In addition to serving individual customers, other companies, and the government, who do many workers in this cluster provide se
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The given question is incomplete. The complete question is :
Carbon tetrachloride can be produced by the following reaction:
Suppose 1.20 mol of and 3.60 mol of
were placed in a 1.00-L flask at an unknown temperature. After equilibrium has been achieved, the mixture contains 0.72 mol of
. Calculate equilibrium constant at the unknown temperature.
Answer: The equilibrium constant at unknown temperature is 0.36
Explanation:
Moles of = 1.20 mole
Moles of = 3.60 mole
Volume of solution = 1.00 L
Initial concentration of =
Initial concentration of =
The given balanced equilibrium reaction is,
Initial conc. 1.20 M 3.60 M 0 0
At eqm. conc. (1.20-x) M (3.60-3x) M (x) M (x) M
The expression for equilibrium constant for this reaction will be,
Now put all the given values in this expression, we get :
Given :Equilibrium concentration of , x =
Thus equilibrium constant at unknown temperature is 0.36
Answer:
The question is incomplete as some details are missing. Here is the complete question ; A chemist adds 45.0mL of a 0.434M copper(II) sulfate CuSO4 solution to a reaction flask. Calculate the mass in grams of copper(II) sulfate the chemist has added to the flask. Round your answer to 2 significant digits
Explanation:
The step by step explanation is as shown in the attachment
