Chemistry Forum

7. During the mixing of gaseous substances D and G, the elementary chemical reaction occurs:

2D+G->2C+B

After some time from the start of the reaction, the transformation of the substances became:

[D]=4 mol/I,[G]=2 mol/,[C]=3.2 mol/l

Calculate:

a) initial concentration of substances

b) the initial speed if the speed determination is 0.5. l^2×mol^-2×s^-1
c)argument how the speed of the chemical reaction changes with the increase of the effective hits of the reactants

2D + G => 2C + B
In equilibrium we have 4 mol/l D , 2 mol/l G and 3,2 mol/l C
In beginning there is no C and no B. So it means 3,2 mol C are produced, what means 2 D gives 2 C. 3,2 mol C has to be add to D what gives 7,2 mol/l . 3,2 mol C means also the half of G = 1,6 mol/l has to be used. So in beginning it was 3,6 mol/ l. In equilibrium at least B is 1,6 mol/l.

K = 3,2^2*1,6/(4^2*2) = 0,512

3,2 mol C has to be add to D what gives 7,2 mol/l

But D is being used shouldnt we remove 3.2 moles from D?

The 3.2 is removed from 7.2 to get final 4.

Ahaa got it thxxxx