Just try to find how you will get the reaction by adding the other reactions. Reverse the second eq as O is in reactant side and half it..
Now in the final reaction there is neither ozone nor oxygen so now you have oxygen on the products side after adding reversed
2 and 3, O ->1/2 O2
adding this to the third eq you get,
NO+O +O3 -> NO2 +3/2 O2
Now you need to remove O3 and O2 using the first equation,
So reverse the first one,half it and add, 3/2O2-> O3 adding it removes O3 and O2 you get the requires equation,
NO + O->NO2 you can do the calculation bit yourself when you add reactions Enthalpy is also added by Hess law so yeah that part should be pretty simple.
<span>HofO3 - [H of O(g) + H of O2] = deltaH
HofO3 = -107.2kJ/mol + 249.8 + 0 (Heat of formn.of O2 is 0
= +142.6kJ/mol </span>
Answer:
0.12 dm³ or 120 cm³
Explanation:
Hi there!
so first step find the number of moles
number of moles = mass ÷ Ar ( since o is an element and when it is alone, it is a diatomic molecule {O2} )
number of moles = mass ÷ Ar
number of moles = 0.16 ÷ ( 16 × 2 )
= 0.16 ÷ 32
= 5 × 10 ( power -3)
1 mol of O2 = 24 dm³ or 24 000 cm³
5 × 10 ( power -3) of O2 = (5 × 10 ( power -3)) × 24
= 0.12 dm³
or
= (5 × 10 ( power -3)) × 24 000
= 120 cm³
Answer: 2.51 moles of oxygen is consumed
Explanation:
Exothermic reaction : It is a type of chemical reaction where the energy is released into the surrounding. In the exothermic reaction, the energy of reactant are more than the energy of product.
In exothermic reaction, the change in enthalpy is, negative
The balanced chemical reaction is:
According to stoichiometry:
When 1 mole of oxygen is consumed , energy released = 285.8 kJ
285.8 kJ of energy is evolved when oxygen consumed = 1 mol
Thus whn 717.4 kJ of energy is evolved when oxygen consumed = moles
2.51 moles of oxygen is consumed
Answer:
If I remember correctly it should be B because it went from Cu^2 to Cu^0
Explanation: