C. All the known elements that exist in the world today
<u>Answer:</u> The rate law for the reaction is ![\text{Rate}=k[NO_2][Cl_2]](https://tex.z-dn.net/?f=%5Ctext%7BRate%7D%3Dk%5BNO_2%5D%5BCl_2%5D)
<u>Explanation:</u>
In a mechanism of the reaction, the slow step in the mechanism always determines the rate of the reaction.
For the given chemical reaction:
![2NO_2+Cl_2\rightarrow 2NO_2Cl](https://tex.z-dn.net/?f=2NO_2%2BCl_2%5Crightarrow%202NO_2Cl)
The intermediate reaction of the mechanism follows:
<u>Step 1:</u> ![NO_2+Cl_2\rightarrow NO_2Cl+Cl;\text{ (slow)}](https://tex.z-dn.net/?f=NO_2%2BCl_2%5Crightarrow%20NO_2Cl%2BCl%3B%5Ctext%7B%20%28slow%29%7D)
<u>Step 2:</u> ![NO_2+Cl\rightarrow NO_2Cl;\text{(fast)}](https://tex.z-dn.net/?f=NO_2%2BCl%5Crightarrow%20NO_2Cl%3B%5Ctext%7B%28fast%29%7D)
As, step 1 is the slow step. It is the rate determining step
Rate law for the reaction follows:
![\text{Rate}=k[NO_2][Cl_2]](https://tex.z-dn.net/?f=%5Ctext%7BRate%7D%3Dk%5BNO_2%5D%5BCl_2%5D)
Hence, the rate law for the reaction is ![\text{Rate}=k[NO_2][Cl_2]](https://tex.z-dn.net/?f=%5Ctext%7BRate%7D%3Dk%5BNO_2%5D%5BCl_2%5D)
Answer:
ΔH = - 2020.57 kJ/mol
Explanation:
Given that :
mass of propanol = 1.685 g
the molar molar mass = 60 g/mol
Thus; the number of moles = mass/molar mass
= 1.685 g/60 g/mol
= 0.028 g/mol
However ;
ΔH = heat capacity C × Δ T
Given that:
The temperature increases from 298.00 K to 302.16 K.
Then ;
Δ T = 302.16 K - 298.00 K
Δ T = 4.16 K
heat capacity C = 13.60 kJ/K
∴
ΔH = 13.60 kJ/K × 4.16 K
ΔH = 56.576 kJ
The equation of the given reaction can be represented as :
![C_3H_7OH_{(l)}+\dfrac{3}{2}O_{2(g)} \to 3CO_{2(g)} +4H_2O_{(l)}](https://tex.z-dn.net/?f=C_3H_7OH_%7B%28l%29%7D%2B%5Cdfrac%7B3%7D%7B2%7DO_%7B2%28g%29%7D%20%20%5Cto%203CO_%7B2%28g%29%7D%20%2B4H_2O_%7B%28l%29%7D)
Thus for 0.028 mol of heat liberated; ΔH = 56.576 kJ
For 1 mole of heat liberated now:
ΔH = 56.576 kJ/0.028 mol
ΔH = 2020.57 kJ/mol
SInce , Heat is liberated, the reaction undergoes an exothermic reaction thus;
ΔH = - 2020.57 kJ/mol