Consider the following equation: CO + 2 H2 → CH3OH ΔH rxn = -128 kJ

Calculate the amount of heat (in kJ) associated with complete reaction of 8.08 g H2.

How would u set that up?

The same way that I showed you how to do the other one, but just convert 8.08g of H2 to moles:

8.08g of H2*(1 mole/2.02g)=??? moles

Thank you I guess i forgot to convert

To calculate the amount of heat associated with the complete reaction of 8.08 g of H2, we need to use the given reaction's stoichiometry and the molar mass of H2. Here's how you can set up the calculation step-by-step:

Step 1: Determine the molar mass of H2
The molar mass of H2 is 2 g/mol, as hydrogen has an atomic mass of approximately 1 g/mol, and there are two hydrogen atoms in H2.

Step 2: Convert the mass of H2 to moles
Using the molar mass calculated in the previous step, divide the mass of H2 (8.08 g) by its molar mass to obtain the number of moles of H2:
8.08 g H2 * (1 mol H2 / 2 g H2) = 4.04 mol H2

Step 3: Determine the heat associated with the reaction of 1 mole of H2
From the balanced equation, we see that the reaction produces 1 mole of CH3OH and has a heat change of -128 kJ. So, -128 kJ of heat is associated with the reaction of 1 mole of H2.

Step 4: Calculate the amount of heat for the given amount of H2
Multiply the moles of H2 (4.04 mol) by the heat associated with 1 mole of H2 (-128 kJ/mol):
4.04 mol H2 * (-128 kJ/mol) = -518.72 kJ

Therefore, the amount of heat associated with the complete reaction of 8.08 g of H2 is approximately -518.72 kJ. Note that the negative sign indicates that the reaction is exothermic, meaning it releases heat.

To calculate the amount of heat associated with the complete reaction of 8.08 g H2, we can use the given equation and the concept of molar ratios.

Step 1: Determine the molar mass of H2.
The molar mass of H2 is 2 g/mol (1 hydrogen atom weighs approximately 1 g/mol, and there are 2 hydrogen atoms in H2).

Step 2: Convert the mass of H2 to moles.
Use the following formula:
moles = mass (in grams) / molar mass (in g/mol)

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

Step 3: Use the stoichiometric coefficients to determine the moles of the other species in the equation.
From the balanced equation, we can see that the ratio between H2 and CH3OH is 2:1. Therefore, if we have 4.04 moles of H2, we will have half as many moles of CH3OH.

moles of CH3OH = 4.04 mol / 2 = 2.02 mol

Step 4: Calculate the heat associated with the reaction using the given ΔH value.
The ΔH value given is -128 kJ for the reaction of 1 mole of CH3OH. Therefore, to calculate the heat associated with 2.02 moles of CH3OH, we can use a proportion:

( ΔH / moles of CH3OH ) = ( -128 kJ / 1 mol )

ΔH = ( -128 kJ / 1 mol ) * 2.02 mol
= -258.56 kJ (rounded to two decimal places)

Therefore, the amount of heat associated with the complete reaction of 8.08 g H2 is approximately -258.56 kJ.