Question

For the following reaction, 6.79 grams of hydrogen gas are mixed with excess iodine . The reaction yields 775 grams of hydrogen iodide . hydrogen ( g ) iodine ( s ) hydrogen iodide ( g ) What is the theoretical yield of hydrogen iodide

Answer 1

Answer:

$m_{HI}=860gHI\\\\Y=90.1\%$

Explanation:

Hello.

In this case, for the reaction:

$H_2+I_2\rightarrow 2HI$

As 6.79 g of hydrogen (molar mass = 2.02 g/mol) react in excess iodine, we can compute the theoretical yield of hydrogen iodide (molar mass = 127.91 g/mol)  via their 1:2 mole ratio shown on the chemical reaction:

$m_{HI}=6.79gH_2*\frac{1molH_2}{2.02gH_2}* \frac{2molHI}{1molH_2}*\frac{127.91gHI}{1molHI}\\\\m_{HI}=860gHI$

Next, we compute the percent yield by divinding the actual yield (775 g) by the theoretical yield (860 g):

$Y=\frac{775g}{860g}*100\%\\\\Y=90.1\%$

Best regards!