Consider the following equilibrium reaction at a given temperature: A (aq) + 3 B (aq) ⇌ C (aq) + 2 D (aq) Kc = 178. If initially the concentrations of the chemical species are as follows: [A]o = 0.364 M [B]o = 0.170 M [C]o = 0.132 M [D]o = 0.932 M to which direction will the reaction run to reach equilibrium?

The reaction proceed toward product side or in forward direction.

Explanation:

is the constant of a certain reaction at equilibrium while is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.

For the given chemical reaction:

The expression of for above equation follows:

We are given:

Putting values in above equation, we get:

We are given:

There are 3 conditions:

As, , the reaction will be favoring product side.

Hence, the reaction proceed toward product side or in forward direction.

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.