Answer: Heating the hydrated forms of cobalt chloride reverses the reactions above, returning cobalt chloride to the blue, water-free, or anhydrous, state. Water is "liberated" in these reactions, known as dehydration reactions.
Explanation:
It’s x200 plus 300 that’s why it is that answer
Fuel......................................
Answer:
52.8 g of O2.
Explanation:
We'll begin by writing the balanced equation for the reaction. This is illustrated below:
4Al + 3O2 —> 2Al2O3
From the balanced equation above,
4 moles of Al reacted with 3 moles of O2 to produce 2 moles of Al2O3
Next, we shall determine the number of mole of O2 needed to react with 2.2 moles of Al. This can be obtained as follow:
From the balanced equation above,
4 moles of Al reacted with 3 moles of O2.
Therefore, 2.2 moles of Al will react with = (2.2 × 3)/4 = 1.65 moles of O2.
Thus, 1.65 moles of O2 is needed for the reaction.
Finally, we shall determine the mass of O2 needed as shown below:
Mole of O2 = 1.65 moles
Molar mass of O2 = 2 × 16= 32 g/mol
Mass of O2 =?
Mole = mass/Molar mass
1.65 = mass of O2 /32
Cross multiply
Mass of O2 = 1.65 × 32
Mass of O2 = 52.8 g
Therefore, 52.8 g of O2 is needed for the reaction.
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
k= rate constant
d) The reaction is first order in [B]: True
For the given rate law:
x = 1= order with respect to A
e) The reaction is first order in [A]: True
For the given rate law:
y =1= order with respect to B
