Answer:
60.0L of hydrogen are needed
Explanation:
Based on the reaction:
3H₂ + N₂ ⇄ 2NH₃
<em>3 moles of hydrogen react 1 mole of nitrogen.</em>
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To solve this question we have to find the moles of nitrogen. With the moles of nitrogen we can find the moles of hydrogen. Using PV = nRT at STP conditions we can find the volume as follows:
<em>Moles Nitrogen -Molar mass: 28g/mol-</em>
25.0g N₂ * (1mol / 28g) = 0.893 moles N₂
<em>Moles hydrogen: </em>
0.893 moles N₂ * (3mol H₂ / 1mol N₂) = 2.679 moles H₂
<em>Volume hydrogen:</em>
PV = nRT
V = nRT / P
<em>Where V is volume in liters,</em>
<em>n are moles of the gas: 2.679 moles</em>
<em>R is gas constant: 0.082atmL/molK</em>
<em>T is absolute temperature: 273.15K at STP</em>
<em>P is 1atm at STP</em>
Replacing:
V = 2.679mol*0.082atmL/molK*273.15K / 1atm
V =
<h3>60.0L of hydrogen are needed</h3>
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