Write the equation for the decomposition of HI, knowing that the reaction requires 9.4 kj/mol of hydrogen forming. If 100.0 kj of energy are added, how many grams of iodine will form.

2HI ==> H2 + I2

9.4 kJ energy produces 2 g H2 AND 2*127 = 253.8 g I2. So 100 kJ will produce what?
2g H2 x 100/9.4 = ? g H2.
253.8 g I2 x 100/9.4 = ? g I2.

2700 gram

2700g

To write the equation for the decomposition of HI, we first need to know that HI stands for hydrogen iodide. The decomposition of HI can be represented by the following balanced chemical equation:

2HI(g) -> H2(g) + I2(g)

Now, let's move on to the second part of the question. Since the reaction requires 9.4 kJ/mol of hydrogen formed, we need to determine how many moles of hydrogen are involved in the reaction. To do this, we use the following conversion:

9.4 kJ/mol * (1 mol H2 / 2 mol HI) = 4.7 kJ/mol

This tells us that for every 4.7 kJ of energy input, one mole of hydrogen gas is formed.

Next, we calculate the number of moles of hydrogen formed using the given energy input of 100.0 kJ. We use the following conversion:

100.0 kJ * (1 mol H2 / 4.7 kJ) = 21.3 mol H2

Now that we know the number of moles of hydrogen formed, we can determine the number of moles of iodine formed by using the balanced chemical equation. From the equation, we can see that for every 2 moles of HI decomposed, 1 mole of iodine gas is formed.

Therefore, the number of moles of iodine formed is:

21.3 mol H2 * (1 mol I2 / 2 mol HI) = 10.65 mol I2

Finally, to calculate the mass of iodine formed, we can use the molar mass of iodine (I2), which is approximately 253.8 g/mol.

Mass of iodine formed = 10.65 mol I2 * 253.8 g/mol = 2704.17 g

Hence, approximately 2704.17 grams of iodine will form when 100.0 kJ of energy are added to the decomposition of HI.