Math  /  Numbers & Operations

Question50. What volume will 0.5 g of H2\mathrm{H}_{2} accupy at s.t.p.? [H=1[H=1 \text {. }

Studdy Solution

STEP 1

1. Standard temperature and pressure (s.t.p.) are defined as 0C0^\circ C (273.15 K) and 1 atm pressure.
2. At s.t.p., 1 mole of an ideal gas occupies 22.4 liters.
3. The molar mass of hydrogen (H2\mathrm{H}_{2}) is 2g/mol2 \, \text{g/mol}.

STEP 2

1. Calculate the number of moles of H2\mathrm{H}_{2}.
2. Use the ideal gas law to find the volume at s.t.p.

STEP 3

Calculate the number of moles of H2\mathrm{H}_{2} using its molar mass.
Number of moles=massmolar mass=0.5g2g/mol\text{Number of moles} = \frac{\text{mass}}{\text{molar mass}} = \frac{0.5 \, \text{g}}{2 \, \text{g/mol}}

STEP 4

Perform the division to find the number of moles.
Number of moles=0.25mol\text{Number of moles} = 0.25 \, \text{mol}

STEP 5

Use the volume of 1 mole of gas at s.t.p. to find the volume of 0.25 moles.
Volume=Number of moles×Volume of 1 mole at s.t.p.\text{Volume} = \text{Number of moles} \times \text{Volume of 1 mole at s.t.p.} $\text{Volume} = 0.25 \, \text{mol} \times 22.4 \, \text{L/mol

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