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

`m_(HI)=860gHI\\\\Y=90.1\%`

Step-by-step 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*(1molH_2)/(2.02gH_2)* (2molHI)/(1molH_2)*(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=(775g)/(860g)*100\%\\\\Y=90.1\%`

Best regards!