Answer: Reaction 1 is non spontaneous.
Explanation:
According to Gibb's equation:
= Gibbs free energy
= enthalpy change
= entropy change
T = temperature in Kelvin
When = +ve, reaction is non spontaneous
= -ve, reaction is spontaneous
= 0, reaction is in equilibrium
For the given reaction 1: 
As for the reaction 1 , the value of Gibbs free energy is positive and thus the reaction 1 is non spontaneous.
The graph is not given in the question, so, the required graph is attached below:
Answer:
According to the graph, the relationship between the density of the sugar solution and the concentration of the sugar solution is directly proportional to each other as they both are increasing exponentially.
The graph shows that, the density of sugar solution will increase with the increase in concentration of sugar in the solution.
Hello!
The
dissociation reaction of HNO₃ is the following:
HNO₃ → H⁺ + NO₃⁻This is a strong acid, so the concentration of HNO₃ would be the same as the concentration of H⁺. The formula for pH is the following:
![pH=-log([H_3O^{+}])=-log(0,75M)=0,12](https://tex.z-dn.net/?f=pH%3D-log%28%5BH_3O%5E%7B%2B%7D%5D%29%3D-log%280%2C75M%29%3D0%2C12)
So, the pH would be
0,12Have a nice day!
An exothermic reaction is one which is accompanied by the release of heat energy.
In the given situation, hydrogen and oxygen combine to form water along with the generation of heat.
2H2 + O2 → 2H2O + heat
Based on the law of conservation of energy: 'energy can be neither created nor destroyed". This implies that whatever energy is released must have been present in the reactants. Therefore, the reactants must be in a higher energy level than products.
If the reaction shown below is exothermic, the energy level of the reactants is higher than products.
Answer:233 Joules/K
Explanation:
∆H= 26.5KJmol-1
Kelvin temperature = 34.6 + 273 = 307.6 K
No of moles= 2.7 moles
2.70 mole x 26.5 kJ/mole = 71.55kilojoules
∆S=71.55 kilojoules / 307.6 K = 0.233 kilojoules/ K
Convert to JK-1
0.233 kilojoules/ K x 1000 Joules/kilojoule = 233 Joules/K
