For the reaction 2H2S(g) – 2H2(g) + S2(g), Kc = 9.1x102 at 750 K. What will happen when 0.10 mol of H2S, 1.0 mol of H2, and 1.5 mol of S2 are added
to a 1.0-L container and the system is brought to 750 K?
Nothing; the system is at equilibrium.
More H2S will be formed.
More S2 will be formed than H2.
The amount of H2 formed will be half the amount of S2 formed.
More H2 will be formed than S2.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

answer carbon and three oxygen atoms;