Question

calculate the mass of 3.011x10^23 atoms of nitrogen

Answer 1

$\Longrightarrow{\boxed{\bold{Answer: 7\:gram}}}$

$\textbf{\underline{Step-by-step explanation :- }}$

Since we know that,

Atomic mass of Nitrogen = 14 g/mol

Then 1 mole of Nitrogen weighs = 14 g

Now, 1 mole = 6.022 × 10²³ atoms

6.022 × 10²³ atoms of N weighs = 14 g

1 atom of N weighs = 14/6.022 × 10²³

Then 3.011 × 10²³ atoms will weigh

= ( 14/6.022 × 10²³ ) × 3.011 × 10²³ g =

$\bold{\huge{ \frac{14}{2} g = 7\:gram}}$

Answer 2

$\huge\underline\mathfrak{Answer}$


7gram


$\huge\underline\mathfrak{Solution}$



$\textbf{Step-By-Step-Solution}$


$\textbf{Step 1}$


Mass of N(2) molecules = 14grams


According to A avagadero rule



$\textbf{Therefore}[tex], 14g of nitrogen = 6.022×[tex]{10}{23}$atom


$mass \: \: of \: 1 \: atom = \frac{14}{6.022 \times {10}^{23}}$



$\textbf{Step 2}$





$mass \: of \: 3.011 \times {10}^{23}$




$= \frac{14}{6.022 \times {10}^{23} } \times 3.011 \times {10}^{23}$


$= \frac{14}{2}$

$= 7gram$

$\huge\underline\mathfrak{Hence}$


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The mass of 3.011x10^23 atoms of nitrogen is $\textbf{7gram}$