Consider the following equation: CO + 2 H 2 → CH 3 OH △H rxn = -128 kJ

Calculate the amount of heat (in kJ) associated with complete reaction of 8.08 g H 2 .

You have 128 kJ heat released with 4*1.01 g hydrogen or 4.04 g hydrogen. So how much would be released with twice the amount of hydrogen?

To calculate the amount of heat associated with the complete reaction of 8.08 g H2, we need to use the molar ratio between H2 and the reaction. Here's how you can do it step by step:

Step 1: Calculate the number of moles of H2
To do this, we need to use the molar mass of H2, which is 2 g/mol. We can use the following formula to calculate the number of moles:

Number of moles = mass / molar mass

Number of moles of H2 = 8.08 g / 2 g/mol = 4.04 mol

Step 2: Determine the molar ratio between H2 and CH3OH
From the balanced equation, we can see that the stoichiometric coefficient of H2 is 2, which means that for every 2 moles of H2, we get 1 mole of CH3OH. Therefore, the molar ratio is 2:1.

Step 3: Calculate the amount of heat associated with the reaction
Now that we know the molar ratio, we can calculate the amount of heat associated with the reaction using the given value:

Amount of heat = Number of moles of H2 x ΔHrxn

Amount of heat = 4.04 mol x -128 kJ/mol = -517.12 kJ

Therefore, the amount of heat associated with the complete reaction of 8.08 g H2 is -517.12 kJ.