Chemistry, asked by WaniaTsiddiqui, 3 months ago

2.48 dm³ of N2 at STP weights

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Answered by humaidafridi18

Answer:

We know that, at standard temperature and pressure, 1 mole of any gas at STP contains 22.4 L of it. Therefore 11.5 liters of hydrogen(H2) is (1/22.4)*11.5 moles = 0.51 moles of hydrogen gas. We know that in 1 mole there is 6.022 × 10^23 molecules

Explanation:

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2.48 dm³ of N2 at STP weights​

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2.48 dm³ of N2 at STP weights