The value of Avogadro's number is $6.02214076 imes 10^{23}$. For a calculation requiring only three significant figures, what value of Avogadro's number should be used?

A student has measured the length of a wire equal to 0.04580 m. This value of length has the number of significant figures equal to

The value of Avogadro's number is $6.02214076 imes 10^{23}$. For a calculation requiring only three significant figures, what value of Avogadro's number should be used?

The respective number of significant figures for the numbers 23.023, 0.0003 and $2.1 imes {10^{ - 3}}$ are

In the context of accuracy of measurement and significant figures in expressing results of experiment, which of the following is/are correct

(1) Out of the two measurements 50.14 cm and 0.00025 ampere, the first one has greater accuracy

(2) If one travels 478 km by rail and 397 m by road, the total distance travelled is 478 km

The mass of a sample is measured as 23.647 g. If the instrument used has a precision of 0.01 g, what is the correctly rounded mass?

If $x = 4.99$ and $y = 0.0099$, what is $x + y$ to the correct number of significant figures?

A student measures two lengths as $2.99$ m and $0.0099$ m. What is the sum of these lengths, taking into account significant figures?

What is the result of $99.9 + 0.099$ when considering significant figures?

A student performs a titration and calculates the concentration of a solution to be $0.1234567$ M. The burette used has a precision of $\pm 0.02$ mL, and the volumetric flask used to prepare the solution has a precision of $\pm 0.1$ mL. Which is the most accurate way to report the concentration, considering significant figures and uncertainty?

A chemist measures the volume of a solution as 25.34 mL using a burette with a precision of ±0.02 mL. They then dilute this solution to a final volume of 250.0 mL using a volumetric flask with a precision of ±0.1 mL. What is the absolute uncertainty in the final concentration of the diluted solution?