Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is

s2(g)+C(s)-->CS2(g) Kc=9.40 at 900k
How many grams of CS2(g) can be prepared by heating 14.5 moles of S2(g) with excess carbon in a 8.15 L reaction vessel held at 900 K until equilibrium is attained?

To solve this problem, we will use the given chemical equation and the equilibrium constant (Kc) to determine the moles of CS2(g) that can be prepared by reacting 14.5 moles of S2(g) in a 8.15 L reaction vessel held at 900 K.

The balanced chemical equation is:
S2(g) + C(s) → CS2(g)

According to the equation, the stoichiometric ratio between S2(g) and CS2(g) is 1:1.

First, let's calculate the initial number of moles of CS2(g) that can be formed:

Initial moles of S2(g) = 14.5 moles
Since the stoichiometric ratio is 1:1, this means that initially, the moles of CS2(g) formed are also 14.5 moles.

Now, we need to use the equilibrium constant to determine the equilibrium concentration of CS2(g).

Kc = [CS2(g)] / [S2(g)]
Given: Kc = 9.40

Since the initial concentration of S2(g) is 14.5 moles in an 8.15 L reaction vessel, the concentration of [S2(g)] is:
[S2(g)] = 14.5 mol / 8.15 L = 1.78 M

Using the equation for the equilibrium constant, we can rearrange it to solve for [CS2(g)]:
[CS2(g)] = Kc * [S2(g)]

[CS2(g)] = 9.40 * 1.78 M = 16.692 M

Now, we need to calculate the number of moles of CS2(g) at equilibrium using the equilibrium concentration and the volume of the reaction vessel:

Equilibrium moles of CS2(g) = [CS2(g)] * Volume
Equilibrium moles of CS2(g) = 16.692 M * 8.15 L = 136.01 moles

So, the maximum number of moles of CS2(g) that can be prepared by heating 14.5 moles of S2(g) is 136.01 moles.

Finally, to calculate the mass of CS2(g) formed, we need to use its molar mass:

Molar mass of CS2 = 12.01 g/mol (C) + 32.07 g/mol (S)
Molar mass of CS2 = 44.08 g/mol

Mass of CS2(g) = Number of moles * Molar mass
Mass of CS2(g) = 136.01 moles * 44.08 g/mol = 5,995.88 grams

Therefore, the maximum mass of CS2(g) that can be prepared is 5,995.88 grams.