The reaction
Fe + Br2 ---> FeBr2 Delta H = -249.8kJ
Calculate delta H when 10.0 g of FeBr2 is formed.
Ahh, that makes a lot of sense. Thanks.
To calculate the value of ∆H when 10.0 g of FeBr2 is formed, you need to use the given value of ∆H for the reaction and use it to find the quantity of heat released or absorbed per gram of FeBr2 formed.
The given value of ∆H is -249.8 kJ, which represents the heat released or absorbed per 1 mole of FeBr2 formed.
To calculate the quantity of FeBr2 formed when 10.0 g of FeBr2 is produced, you need to determine the number of moles of FeBr2.
Step 1: Find the molar mass of FeBr2.
The molar mass of Fe is approximately 55.85 g/mol, and the molar mass of Br is approximately 79.90 g/mol. Since FeBr2 contains one Fe atom and two Br atoms, the molar mass of FeBr2 is:
Molar mass of FeBr2 = (1 x molar mass of Fe) + (2 x molar mass of Br)
Step 2: Calculate the number of moles of FeBr2.
Moles of FeBr2 = Mass of FeBr2 / Molar mass of FeBr2
Step 3: Calculate ∆H for 10.0 g of FeBr2 formed.
∆H = (∆H per mole of FeBr2) x (moles of FeBr2)
Now, let's proceed with the calculations.
Step 1: Find the molar mass of FeBr2.
Molar mass of Fe = 55.85 g/mol
Molar mass of Br2 = 2 x 79.90 g/mol = 159.80 g/mol
Molar mass of FeBr2 = 55.85 g/mol + 159.80 g/mol = 215.65 g/mol
Step 2: Calculate the number of moles of FeBr2.
Moles of FeBr2 = 10.0 g / 215.65 g/mol
Step 3: Calculate ∆H for 10.0 g of FeBr2 formed.
∆H = -249.8 kJ/mol x (moles of FeBr2)
Now, substitute the value of moles of FeBr2 obtained in step 2 to calculate the final answer.