A sample of a compound used to polish dentures and as a nutrient and dietary supplement is analyzed and found to contain 9.0231
1 answer:
Answer:
Explanation:
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In this case, since the determination of empirical formulas requires the moles of the constituents, we first need to calculate the moles in the given grams of the listed elements:
Next, we divide each moles by the fewest moles, in this case, those of phosphorous, in order to determine their subscripts in the empirical formula:
Thus, we multiply these subscripts by 5 to get whole numbers:
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Answer :
The equilibrium concentration of CO is, 0.016 M
The equilibrium concentration of Cl₂ is, 0.034 M
The equilibrium concentration of COCl₂ is, 0.139 M
Explanation :
The given chemical reaction is:
Initial conc. 0.1550 0.173 0
At eqm. (0.1550-x) (0.173-x) x
As we are given:
The expression for equilibrium constant is:
Now put all the given values in this expression, we get:
x = 0.139 and x = 0.193
We are neglecting value of x = 0.193 because equilibrium concentration can not be more than initial concentration.
Thus, we are taking value of x = 0.139
The equilibrium concentration of CO = (0.1550-x) = (0.1550-0.139) = 0.016 M
The equilibrium concentration of Cl₂ = (0.173-x) = (0.173-0.139) = 0.034 M
The equilibrium concentration of COCl₂ = x = 0.139 M