Answer
not too sure, but perhaps, 24
Explanation:
1 mole = 12 apples
2 moles = 24 apples
The rate law equation for Ozone reaction
r=k[O][O₂]
<h3>Further e
xplanation</h3>
Given
Reaction of Ozone :.
O(g) + O2(g) → O3(g)
Required
the rate law equation
Solution
The rate law is a chemical equation that shows the relationship between reaction rate and the concentration / pressure of the reactants
For reaction
aA + bB ⇒ C + D
The rate law can be formulated:
![\large{\boxed{\boxed{\bold{r~=~k.[A]^a[B]^b}}}](https://tex.z-dn.net/?f=%5Clarge%7B%5Cboxed%7B%5Cboxed%7B%5Cbold%7Br~%3D~k.%5BA%5D%5Ea%5BB%5D%5Eb%7D%7D%7D)
where
r = reaction rate, M / s
k = constant, mol¹⁻⁽ᵃ⁺ᵇ⁾. L⁽ᵃ⁺ᵇ⁾⁻¹. S⁻¹
a = reaction order to A
b = reaction order to B
[A] = [B] = concentration of substances
So for Ozone reaction, the rate law (first orde for both O and O₂) :
![\tt \boxed{\bold{r=k[O][O_2]}}](https://tex.z-dn.net/?f=%5Ctt%20%5Cboxed%7B%5Cbold%7Br%3Dk%5BO%5D%5BO_2%5D%7D%7D)
To test for hydrogen, burn a candle near the suspected source of hydrogen. If you hear a squeaky pop sound, hydrogen is present because when hydrogen gas burns, it makes a squeaky pop sound.
12 atm is the new pressure of the air‑fuel mixture when A gaseous air‑fuel mixture in a sealed car engine cylinder has an initial volume of 600 ml at 1.0atm and final volume of 50 ml.
Explanation:
Data given:
The air fuel mixture is assumed to be having ideal behaviour
initial volume of gaseous air fuel mixture V1 = 600 ml
initial pressure of gaseous air fuel mixture P1= 1 atm
final volume when piston is removed, V2= 50 ml
final pressure of the gaseous air mixture, P2 = ?
Applying the Boyle's Law,
P1V1 = P2V2
rearranging the equation:
P2 = 
putting the value in the equation,
P2 = 
P2 = 12 atm
the pressure is increased to 12 atm when volume is reduced to 50 ml.