In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following balanced chemical equation: Pcl5(s)+4H2O(l) ---> H3PO4 (aq) + 5HCl (g) The molar masses for each compound in the equation are as follows; PCl5: 208.224 g/mol H2O: 18.015 g/mol H3PO4: 97.994 g/mol HCl; 36.45 g/mol What is the limiting reagent in this scenario? The answer given to me was: From, the above equation, it is observed that 1 mole of PCl5 is reacted with 4 moles of H2O. Then, 0.058 moles of PCl5 are reacted with 0.058 mol/1 mol × 4 mol= 0.232 moles of H2O. But the actual number of moles of water available is 0.833 mol. So, in this chemical reaction, water is available in excess amount and PCl5 is present in a lesser amount. So, all the PCl5 is consumed in this reaction, as it is present in less amount compared to the other reactant. And, hence, the limiting reagent is PCl5. Now, the excess amount of water is = (0.833 - 0.232) mol = 0.601 mol. Could you elaborate on the answer? What is canceling out that dimensional analysis conversion factor for 4x0.058mol /1 mol? Could you label them with units?
In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following balanced chemical equation:
Pcl5(s)+4H2O(l) ---> H3PO4 (aq) + 5HCl (g)
The molar masses for each compound in the equation are as follows;
PCl5: 208.224 g/mol
H2O: 18.015 g/mol
H3PO4: 97.994 g/mol
HCl; 36.45 g/mol
What is the limiting reagent in this scenario?
The answer given to me was:
From, the above equation, it is observed that 1 mole of PCl5 is reacted with 4 moles of H2O.
Then, 0.058 moles of PCl5 are reacted with
0.058 mol/1 mol × 4 mol= 0.232 moles of H2O.
But the actual number of moles of water available is 0.833 mol. So, in this
Could you elaborate on the answer? What is canceling out that dimensional analysis conversion factor for 4x0.058mol /1 mol? Could you label them with units?
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