Question

you measure the products of a chemical reaction to be 0.56 g, 0.59 g, and 0.60 g. the actual mass is 2.62 g.
you measure the products of a chemical reaction to be 10.15 g, 10.16 g, and 10.13 g. the actual mass is 10.14 g.
you measure the products of a chemical reaction to be 5.22 g, 4.35 g, and 5.89 g. the actual mass is 3.35 g.

Explanation:

Step1: Define accuracy and precision

Accuracy is closeness to true - value. Precision is closeness of measurements to each other.

Step2: Analyze first set of measurements (0.56 g, 0.59 g, 0.60 g; actual 2.62 g)

The measured values are close to each other (precision), but far from the actual value (not accurate).

Step3: Analyze second set of measurements (10.15 g, 10.16 g, 10.13 g; actual 10.14 g)

The measured values are close to each other (precision) and close to the actual value (accuracy).

Step4: Analyze third set of measurements (5.22 g, 4.35 g, 5.89 g; actual 3.35 g)

The measured values are not close to each other (not precise) and far from the actual value (not accurate).

Answer:

1. precise but not accurate
2. both accurate and precise
3. neither accurate nor precise