Consider the reaction:

Complete the table. Assume that all concentrations are equilibrium concentrations in moles per liter, M.

T(°C) |
H2 |
[I2] |
[HI] |
Keq |

25 |
0.355 |
0.388 |
0.0922 |
______ |

340 |
______ |
0.0455 |
0.387 |
9.6 |

445 |
0.0485 |
0.0468 |
______ |
50.2 |

Solution 62P :

Step 1:

Given the reaction:

H2(g) + I2(g) ⇋ 2HI(g)

Here, we have to complete the table assuming that all concentrations are equilibrium concentrations in moles per liter, M.

T(°C) |
H2 |
[I2] |
[HI] |
Keq |

25 |
0.355 |
0.388 |
0.0922 |
______ |

340 |
______ |
0.0455 |
0.387 |
9.6 |

445 |
0.0485 |
0.0468 |
______ |
50.2 |

We know the formula for equilibrium constant (Kc or Keq):

Keq = , i.e Keq =

Now, consider 1st row :

T(°C) = 25

H2 = 0.355

[I2] = 0.388

[HI] = 0.0922

Keq = ?

Hence, Keq =

= 0.0617

Step 2:

Now, consider 2nd row :

T(°C) = 340

H2 = ?

[I2] = 0.0455

[HI] = 0.387

Keq = 9.6

Keq =

9.6 =

[] =

= 0.34287