Based on the following chemical equation, answer the questions below. Show all your calculation
The balanced chemical reaction of iodine with hydrogen sulfide is as follows:
H2S(g)+I2(s)-----2HI(g) + S(s)
(a) Based on the above chemically balanced equation, how many grams of HI should be produced from the reaction of 25.0g of H2S when there is excess amount of I2?
(b) Actually 30.0g of HI is produced in this reaction, what is the percent yield of HI?
a. mols H2S = grams/molar mass
Use the coefficients in the balanced equation to convert mols H2S to mols HI. That will be ?mols H2S x (2 mols HI/1 mol H2S) = ?mols H2S x 2/1 = ? mols HI
Then convert mols HI to grams HI. grams = mols x molar mass. This is the theoretical yield (TY).
b. Actual yield (AY) is 30.0 g.
%yield = (AY/TY)*100 = ?
To solve these problems, we'll use stoichiometry, which is a method used in chemistry to relate the number of moles and masses of substances involved in a chemical reaction. Here's how we can find the answers to both questions:
(a) Based on the balanced equation, we can see that 1 mole of H2S reacts with 1 mole of I2 to produce 2 moles of HI. We can use this ratio to convert the given amount of H2S to HI.
Step 1: Convert grams of H2S to moles of H2S.
Given:
Mass of H2S = 25.0 g
Molar mass of H2S = 34.08 g/mol
Using the formula:
moles = mass / molar mass
moles of H2S = 25.0 g / 34.08 g/mol
Step 2: Use the stoichiometric ratio to convert moles of H2S to moles of HI.
From the balanced equation, we can see that the ratio of moles of H2S to moles of HI is 1:2.
moles of HI = moles of H2S * (2 moles of HI / 1 mole of H2S)
Step 3: Convert moles of HI to grams of HI.
Given:
Molar mass of HI = 127.91 g/mol
Using the formula:
mass = moles * molar mass
mass of HI = moles of HI * 127.91 g/mol
By substituting the calculated value of moles of H2S into this equation, we can find the mass of HI produced.
(b) To calculate the percent yield of HI, we need the actual yield and the theoretical yield. Theoretical yield refers to the calculated value from the balanced equation, whereas the actual yield is the given value of 30.0 g.
The percent yield can be calculated using the formula:
Percent Yield = (Actual Yield / Theoretical Yield) * 100
To find the theoretical yield:
Using the balanced equation, we can determine the stoichiometric ratio between H2S and HI (2:1). Therefore, the theoretical yield of HI is half the moles of H2S calculated in part (a).
Now, you can perform these calculations by substituting the values in the respective equations to find the answers to both questions.