At elevated temperatures, SbCl5 gas decomposes into SbCl3 gas and Cl2 gas as shown by the following equation: SbCl5(g)<=> SbCl3(g) + Cl2(g)

Question

1. What is the concentration in moles per liter of SbCl5 in the container before any decomposition occurs?

2. What is the pressure in atmospheres of SbCl5 in the container before any decomposition occurs?

b)If the SbCl5 is 29.2 percent decomposed when equilibrium is
established at 182°C, calculate the values for equilibrium constants Kp and Kc, for this decomposition reaction.
Kc=?
Kp=?

c.In order to produce some SbCl5, a 1.00 mole sample of SbCl3 is first
placed in an empty 2.00 liter container maintained at a temperature
different from 182ºC. At this temperature, Kc, equals 0.117. How many moles of Cl2 must be added to this container to reduce the number of
moles of SbCl3 to 0.500 mole at equilibrium?

Answer 1

I think you need more information. Do you have a number of moles? a volume? pressure?
1. (Cl2) = 0; (SbCl3) = 0; (SbCl5) = whatever you started with.