Home
Class 11
CHEMISTRY
In the reaction, A + B hArr2C, at equili...

In the reaction, `A + B hArr2C`, at equilibrium, the concentration of A and B is `0.20` mol `L^(-1)` each and that of C was found to be `0.60` mol `L^(-1)`. The equilibrium constant of the reaction is

A

`2.4`

B

`18`

C

`4.8`

D

`9`

Text Solution

Verified by Experts

The correct Answer is:
D
`A + B hArr 2C`
`K_(c) = ([C]^(2))/([A][B]) = ([0.6]^(2))/([0.2][0.2]) = 9`
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    A2Z|Exercise Le - Chatellers'S Principle|93 Videos

  • CHEMICAL EQUILIBRIUM

    A2Z|Exercise Degree Of Dissociation, Vapour Density And Simultaneous Equilibria|20 Videos

  • CHEMICAL EQUILIBRIUM

    A2Z|Exercise Calculation Of Equilibrium Constant|20 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    A2Z|Exercise Section D - Chapter End Test|30 Videos

  • CHEMICAL THERMODYNAMICS

    A2Z|Exercise Section D - Chapter End Test|30 Videos

Similar Questions

Explore conceptually related problems

For the system A(g)+2B(g)hArr C(g) , the equilibrium concentration is A="0.06 mol L"^(-1), B="0.12 mol L"^(-1), C="0.216 mol L"^(-1) . The equilibrium cosntant K_(C) for the reaction is

For the reaction, A iff n B the concentration of A decreases from 0.06 to 0.03 mol L^(-1) and that of B rises from 0 to 0.06 mol L^(-1) at equilibrium. The values of n and the equilibrium constant for the reaction, respectively, are

In the system X+2YhArrZ , the equilibrium concentration are, [X]=0.06" mol L"^(-1),[Y]=0.12" mol L"^(-1) , [Z]=0.216" mol L"^(-1) . Find the equilibrium constant of the reaction.

For reaction 2A+B hArr 2C, K=x Equilibrium constant for C hArr A+1//2 B will be

The initial molar concentration of the reactants A and B were 0.1 M and 0.2 M respectively in the following reaction A+B hArr 2C When equilibrium was attained the concentration of A in the reaction mixture was found to be 0.06M . Calculate the equilibrium constant.

A2Z-CHEMICAL EQUILIBRIUM-Application Of Equllibrium Constant (K)
  1. Theory of 'active mass' indicates that the rate of a chemical reaction...

    Text Solution

    |

  2. 56 g of nitrogen and 8 g hydrogen gas are heated in a closed vessel. A...

    Text Solution

    |

  3. In the reaction, A + B hArr2C, at equilibrium, the concentration of A ...

    Text Solution

    |

  4. At 298 K equilibrium constant K(1) and K(2) of following reaction SO(2...

    Text Solution

    |

  5. The rate at which a substance reacts, depends on its:

    Text Solution

    |

  6. For the reaction A+B hArr C+D, the initial concentrations of A and B a...

    Text Solution

    |

  7. Which of the following statements is false ?

    Text Solution

    |

  8. If in the reaction N(2)O(4) = 2N(2) , alpha is that part of N(2)O(4) w...

    Text Solution

    |

  9. 4.5 moles each of hydrogen and iodine heated in a sealed 10 litrevesel...

    Text Solution

    |

  10. 1.50 moles each of hydrogen and iodine is p[laced in a sealed 10 litre...

    Text Solution

    |

  11. In a 0.25 L tube dissociation of 4 mol of NO is taking place. If its d...

    Text Solution

    |

  12. On decomposition of NH(4)HS , the following equilibrium is estabilishe...

    Text Solution

    |

  13. 15 moles of H(2) and 5.2 moles of I(2) are mixed are allowed to attain...

    Text Solution

    |

  14. 1.1 mole of A mixed with 2.2 mole of B and the mixture is kept in a 1 ...

    Text Solution

    |

  15. An equilibrium mixture in a vessel of capacity 100 litre contain 1 mo...

    Text Solution

    |

  16. The reaction, PC1(5)hArrPC1(3) + C1(2) is started in a 5 litre contain...

    Text Solution

    |

  17. Some gaseous equilibrium are given below: CO + H(2)OhArrCO(2) + H(2)...

    Text Solution

    |

  18. In a container equilibrium N(2)O(4) (g)hArr2NO(2) (g) is attained at 2...

    Text Solution

    |

  19. Ammonia gas at 15 atm is introduced in a rigid vessel at 300 K. At equ...

    Text Solution

    |

  20. K(c) = 9 for the reaction, A + B hArrC + D. If A and B are taken in eq...

    Text Solution

    |