Question

mass of vinegar and cup (g) 484.81 g
mass of tablet (g) 3.22g
mass of vinegar, cup, and tablet - before reaction (g) 488.03g
mass after reaction (g) 487.04g
mass of co₂ (g) 0.99g

1. use the mass of co₂ from table 2 and the following balanced chemical equation to calculate the mass of nahco₃ in the tablet (the chemical equation simplifies nahco₃ to hco₃⁻ - use the molar mass of nahco₃ in your calculations). show your work for full credit.

1.89g

1. use your answer from question 4 as the experimental value to calculate the percent error (equation 1) for this experiment. assume that the reported amount of nahco₃ on the package (1.92 g) is the accepted value. show your work for full credit.

percent error = \frac{|experimental value - accepted value|}{accepted value}×100 equation 1

Explanation:

Step1: Recall percent - error formula

Percent Error=$\frac{\vert\text{experimental value}-\text{accepted value}\vert}{\text{accepted value}}\times100$

Step2: Identify values

The experimental value of $NaHCO_3$ from question 4 is $1.89$ g, and the accepted value is $1.92$ g.

Step3: Substitute values into formula

Percent Error=$\frac{\vert1.89 - 1.92\vert}{1.92}\times100$
First, calculate the numerator: $\vert1.89 - 1.92\vert=\vert- 0.03\vert = 0.03$
Then, $\frac{0.03}{1.92}\times100=\frac{3}{1.92}\approx1.56\%$

Answer:

$1.56\%$