You run an experiment according to this equation: 2HCl+CaCO_(3)arrow H_(2)O+CaCl_(2) +CO_(2) When running your lab you started with 62 .16 grams of HCl and 50.18 grams of CaCO_(3) If, after the reaction finishes, your products have a total mass of 80.10, what was the percent yield? Round your answer to the nearest 0.01 and include units! Your Answer: square square Answer units

Question

You run an experiment according to this equation: 2HCl+CaCO_(3)arrow H_(2)O+CaCl_(2) +CO_(2) When running your lab you started with 62 .16 grams of HCl and 50.18 grams of CaCO_(3) If, after the reaction finishes, your products have a total mass of 80.10, what was the percent yield? Round your answer to the nearest 0.01 and include units! Your Answer: square square Answer units

Answer 1

### 71.31%

Answer 2

## Step1: Calculate the Molar Masses### Determine the molar masses of

and

using their atomic weights.-

:

-

:

## Step2: Calculate Moles of Reactants### Convert the given masses of

and

to moles.- Moles of

:

- Moles of

:

## Step3: Determine Limiting Reactant### Identify the limiting reactant by comparing the mole ratio from the balanced equation.- The balanced equation shows a 2:1 ratio of

to

.- Required moles of

for 0.501 mol of

:

- Since we have 1.705 mol of

,

is the limiting reactant.## Step4: Calculate Theoretical Yield### Use the limiting reactant to calculate the theoretical yield of products.- Total mass of reactants:

- Theoretical mass of products (should be equal to total mass of reactants):

## Step5: Calculate Percent Yield### Compare the actual mass of products to the theoretical mass to find the percent yield.- Actual mass of products:

- Percent yield:

Problemas

Roztwór

Respuesta

Explicación