Question

according to the following reaction, how many grams of phosphoric acid will be formed upon the complete reaction of 22.8 grams of tetraphosphorus decaoxide with excess perchloric acid (hclo_4)? tetraphosphorus decaoxide (s) + perchloric acid (hclo_4) (aq) → phosphoric acid (aq) + dichlorine heptoxide (l) use the references to access important values if needed for this question. mass = g 9 more group attempts remaining submit answer retry entire group

Explanation:

Step1: Write the balanced chemical equation

$10HClO_4(aq)+P_4O_{10}(s)
ightarrow 4H_3PO_4(aq) + 5Cl_2O_7(l)$

Step2: Calculate the molar mass of $P_4O_{10}$

The molar mass of $P = 30.97\ g/mol$ and $O=16.00\ g/mol$. For $P_4O_{10}$, $M=(4\times30.97 + 10\times16.00)\ g/mol=283.88\ g/mol$

Step3: Calculate the number of moles of $P_4O_{10}$

Given mass of $P_4O_{10}=22.8\ g$. Using $n=\frac{m}{M}$, where $m = 22.8\ g$ and $M = 283.88\ g/mol$. So $n=\frac{22.8}{283.88}\ mol\approx0.0803\ mol$

Step4: Determine the mole - ratio of $P_4O_{10}$ to $H_3PO_4$

From the balanced equation, the mole - ratio of $P_4O_{10}$ to $H_3PO_4$ is $1:4$. So the number of moles of $H_3PO_4$ formed, $n_{H_3PO_4}=4\times n_{P_4O_{10}} = 4\times0.0803\ mol = 0.3212\ mol$

Step5: Calculate the molar mass of $H_3PO_4$

The molar mass of $H = 1.01\ g/mol$, $P = 30.97\ g/mol$ and $O = 16.00\ g/mol$. For $H_3PO_4$, $M=(3\times1.01+30.97 + 4\times16.00)\ g/mol = 97.99\ g/mol$

Step6: Calculate the mass of $H_3PO_4$

Using $m=n\times M$, where $n = 0.3212\ mol$ and $M = 97.99\ g/mol$. So $m=0.3212\times97.99\ g\approx31.5\ g$

Answer:

$31.5$