P_(4)+6Cl_(2)arrow 4PCl_(3) reaction of 75.0g P_(4) with excess chlorine gas produces 110g PCl_(3) In lab. Find the theoretical yield and calc percent yield for the reaction. 78% 64% 27% 33%

To find the theoretical yield and percent yield for the reaction, we need to follow these steps:<br /><br />1. Calculate the molar mass of $P_{4}$ and $PCl_{3}$.<br />2. Convert the given mass of $P_{4}$ to moles.<br />3. Use the stoichiometry of the balanced equation to find the moles of $PCl_{3}$ produced.<br />4. Convert the moles of $PCl_{3}$ to grams to find the theoretical yield.<br />5. Calculate the percent yield using the given actual yield.<br /><br />Step 1: Calculate the molar mass of $P_{4}$ and $PCl_{3}$.<br />Molar mass of $P_{4}$ = 4 * 30.97 g/mol = 123.88 g/mol<br />Molar mass of $PCl_{3}$ = 30.97 g/mol (P) + 3 * 35.45 g/mol (Cl) = 137.32 g/mol<br /><br />Step 2: Convert the given mass of $P_{4}$ to moles.<br />Moles of $P_{4}$ = 75.0 g / 123.88 g/mol = 0.605 mol<br /><br />Step 3: Use the stoichiometry of the balanced equation to find the moles of $PCl_{3}$ produced.<br />According to the balanced equation, 1 mole of $P_{4}$ produces 4 moles of $PCl_{3}$.<br />Moles of $PCl_{3}$ produced = 0.605 mol $P_{4}$ * 4 = 2.42 mol $PCl_{3}$<br /><br />Step 4: Convert the moles of $PCl_{3}$ to grams to find the theoretical yield.<br />Theoretical yield of $PCl_{3}$ = 2.42 mol * 137.32 g/mol = 332.5 g<br /><br />Step 5: Calculate the percent yield using the given actual yield.<br />Percent yield = (Actual yield / Theoretical yield) * 100<br />Percent yield = (110 g / 332.5 g) * 100 = 33.1%<br /><br />Therefore, the theoretical yield is 332.5 g and the percent yield is 33.1%.