Leave a Message!
Please Sign in/ Signup to leave a message.
Question#1

In the reaction \( A + 2B \leftrightarrow 2C \)  , if 2 moles of A, 3.0 moles of B and 2.0 moles of C are placed in a 2.0L flask and the equilibrium concentration of C is 0.5 mole/ L . The equilibrium constant Kc for the reaction is [KCET 1996] 

Please select an option
Question#2

In a chemical equilibrium, the rate constant of the backward reaction is 7.5 x 10-4 and the equilibrium constant is 1.5. So the rate constant of the forward reaction is [KCET 1989] 

Please select an option
Question#3

A mixture of 0.3 mole of H2 and 0.3 mole of I2 is allowed to react in a 10 litre evacuated flask at 500oC . The reaction is  \( H_2 + I_2 \leftrightarrow 2HI \)  , the K is found to be 64. The amount of unreacted I2 at equilibrium is [KCET 1990] 

Please select an option
Question#4

A quantity of PCl5 was heated in a 10 litre vessel at 250oC \(  PCl_5 (g) \leftrightarrow PCl_3(g) + Cl_2 (g) \)  . At equilibrium the vessel contains 0.1 mole of PCl5 0.20 mole of PCl3 and 0.2 mole of Cl 2. The equilibrium constant of the reaction is [KCET 1993, 2001; MP PMT 2003] 

Please select an option
Question#5

For the reaction \( 2SO_2 + O_2 ? 2SO_3 \) , the units of Kc are [CPMT 1990] 

Please select an option
Question#6

\( A + B \leftrightarrow C + D \) . If finally, the concentration of A and B are both equal but at equilibrium concentration of D will be twice of that of A then what will be the equilibrium constant of reaction. [BHU 2005] 

Please select an option
Question#7

For the reaction \( N_2(g) + 3H_2(g) \leftrightarrow 2NH_3(g) \) the correct expression of equilibrium constant K is [CPMT 1984, 2000] 

Please select an option
Question#8

In a chemical equilibrium \( A + B \leftrightarrow C + D \) , when one mole each of the two reactants are mixed, 0.6 mole each of the products are formed. The equilibrium constant calculated is [CBSE PMT 1989] 

Please select an option
Question#9

Concentration of a gas is expressed in the following terms in the calculation of equilibrium constant [EAMCET 1982] 

Please select an option
Question#10

For the system \( 3A + 2B \leftrightarrow C \) the expression for equilibrium constant is [NCERT 1981; CPMT 1989; MP PMT 1990; RPMT 1999; Pb. PMT 2002; Pb. CET 2002] 

Please select an option
Question#11

Unit of Kc for following reaction is H2 + I2 -------> 2HI  MDACT2010

Please select an option
Question#12

A reaction between CO and H20 is 

\(CO+H_2 O \longleftrightarrow CO_2+ H_2\)

The unit of equilibrium for this reaction is ETEA2010


Please select an option
Question#13

Select the correct equilibrium constant expression, Kc for the following reversible reaction. 

Ce+4 (aq) + Fe+2 (aq)<=====> Ce+3(aq) + Fe+3(aq) ETEA2012 Med

Please select an option
Question#14

The equilibrium constant in a reversible reaction at a given temperature [AIIMS 1982]

Please select an option
Question#15

A reversible chemical reaction having two reactants in equilibrium. If the concentrations of the reactants are doubled, then the equilibrium constant will [CPMT 1982, 90; MP PMT 1990,2004; MNR 1992; UPSEAT 2002; KCET 1999; Pb. CET 2004]

Please select an option
Question#16

On a given condition, the equilibrium concentration of HI, H2 and I2 are 0.80, 0.10 and 0.10 mole/litre. The equilibrium constant for the reaction H2 + I2 ------> 2HI will be [MP PET 1986]

Please select an option
Question#17

4 moles of A are mixed with 4 moles of B. At equilibrium for the reaction A + B ----> C + D , 2 moles of C and D are formed. The equilibrium constant for the reaction will be [CPMT 1992]

Please select an option
Question#18

In the reversible reaction A + B ------> C + D , the concentration of each C and D at equilibrium was 0.8 mole/litre, then the equilibrium constant Kc will be [MP PET 1986]

Please select an option
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