May 31, 2016

Homework Help: Chemistry-w/addition

Posted by Fred on Saturday, January 15, 2011 at 2:13pm.

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

(a) An 59.8 gram sample of SbCl5 (molecular weight 299.0) is placed in an evacuated 15.0 liter container at 182C.

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 182C, calculate the values for equilibrium constants Kp and Kc, for this decomposition reaction.

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 182C. 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 This Question

First Name:
School Subject:

Related Questions

More Related Questions