Question

Silane (SiH₄) is the silicon analogue of methane (CH₄). It is prepared industrially according to the following equations: Si(s) + 3HCl(g) → HSiCl3(l) + H₂(g) 4HSiCl3(l) → SiH₄(g) + 3SiCl4(l). a. If 156 mL of HSiCl3 (d = 1.34 g/mL) is isolated when 15.0 L of HCl at 10.0 atm and 35°C is used, what is the percent yield of HSiCl3? b. When 156 mL of HSiCl3 is heated, what volume of SiH₄ at 10.0 atm and 35°C will be obtained if the percent yield of the reaction is 93.1

Answer 1

To calculate percent yield, convert the actual yield to moles and compare it to the theoretical yield. To calculate the volume of SiH4 obtained, convert the given volume of HSiCl3 to moles and use the mole ratio from the balanced equation.

Step-by-step explanation:

To calculate the percent yield of HSiCl3, we need to determine the moles of HSiCl3 produced and compare it to the theoretical yield. First, we convert the given volume of HSiCl3 to grams using its density. Then, we convert grams of HSiCl3 to moles using its molar mass. Next, we calculate the moles of HCl used in the reaction using the ideal gas law. From the balanced equation, we determine the mole ratio between HCl and HSiCl3. Finally, we divide the actual yield by the theoretical yield and multiply by 100 to calculate the percent yield.

To calculate the volume of SiH4 obtained, we start by converting the given volume of HSiCl3 to moles using its molar mass. Next, we use the mole ratio from the balanced equation to determine the moles of SiH4 produced. Finally, we use the ideal gas law to calculate the volume of SiH4 at the given temperature and pressure.