4) C4H10

10ml of a gaseous hydrocarbon on combustion gives 40 ml of CO2 and 50 ml vapour under the same conditions. The hydrocarbon is 

1) C4H6 2)C6H10 3)C4H8 4)C4H10

Acetylene can be prepared from calcium carbonate by a series of reactions. The mass of 80% calcium carbonate required to prepare 2 moles of acetylene is

1)220g 2)160g 3)250g 4)320g

The mass of 80% pure H2SO4 required to completely neutralize 60g of NaOH is 

1)92 g 2)58.8 g 3)73.5 g 4)98 g

4g of a mixture of Na2CO3 and NaHCO3 on heating liberates 448 ml of CO2 at STP 

percentage of Na2CO3 in the mixture is 

 1)84 2)16 3)54 4)80

How many moles of Zn(Fe S2) from 2 moles of Zn , 3 moles of Fe , 5 moles of ‘ S’ 

atoms

A gas mixture Contains C2H4 and CO2. 40 liter of this mixture require 30 liter of O2

for combustion. The percentage of CO2 in the original mixture is

What volume of O2 Required for the combustion of 1.4 liters of propane (C3H8) under similar conditions 

25g of mixture of Na CO 2 3 and NaHCO3upon heating looses 6.2g of weight what is the percentage of NaHCO3 is the mixture

If a mixture of 3 moles of hydrogen (H2) one mole of (N2) converted completely to 

NH3 the ratio of initial and final value at the same temperature and pressure is

One gram of impure Mg when treated with dilute acid gave 896 CC of H2 at (O0C and 1 atm) what is the percentage of Mg in the metal

0.2 moles of a compound SxCly upon several reactions produces 0.2 moles PbCl2 and 0.4 moles BaSO4 Then(X+Y) is

How many liters of air contains 21% of O2 is required for the combustion of 4 g of 

methane (CH4) give the answer in four significant figurers (O0C and 1 atoms)

68 g of H2O2 Upon complete decomposition produces O2 the oxygen produced can burn how many grams of Mg metal

The number of moles potassiumchlorate needed to produce 11.2 liter of oxygen at 

NTP is 1/x the ‘x’ can be

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