given:
25.9 kJ + 1/2 H2 + 1/2 I2 => HI
how much energy is needed for the reaction of 4.57x10^24 molecules of iodine, I2, with excess hydrogen, H2?
mols I2 = 4.57E24/6.02E23 = 7.59
Atoms I = 7.59/2 = about 3.8 but you need to do it more accurately.
The equation tells you that it takes 25.9 kJ for 1 mol I atoms. You have 3.8 mols I.
25.9 kJ x 3.8 = ?
To determine the amount of energy needed for the reaction of 4.57x10^24 molecules of iodine (I2) with excess hydrogen (H2), we need to use the given energy change for the reaction.
In this case, the given energy change is 25.9 kJ for 1 mole of the reaction. So, we first need to convert the given amount of molecules of iodine (I2) into moles.
We know that 1 mole of a substance contains 6.022x10^23 molecules. Therefore, we can calculate the number of moles of iodine (I2) using the following conversion:
Moles of I2 = Number of molecules of I2 / Avogadro's number (6.022x10^23 molecules/mol)
Moles of I2 = 4.57x10^24 molecules / 6.022x10^23 molecules/mol
Now, we can find the energy change for the given number of moles of iodine (I2) using stoichiometry. According to the balanced equation:
25.9 kJ + 1/2 H2 + 1/2 I2 => HI
From the equation, we can see that 1 mole of iodine (I2) requires 25.9 kJ of energy. Therefore, we can set up a proportion to find the energy change for the given number of moles:
Energy change for the given moles of I2 / Moles of I2 = Energy change for 1 mole of I2 / 1 mole of I2
Now, substituting the values in:
Energy change for the given moles of I2 / (4.57x10^24 molecules / 6.022x10^23 molecules/mol) = 25.9 kJ / 1 mole of I2
Simplifying the equation:
Energy change for the given moles of I2 = (4.57x10^24 molecules / 6.022x10^23 molecules/mol) * 25.9 kJ
Finally, calculating the value:
Energy change for the given moles of I2 = 4.57x10^24 molecules * 25.9 kJ / 6.022x10^23 molecules/mol
Now, calculate the result to find how much energy is needed for the reaction of 4.57x10^24 molecules of iodine (I2) with excess hydrogen (H2).