An equal number of moles of i2(g) and br2(g) are placed into a closed container and allowed to establish the following equilibrium:
i2(g) + br2(g) 2ibr(g)
keq = 280
which one of the following relates [ibr] to [i2] at equilibrium?
[i2] = [ibr]
[i2] < [ibr]
[i2] = 2 [ibr]
[i2] = 280 [ibr]

Answer : The correct option is,

Solution : Given,

Moles of = Moles of

The balanced equilibrium reaction is,

The expression for equilibrium constant is,

As per question, Moles of = Moles of

Now put all the given values in above formula, we get the relation between the and .

From this we conclude that the concentration of is greater than the concentration of .

Therefore, the correct option is,

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.