Based on this reaction:
H2(g) + I2(g)= 2HI(g)
How many moles of iodine are necessary for form 0.530 moles of hydrogen iodine
Look at the equation. 1 mol I2 will produce 2 mols HI; therefore, 0.530 mols HI will require 1/2 that of I2.
To determine the number of moles of iodine necessary to form 0.530 moles of hydrogen iodine (HI), we can use the balanced equation and stoichiometry.
The balanced equation gives us a ratio between the number of moles of hydrogen (H2), iodine (I2), and hydrogen iodine (HI). From the equation:
H2(g) + I2(g) = 2HI(g)
We see that 1 mole of I2 reacts to form 2 moles of HI. Therefore, the stoichiometric ratio is 1 mole of I2 to 2 moles of HI.
Given that we want to calculate the moles of I2 required to form 0.530 moles of HI, we can set up a proportion using the stoichiometric ratio:
1 mole I2 / 2 moles HI = X moles I2 / 0.530 moles HI
Cross-multiplying the equation, we get:
0.530 moles HI * 1 mole I2 = 2 moles HI * X moles I2
Simplifying, we have:
X moles I2 = (0.530 moles HI * 1 mole I2) / 2 moles HI
Performing the calculation, we find:
X moles I2 = 0.265 moles I2
So, it takes 0.265 moles of iodine (I2) to form 0.530 moles of hydrogen iodine (HI).