Carbon disulfide is prepared by heating sulfur and charcoal. the chemical equation is s2(g)+c(s)↽−−⇀cs2(=9.40 at 900 k how many grams of cs2(g) can be prepared by heating 8.08 mol s2(g) with excess carbon in a 5.35 l reaction vessel held at 900 k until equilibrium is attained?

Answer : The mass of is, 555.028 grams

Explanation :

First er have to calculate the concentration of .

Now we have to calculate the concentration of .

The given balanced chemical reaction is,

Initial conc.         1.51       0         0

At eqm. conc.   (1.51-x)  (x)       (x)

The expression for equilibrium constant for this reaction will be,

Now put all the given values in this expression, we get :

By solving the term 'x', we get :

x = 1.365 M

Concentration of = x M = 1.365 M

Now we have to calculate the moles of .

Now we have to calculate the mass of .

Molar mass of = 76 g/mole

Therefore, the mass of is, 555.028 grams

i know insulin is primary but i dont know the others im sorry

explanation: