3) Phosphorous trichloride reacts with chlorine to phosphorous pentachloride. In this gas-phase reaction the starting amounts are 0.2 mol phosphorous trichloride and 0.1 mol chlorine at 250° C and a (constant) volume of 1 L. In equilibrium, the number of moles for phosphorous trichloride is 0.12 mol. Determine the starting concentrations, the equilibrium concentrations, and the equilibrium constant! You can use Kc in this case.
3) Phosphorous trichloride reacts with chlorine to phosphorous pentachloride. In this gas-phase reaction the starting amounts are 0.2 mol phosphorous trichloride and 0.1 mol chlorine at 250° C and a (constant) volume of 1 L. In equilibrium, the number of moles for phosphorous trichloride is 0.12 mol. Determine the starting concentrations, the equilibrium concentrations, and the equilibrium constant! You can use Kc in this case.
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.81P
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please help me with question 3. Thank you, a detailed explanation would help a lot.
![3) Phosphorous trichloride reacts with chlorine to phosphorous pentachloride. In this gas-phase
reaction the starting amounts are 0.2 mol phosphorous trichloride and 0.1 mol chlorine at
250° C and a (constant) volume of 1 L. In equilibrium, the number of moles for
phosphorous trichloride is 0.12 mol. Determine the starting concentrations, the equilibrium
concentrations, and the equilibrium constant! You can use Kc in this case.
4) For the reaction in #3, the reaction enthalpy is -88 kJ. In which way will both the
concentration of chlorine and the equilibrium constant K, be influenced, if
a) PCI3 is added?
b) PCI5 is added?
c) the temperature is raised?
d) the volume is reduced?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3f41cc0c-1bd1-4c63-bff1-d9a8b87d82b8%2F949a70ed-7e70-46ea-a68d-02a7e7b68f83%2Fsrx49o2_processed.jpeg&w=3840&q=75)
Transcribed Image Text:3) Phosphorous trichloride reacts with chlorine to phosphorous pentachloride. In this gas-phase
reaction the starting amounts are 0.2 mol phosphorous trichloride and 0.1 mol chlorine at
250° C and a (constant) volume of 1 L. In equilibrium, the number of moles for
phosphorous trichloride is 0.12 mol. Determine the starting concentrations, the equilibrium
concentrations, and the equilibrium constant! You can use Kc in this case.
4) For the reaction in #3, the reaction enthalpy is -88 kJ. In which way will both the
concentration of chlorine and the equilibrium constant K, be influenced, if
a) PCI3 is added?
b) PCI5 is added?
c) the temperature is raised?
d) the volume is reduced?
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