Answer:
I have no Idea please give more context to your question.
Explanation:
The entropy of the given reactions increases (S° > 0):
- 2C2H6(g) + 7O2(g) ----> 4CO2(g) + 6H2O(g) ---> S° > 0.
- NH4Cl(s) ----> NH3(g) + HCl(g) ---> S° > 0.
<h3>What is entropy?</h3>
Entropy measure how disordered a system is. It a measure of how dispersed or random the total energy of a system is. The symbol for entropy is S.
A system in which entropy increases is one in which S° > 0.
The entropy of a system decreases when S° < 0.
Entropy of a system increases (S° > 0) if any change results in an increase in temperature, increase in number of molecules, or an increase in volume.
Considering the given systems, the entropy changes is as follows:
- 2C2H6(g) + 7O2(g) ----> 4CO2(g) + 6H2O(g) ---> S° > 0.
- 2CO2(g) + N2(g) ---->2CO(g) + 2NO(g) --> no change
- 2N2(g) + O2(g) -----> 2N2O(g) ---> decreases
- S (s,rhombic) + 2CO(g) ----> SO2(g) + 2C (s,graphite) ---> no change
- NH4Cl(s) ----> NH3(g) + HCl(g) ---> S° > 0.
In conclusion, an increase in volume and moles of substances results in entropy increase.
Learn more about entropy at: brainly.com/question/26691503
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Given data:
Hydrogen (H) = 3.730 % by mass
Carbon (C) = 44.44%
Nitrogen (N) = 51.83 %
This means that if the sample weighs 100 g then:
Mass of H = 3.730 g
Mass of C = 44.44 g
Mass of N = 51.83 g
Now, calculate the # moles of each element:
# moles of H = 3.730 g/ 1 g.mole-1 = 3.730 moles
# moles of C = 44.44/12 = 3.703 moles
# moles of N = 51.83/14 = 3.702 moles
Divide by the lowest # moles:
H = 3.730/3.702 = 1
C = 3.703/3.702 = 1
N = 3.702/3.702 = 1
Empirical Formula = HCN
