QUESTION 13 Consider the following reaction CO(g) + 3H2 (g)# CH4(g) + H2O(g) Kp

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QUESTION 13 Consider the following reaction CO(g) + 3H2 (g)# CH4(g) + H2O(g) Kp 138 at 1200 K Assurme the reaction has reached equitrum Then, the presszeisincreased by makigtho reaction vesse smaller. How wil the maction?pond tone. establish equilbrium? Kc will change to a larger value Kc will change to a smaller value no change: the reaction will still be at equiibrium the reverse reaction will establish more reactants the forward reaction wil establish more products QUESTION 14 Click Save and Submit to sove and submit. Click Save All Answers to ste all answers Save All A a88 a 5 option command

Explanation / Answer

In the given reaction, the number of moles of gaseous reactants =4

and the number of moles of gaseous product = 2

Kp = [ CH4][H2O]] / [CO][H2]3 = 138

When the pressure is increased, then the reaction willshift in a direction having lesser number of moles i.e. towards product by Le-Chatlier Principle which states that when a reaction in equilibrium is subjected to a change in reaction conditions(pressure,temperature,volume etc) then the equilibrium will shift in a direction to undo the effect of change.

Thus in this system, Pressure is increased , so reaction will shift in a direction which favors less pressure

Now, pressure is directly proportional to number of moles

Thus reaction will favor forward reaction forming more products.

Thus, the forward reaction will establish more products.

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