Shanxian Chemical
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Density of Hydrogen at STP
On the density of hydrogen under standard conditions
If you want to know the density of hydrogen under standard conditions, you must know the relevant numbers. The standard conditions are specific temperature and pressure conditions, the temperature is 0 dollars ^ {\ circ} C $ (ie $273.15K $), the pressure is $101.325kPa $.
Hydrogen, the chemical formula is $H_ {2} $, the molar mass is about $2g/mol $. According to the ideal gas state equation $PV = nRT $ (where $P $is the pressure, $V $is the volume, $n $is the amount of substance, $R $is the molar gas constant, and $T $is the temperature), we can get $n =\ frac {m} {M} $ ($m $is the mass, $M $is the molar mass).
Let the mass of hydrogen be $m $and the amount of substance be $n $, then $n =\ frac {m} {2g/mol} $. In the standard case, by substituting $P = 101.325kPa $, $T = 273.15K $, $R = 8.314J/(mol\ cdot K) $into the ideal gas equation of state, we can obtain $V =\ frac {nRT} {P} $.
Because of the density $\ rho =\ frac {m} {V} $, substitute $n =\ frac {m} {2g/mol} $into $V =\ frac {nRT} {P} $, and get $V =\ frac {mRT} {2g/mol\ cdot P} $, then $\ rho =\ frac {m} {\ frac {mRT} {2g/mol\ cdot P}} =\ frac {2g/mol\ cdot P} {RT} $.
Substitute the values under standard conditions, that is, $P = 101.325kPa $, $T = 273.15K $, $R = 8.314J/(mol\ cdot K) $, and the density of hydrogen under standard conditions is calculated to be about $0.0899g/L $.
From this, it can be seen that under standard conditions, the density of hydrogen is small, which makes it unique in many fields and is important for research and application in the world.
If you want to know the density of hydrogen under standard conditions, you must know the relevant numbers. The standard conditions are specific temperature and pressure conditions, the temperature is 0 dollars ^ {\ circ} C $ (ie $273.15K $), the pressure is $101.325kPa $.
Hydrogen, the chemical formula is $H_ {2} $, the molar mass is about $2g/mol $. According to the ideal gas state equation $PV = nRT $ (where $P $is the pressure, $V $is the volume, $n $is the amount of substance, $R $is the molar gas constant, and $T $is the temperature), we can get $n =\ frac {m} {M} $ ($m $is the mass, $M $is the molar mass).
Let the mass of hydrogen be $m $and the amount of substance be $n $, then $n =\ frac {m} {2g/mol} $. In the standard case, by substituting $P = 101.325kPa $, $T = 273.15K $, $R = 8.314J/(mol\ cdot K) $into the ideal gas equation of state, we can obtain $V =\ frac {nRT} {P} $.
Because of the density $\ rho =\ frac {m} {V} $, substitute $n =\ frac {m} {2g/mol} $into $V =\ frac {nRT} {P} $, and get $V =\ frac {mRT} {2g/mol\ cdot P} $, then $\ rho =\ frac {m} {\ frac {mRT} {2g/mol\ cdot P}} =\ frac {2g/mol\ cdot P} {RT} $.
Substitute the values under standard conditions, that is, $P = 101.325kPa $, $T = 273.15K $, $R = 8.314J/(mol\ cdot K) $, and the density of hydrogen under standard conditions is calculated to be about $0.0899g/L $.
From this, it can be seen that under standard conditions, the density of hydrogen is small, which makes it unique in many fields and is important for research and application in the world.
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