Respuesta :
Answer is: rate of production of hydrogen is 0,01758 kg/s.
Chemical reaction: CH₄ + H₂O → CO + 3H₂.
V(CH₄) = 159 L.
p = 0,86 atm · 101,325 kPa/atm = 87,14 kPa.
T = 294°C = 567 K.
R = 8,314 J/K·mol.
Ideal gas law: p·V = n·R·T.
n(CH₄) = p·V ÷ R·T.
n(CH₄) = 87,14 kPa · 159 L ÷ 8,314 J/K·mol · 567 K.
n(CH₄) = 2,93 mol.
From chemical reaction: n(CH₄) : n(H₂) = 1 : 3.
n(H₂) = 2,93 mol · 3 = 8,79 mol.
m(H₂) = 8,79 mol · 2 g/mol.
m(H₂) = 17,58 g · 0,001 kg/g = 0,01758 kg.
Chemical reaction: CH₄ + H₂O → CO + 3H₂.
V(CH₄) = 159 L.
p = 0,86 atm · 101,325 kPa/atm = 87,14 kPa.
T = 294°C = 567 K.
R = 8,314 J/K·mol.
Ideal gas law: p·V = n·R·T.
n(CH₄) = p·V ÷ R·T.
n(CH₄) = 87,14 kPa · 159 L ÷ 8,314 J/K·mol · 567 K.
n(CH₄) = 2,93 mol.
From chemical reaction: n(CH₄) : n(H₂) = 1 : 3.
n(H₂) = 2,93 mol · 3 = 8,79 mol.
m(H₂) = 8,79 mol · 2 g/mol.
m(H₂) = 17,58 g · 0,001 kg/g = 0,01758 kg.
The rate of the dihydrogen production is 0.0175 kg/sec for the given reaction.
The given reaction
[tex]\bold {CH_4 + H_2O \rightarrow CO + 3H_2}[/tex]
One mole of Methane is react with one mole of water to form 1 mole of CO and 3 moles of Hydrogen.
The rate of hydrogen production can be calculated from ideal gas law
[tex]\bold {pV = nRT}[/tex]
Where,
p- pressure = 0,86 atm · 101,325 kPa/atm = 87,14 kPa.
V- volume of methane = 159 L
T - temperature= 294°C = 567 K.
R - gas constant = 8,314 J/K·mol.
n - number of moles = ?
Put the values in the formula, sole it for n,
[tex]\bold{n(CH₄) = \dfrac {pV} {RT}}\\\\\bold {n(CH₄) = \dfrac {87,14 kPa \times 159 L} {8,314 J/K.mol \times 567 K}.}\\\\\bold {n(CH₄) = 2,93 mol}[/tex]
Since, the molar ratio of methane to hydrogen is 3:1.
SO,
[tex]\bold {n(H_2) = 2,93 mol \times 3 }\\\\\bold {n (H_2) = 8,79 mol.}\\[/tex]
Hence, the mass of the dihydrogen produced,
[tex]\bold{ m(H_2) = 8.79 mol \times 2 g/mol.}\\\\\bold {m(H_2) = 17.58 g \times 0.001 kg/g}\\\\\bold {m(H_2) = 0.01758 kg}[/tex]
Therefore, the rate of the dihydrogen production is 0.0175 kg/sec for the given reaction.
To know more about Methane reaction:
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