Question

Calculate the number of molecules present in 11.5 dm3 of N2 at STP

Answer 1

Answer:

• At standard temperature and pressure

1 mole of any gas at STP contains → 22.4 liters

11.5 liters of hydrogen (H2) contains → $</strong><strong>\</strong><strong>r</strong><strong>e</strong><strong>d</strong><strong>{</strong><strong>( \frac{1}{22.4} )</strong><strong>}</strong><strong> \times </strong><strong>\</strong><strong>r</strong><strong>e</strong><strong>d</strong><strong>{</strong><strong>(11.5)</strong><strong>}</strong><strong> \: \: </strong><strong>\</strong><strong>b</strong><strong>l</strong><strong>u</strong><strong>e</strong><strong>{</strong><strong>moles</strong><strong>}</strong><strong>$

=> 0.51 moles of hydrogen gas

1 mole contains → $</strong><strong>\</strong><strong>p</strong><strong>i</strong><strong>n</strong><strong>k</strong><strong>{</strong><strong>(6.022</strong><strong> \: \: \times {10}^{23} )</strong><strong>}</strong><strong> \: \: </strong><strong>\</strong><strong>g</strong><strong>r</strong><strong>e</strong><strong>e</strong><strong>n</strong><strong>{</strong><strong>molecules</strong><strong>}</strong><strong>$

Answer 2

Answer:

At standard temperature and pressure

1 mole of any gas at STP contains → 22.4 liters

11.5 liters of hydrogen (H2) contains → [tex]( \frac{1}{22.4} ) \times (11.5) \: \: {moles

→ ( 22.4)×(11.5) moles

=> 0.51 moles of hydrogen gas

1 mole contains → ( 6.022 × 10^23 ) molecules

→ (6.022×10^23) molecules