its called a coefficient
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answer: - 8.97 atm.
solution: - moles of each gas, volume of the vessel and temperature are given. so, we could easily use the partial pressure of each gas using ideal gas law equation.
pv = nrt
p is the pressure, v is the volume, n is the moles of the gas, r is universal gas constant and t is kelvin temperature.
the equation is rearranged for the pressure as:
to calculate the partial pressure of fluorine we will use its moles.
n = 2.0 mol
v = 5.0 l
t = 273 k
r = 0.0821
p = ?
let's plug in the values and calculate the partial pressure of fluorine.
p = 8.97 atm
so, the partial pressure of fluorine gas is 8.97 atm.
to solve this problem, we can use the combined gas laws:
p₁v₁/t₁ = p₂v₂/t₂ multiply each side by t₁
p₁v₁ = p₂v₂ × t₁/t₂ divide each side by v₁
p₁ = p₂ × v₂/v₁ × t₁/t₂
p₁ = ? ; v₁ = 34.3 l; t₁ = 31.5 °c
p₂ = 122.2 kpa; v₂ = 29.2 l; t₂ = 21.0 °c
(a) convert temperatures to kelvins
t₁ = (31.5 + 273.15) k = 304.65 k
t₂ = (21.0 + 273.15) k = 294.15 k
(b) calculate the pressure
p₁ = 122.2 kpa × (29.2/34.3) × (304.65/294.15)
= 122.2 kpa × 0.8542 × 1.0357
= 108 kpa