a. The equation for the decomposition of hydrogen Iodide is
2HI (g) H2 (g) + I2 (g) H= +52kJ Write the equilibrium concentration for the reaction. b. i. Many industrial reactions make use of catalyst. What is a catalyst and explain how it works. ii. State and explain the effect of the catalyst on the value of the equilibrium constant and on the rate of reaction.
c. Using Le Chatelier’s principle and equation for the decomposition of hydrogen Iodide, explain the effect on the position of equilibrium of; i. Increasing the pressure at constant temperature. ii. Increasing temperature.
Answers
(a). Hey, Your Question is little bit wrong. There is no need of the Enthaly as given in the question. From the Enthaly Equilibrium conc. can not be calculated until the temp. or other conditions are not given in the question.
I think, We need to find the Expression for the equilibrium constant expressing the Equilibrium concentration.
The Equilibrium constant is given by,
2HI ⇒ H₂ + I₂
Kc = [H₂][I₂]/[HI]²
Now, In the question there must be given the concentration of the Hydrogen, Iodine and Hydrogen Iodide at the Equilibrium. So by putting this value there, you may fin d the answer.
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(b).
(i) Catalyst are those materials which are used in the chemical reaction so to increase its rate without undergoing change in themselves.
(ii) Catalyst does not have any effects on the equilibrium. But it increase the rate of the reaction and nothing else.
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(c).
(i) If the Pressure is increased in the equilibrium then reaction will move in the Backwards direction because no. of moles are less in the backwards direction.
(ii). This reaction is endothermic in nature. Now, we know that for the endothermic reaction, increase in temperature causing the reaction to move in the Forward direction and vice versa.
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Hope it helps.
Y=VosinѲt-1/2a2t2
-3.0m=Vsin30ot-(4.9m/s2)t2
-3.0m=(20m)tan30o-4.9x400
V2cos230os2
V = 13.4m/s