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)
H2(g) + I2(g) -> 2HI (g)
2.33 mols H2 x (2 mol HI/1 mol H2) = 2.33 x 2/1 = ? mols HI
Why did the chemist break up with the biologist? Because there was no chemical reaction between them!
Now, let's balance this reaction and solve for the number of moles of HI produced when 2.33 moles of H2 are consumed.
Well, first off, we notice that we have an uneven number of hydrogens on both sides of the equation, so let's start there. We need 2 hydrogens on the left side to match the 2 hydrogens in HI on the right side. Therefore, the balanced equation is:
H2(g) + I2(g) -> 2HI(g)
Now, we can see that the mole ratio of H2 to HI is 1:2. So, if we have 2.33 moles of H2, we would expect to produce twice that amount of HI. Hence, the number of moles of HI produced would be 2 times 2.33, which is 4.66 moles.
Remember, though, chemistry can sometimes be irrational, so don't take my word for it. Double-check your calculations!
To balance the chemical equation, follow these steps:
1. Count the number of atoms of each element on both sides of the equation.
On the left side:
- Hydrogen atoms: 2
- Iodine atoms: 2
On the right side:
- Hydrogen atoms: 1
- Iodine atoms: 1
2. Balance the iodine atoms by placing a coefficient in front of the iodine molecules on the left side.
The equation now becomes:
___H2(g) + __I2(g) -> ___HI(g)
3. Balance the hydrogen atoms by placing a coefficient in front of the hydrogen molecules on the right side.
The equation becomes:
___H2(g) + __I2(g) -> 2HI(g)
4. The equation is now balanced, with 2 moles of HI produced for every 1 mole of I2 consumed.
To determine the number of moles of HI produced when 2.33 moles of H2(g) are consumed, use the ratio of coefficients from the balanced equation.
- The coefficient for H2 is 1, and the coefficient for HI is 2.
- Since the coefficients are in a 1:2 ratio, the number of moles of HI produced will also be 2 times greater than the number of moles of H2 consumed.
Therefore, when 2.33 moles of H2 are consumed, the number of moles of HI produced is 2.33 * 2 = 4.66 moles of HI.
To balance the chemical equation:
H2(g) + I2(g) -> 2HI(g)
The balanced equation indicates that 1 mole of H2 reacts with 1 mole of I2 to produce 2 moles of HI.
To determine the number of moles of HI produced when 2.33 moles of H2 are consumed, we use the ratio of H2 to HI from the balanced equation.
Given: 2.33 moles H2
From the balanced equation: 1 mole H2 produces 2 moles HI
Using the ratio, we can set up a proportion to find the number of moles of HI produced:
(2.33 moles H2) * (2 moles HI / 1 mole H2) = 4.66 moles HI
Therefore, 2.33 moles of H2 will produce 4.66 moles of HI.