The equilibrium constant for the reaction: #PCl_5 rightleftharpoons PCl_3 + Cl_2# is 0.0121. A vessel is charged with #PCl_5#, giving an initial pressure of 0.123 atmospheric. How do you calculate the partial pressure of #PCl_3# at equilibrium?
At equilibrium,
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To calculate the partial pressure of PCl3 at equilibrium, you would use the equilibrium constant expression for the reaction:
Kc = [PCl3][Cl2] / [PCl5]
Since the initial pressure of PCl5 is given as 0.123 atm and assuming it decreases by x at equilibrium, the equilibrium pressure of PCl5 would be (0.123 - x) atm.
Using stoichiometry, the equilibrium pressure of PCl3 and Cl2 would both be x atm.
Now, you can plug these values into the equilibrium constant expression and solve for x. Once you find the value of x, you can use it to calculate the equilibrium partial pressure of PCl3.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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