Calculate the Universal Gas Constant () to the correct number of significant figures if , given Avog — Mole Concept and Some Basic Concepts of Chemistry Chemistry Question
Question
Calculate the Universal Gas Constant ($R$) to the correct number of significant figures if $R = N_A \times k_B$, given Avogadro's number $N_A = 6.023 \times 10^{23} \text{ mol}^{-1}$ and Boltzmann's constant $k_B = 1.380 \times 10^{-23} \text{ J K}^{-1}$.
Answer: B
💡 Solution & Explanation
First, multiply the values: $(6.023 \times 10^{23}) \times (1.380 \times 10^{-23}) = 8.31174$. According to the rules of significant figures for multiplication, the final answer must have the same number of significant figures as the term with the fewest. Both $6.023$ and $1.380$ have 4 significant figures. Therefore, $8.31174$ rounded to 4 significant figures is $8.312$.
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