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Question#1

The right option for mass of CO2 produced by heating 20g of 20% pure lime is  NEET2023

\( CaCO_3 \rightarrow CaO + CO_2 \) 

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Question#2

1.5 mol of O2 combine with Mg to form oxide MgO . The mass of Mg (at. mass 24) that has combined is [KCET 2001]

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Question#3

H 2 evolved at STP on complete reaction of 27 g of Aluminium with excess of aqueous NaOH would be [CPMT 1991]

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Question#4

If \(1 \frac{1}{2} \) moles of oxygen combine with \( Al \)  to form \( Al_2O_3 \)  the weight of \( Al \)  used in the reaction is (Al=27) [EAMCET 1980]

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Question#5

Stoichiometry is NUMS-2021

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Question#6

What is the weight of oxygen required for the complete combustion of 2.8 kg of ethylene [CBSE PMT 1989]

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Question#7

Assuming fully decomposed, the volume of CO2 released at STP on heating 9.85g of BaCO3 (Atomic mass of Ba=137) will be [CBSE PMT 2000] 

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Question#8

The number of gram molecules of oxygen in 6.02 x1024 CO molecules is 1990

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Question#9

\( 2XeF_6 + SiO_2 \rightarrow 2XeOF_4 + SiF_4 \) 

If 122.6g of XeF6 reacts with 60g of SiO2 to form the product. Select the limiting reagent and amount of SiF4 formed . XeF6=245.3amu SiO2= 60amu SiF4=104amu ETEA2016 Medical qNo28

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Question#10

The volume of CO2 produced by heating 33.5g Li2CO at room temprature and pressure. ETEA2018 eng

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Question#11

\( 2KClO_3 \rightarrow KCl + 3O_2 \)    

Molecular mass of KClO3 =122.5g/mol for the production of 33.6dm3 of O At STP the mass of KClO3 to be decomposed is.  ETEA-2018-eng



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Question#12

A mixture of 2.3g of formic acid and 4.5g oxalic acid is treated with con.H2SO4 . The evolved gaseous mixture is passed through  KOH pellets. Weight of remaining product at STP will be NEET2018

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Question#13

Number of mole of hydrogen molecules required to produce 20mole of ammonia through Haber's process  NEET-2019

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Question#14

How many mole of calcium are present in 1.75Kg of calcium carbonate ? MDCAT2019

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Question#15
How many mole of Calcium are present in 1.75kg of Calcium carbonate ? MdCAT 2019
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Categories
1.    Introduction To Fundamental
         Atomic Mass
         Empirical formula
         Molecular Formula
         Concept of Mole
         Stoichiometry
         Limiting Reactant
         Percentage yield
2.    Atomic Strcuture
         Constituents of atom
         Properties of canal rays
         Rutherford Model
         Planks Theory
         Spectrum
         Bohr Model
         Hydrogen Spectrum
         de Broglie relation
         Uncertainty principle
         Quantum Number
         Electronic configuration
4.    Liquids
         Intermolecular forces
         hydrogen Bonding
         Evaporation
         Vapor Pressure
5.    Solids
         Types of Solids
         Ionic Solids
         Covalent Solids
         Molecular Solids
         Metallic solids
         Unit Cell
         Crystal System
7.    Reaction kinetics
10.    chemical Bonding
         Valency
         Octate Rule
         Ionization Energy
         Electron affinity
         Electronegativity
         Ionic Bond
         Covalent Bond
         Polarization
         Coordinate covalent Bond
         Sigma and pi Bond
         Hydrogen Bond
         VSEPR theory
         VBT
         Hybridization
         MOT
         Dipole moment
14.    Chemistry Of Hydrocarbons
17.    Alkyl halides
         IUPAC system
         SN1 & SN2
         E1 & E2
         Nucleophile and Base
20.    Macromolecules