First step is to balance the reaction equation. Hence we get
P4 + 5 O2 => 2 P2O5
Second, we calculate the amounts we start with
P4: 112 g = 112 g/ 124 g/mol – 0.903 mol
O2: 112 g = 112 g / 32 g/mol = 3.5 mol
Lastly, we calculate the amount of P2O5 produced.
2.5 mol of O2 will react with 0.7 mol of P2O5 to produce 1.4
mol of P2O5.
This is 1.4 * (31*2 + 16*5) = 198.8 g
Answer: The reaction is first order overall.
Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.
![Rate=k[A]^x[B]^y](https://tex.z-dn.net/?f=Rate%3Dk%5BA%5D%5Ex%5BB%5D%5Ey)
k= rate constant
For the given rate law:
![Rate=k[A]^1[B]^1](https://tex.z-dn.net/?f=Rate%3Dk%5BA%5D%5E1%5BB%5D%5E1)
x = 1= order with respect to A
y =1= order with respect to B
n =( x+y)= (1+1) = 2 = Total order
a) If [A] is doubled, the reaction rate will increase by a factor of 2: True
![Rate'=k[2A]^1[B]^1](https://tex.z-dn.net/?f=Rate%27%3Dk%5B2A%5D%5E1%5BB%5D%5E1)
![Rate'=k[2]^1[A]^1[B]^1](https://tex.z-dn.net/?f=Rate%27%3Dk%5B2%5D%5E1%5BA%5D%5E1%5BB%5D%5E1)
![Rate'=[2]^1\times Rate](https://tex.z-dn.net/?f=Rate%27%3D%5B2%5D%5E1%5Ctimes%20Rate)
![Rate'=[2]\times Rate](https://tex.z-dn.net/?f=Rate%27%3D%5B2%5D%5Ctimes%20Rate)
b) The reaction is first order overall: False
The overall order is 1+1= 2.
c) k is the reaction rate constant: True
![Rate=k[A]^x[B]^y](https://tex.z-dn.net/?f=Rate%3Dk%5BA%5D%5Ex%5BB%5D%5Ey)
k= rate constant
d) The reaction is first order in [B]: True
For the given rate law:
![Rate=k[A]^1[B]^1](https://tex.z-dn.net/?f=Rate%3Dk%5BA%5D%5E1%5BB%5D%5E1)
x = 1= order with respect to A
e) The reaction is first order in [A]: True
For the given rate law:
![Rate=k[A]^1[B]^1](https://tex.z-dn.net/?f=Rate%3Dk%5BA%5D%5E1%5BB%5D%5E1)
y =1= order with respect to B