Answer:
* Limiting reagent: potassium.
*
Explanation:
Hello,
In this case, the undergoing chemical reaction is:
In such a way, the reacting moles of chlorine are:
Now, the amount of chlorine gas that would react with 5.00 g of potassium result:
Thus, the chlorine will be in excess and the potassium will be the limiting reagent. Therefore, the mass of excess chlorine turns out:
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Answer:
Explanation:
Hello there!
In this case, according to the given chemical reaction at equilibrium, we can set up the equilibrium expression as follows:
Which can be written in terms of x, according to the ICE table:
Thus, we solve for x to obtain that it has a value of 0.01436 M and therefore, the concentrations at equilibrium turn out to be:
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Answer:
Explanation:
Hello.
In this case, since the acid is monoprotic and the KOH has one hydroxyl ion only, we can see that at the equivalence point the moles of both of them are the same:
Thus, since we are given 1.70 g of the acid, we compute the moles of acid that were titrated:
Which equal the moles of KOH. In such a way, since the molarity is defined as moles over liters (M=n/V), the liters are moles over molarity (V=n/M), thus, the resulting volume is:
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