An equilibrium mixture contains 0.600 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-l container. this is the equation: co(g)+h2o(> < -- co2(g) + h2(g). how many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol?

Answer : The moles of added will be 1.12 mole.

Solution :  Given,

Moles of and at equilibrium = 0.200 mol

Moles of and at equilibrium = 0.600 mol

First we have to calculate the concentration of at equilibrium.

Now we have to calculate the value of equilibrium constant.

The given equilibrium reaction is,

The expression of will be,

Now we have to calculate the moles of added.

Let the moles of added is 'x'.

The given equilibrium reaction is,

Initially              0.200   0.200         0.600    0.600

Added moles       0           0                 x             0

Change             +0.1       +0.1             -0.1         -0.1

Final                   0.3         0.3          (0.5+x)        0.5

The expression of will be,

Therefore, the moles of added will be 1.12 mole.

chemistry sucks a**

explanation:

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.