Respuesta :
Answer:
Partial pressure of hydrogen molecule = 9·246 atm
Total pressure within the container = 15·41 atm
Explanation:
Given chemical equation
H2 (g) → 2 H(g)
For every 1 mole of hydrogen molecule dissociated, 2 moles of hydrogen atoms is formed
Given number of moles of hydrogen molecule = 10 ÷ 2 = 5
As 25% of H2 is dissociated, it means that 5 ÷ 4 moles of hydrogen molecule is dissociated
Number of moles of hydrogen atom formed = 2 × 1·25 = 2·5
Remaining moles of hydrogen molecule = 5 - 1·25 = 3·75
Assuming that both hydrogen molecule and hydrogen atom as ideal gases
Ideal gas equation = P × V = n × R × T
where P is the pressure of the gas
V is the volume occupied by the gas
n is the number of moles of gas
R is the ideal gas constant
T is the temperature of the gas
Partial pressure is defined as the pressure exerted by the gas when it occupies the complete volume of the container
Let the partial pressure of hydrogen molecule be P atm
Applying ideal gas equation to the hydrogen molecule
V = 100 L
n = 3·75
T = 2730°C = 2730 + 273 K = 3003 K
P × 100 = 3·75 × 0·0821 × 3003
∴ P = 9·246 atm
Let [tex]P_{1}[/tex] be the partial pressure of hydrogen atom
Applying ideal gas equation to the hydrogen atom
V = 100 L
n = 2·5
T = 2730°C = 2730 + 273 K = 3003 K
[tex]P_{1}[/tex] × 100 = 2·5 × 0·0821 × 3003
∴ [tex]P_{1}[/tex] = 6·164 atm
Total pressure within the container = P + [tex]P_{1}[/tex] = 9·246 + 6·164 atm = 15·41 atm
∴ Total pressure = 15·41 atm
