Hello, I really don't understand how to find the grams of moles in some of these reactions. If someone could help I would appreciate it.
1) Balance the following chemical reaction and determine the number of moles of HI produced when 2.33 moles of H2(g) are consumed in the following chemical reaction:
___H2(g) + __I2(g) → ___HI (g)
(I know the balanced equation for this reaction is H2 + I2 → 2HI)
I worked this exact problem above.
To find the number of moles of HI produced when 2.33 moles of H2(g) are consumed, we need to use stoichiometry, which is a way to relate the ratios of moles of different substances in a balanced chemical equation.
Given that the balanced equation for the reaction is H2 + I2 → 2HI, we can see that for every 1 mole of H2 consumed, we get 2 moles of HI produced.
Now, let's set up a proportion to solve for the moles of HI produced. We can use the following setup:
(2 moles of HI / 1 mole of H2) = (x moles of HI / 2.33 moles of H2)
To solve for x (the moles of HI), we can cross-multiply and divide:
2 moles of HI * 2.33 moles of H2 = x moles of HI * 1 mole of H2
x moles of HI = (2 moles of HI * 2.33 moles of H2) / 1 mole of H2
Simplifying the equation gives us:
x = 4.66 moles of HI
Therefore, when 2.33 moles of H2(g) are consumed, 4.66 moles of HI are produced.
Remember, stoichiometry is a useful tool to calculate the amount of reactants or products in a chemical reaction based on their balanced equation.