Question

How many grams of HCL solution which is 73% by mass are needed to saturate 16.8 liters of propene at STP ?

Answer 1

Answer on Question #60182, Chemistry / General Chemistry

1. How many grams of HCL solution which is 73% by mass are needed to saturate 16.8 liters of propene at STP?

Solution:

$$\begin{array}{l} C_3H_6 + HCl = C_3H_7Cl \\ M(HCl) = 36.5 \text{ g/mol} \\ Vm = 22.4 \text{ L (STP)} \\ n = \frac{m}{M} = \frac{V}{Vm} \\ m(HCl) = \frac{V(C3H6) \times M(HCl)}{Vm} \\ m(HCl) = \frac{16.8 \times 36.5}{22.4} = 27.375\text{g} \\ \end{array}$$

Find mass of 73% HCL solution:

$$\omega = \frac{\text{mass of solute}}{\text{mass of solution}} \times 100\%$$

mass of solute – 27.375g.

$$\text{mass of solution} = \frac{\text{mass of solute}}{\omega} \times 100\% = \frac{27.35\text{g}}{73\%} \times 100\% = 37.465\text{g}$$

Answer: Need 37.465g of 73% HCl solution.

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