Answer:
Na+Cl2-----NaCl
Explanation:
it's the chemical formula of common salt.
Answer: 225.75g
Explanation:
Molar Mass of Fe(OH)2 = 56 + 2(16 + 1) = 56 + 2(17) = 56 + 34 = 90g/mol
1mole(90g) of Fe(OH)2 contained 6.02x10^23 units.
Therefore, Xg of Fe(OH)2 will contain 1.51x10^24 units
Xg of Fe(OH)2 = (90x1.51x10^24)/6.02x10^23 = 225.75g
The entropy change, so the appropriate sign is negative. -286.23 J/K (decrease in entropy) Non-spontaneous process.
Entropy is a systematic idea in addition to measurable physical belongings that is most normally associated with a country of ailment, randomness, or uncertainty.
A result of entropy is that certain processes are irreversible or impossible, apart from the requirement of now not violating the conservation of electricity, the latter being expressed inside the first regulation of thermodynamics. Entropy is valuable to the second regulation of thermodynamics.
ENTROPY CHANGE = ENTROPY OF PRODUCT - ENTROPY OF REACTANT
ΔS = ΣΔSf(product) - ΣΔSf(reactant)
1. At STP
[2ΔSf(HNO3 (aq)) + 1ΔSf(NO (g))] - [3ΔSf(NO2 (g)) + 1ΔSf(H2O (ℓ))]
ΔSf(HNO3 (aq) = 146.44 J/K
ΔSf(NO (g) = 210.65 J/K
ΔSf(NO2 (g) = 239.95 J/K
ΔSf(H2O (ℓ) = 69.91 J/K
2(146.44) + 1(210.65)] - [3(239.95) + 1(69.91)] = -286.23 J/K
-286.23 J/K (decrease in entropy)
Non-spontaneous process.
Learn more about entropy here:-brainly.com/question/419265
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<em>Transferases</em> - C) Catalyze the movement of a functional group from one molecule to another
<em>Isomerases</em> - D) Catalyze structural changes in a molecule
<em>Ligases</em> - B) Catalyze reactions involving the joining of two substrates
<em>Oxidoreductases</em> - A) Catalyze reduction reactions
Answer : The correct option is, (C) 1.4 g
Solution : Given,
Mass of ammonia = 1.7 g
Molar mass of ammonia = 17 g/mole
Molar mass of nitrogen = 28 g/mole
First we have to calculate the moles of ammonia gas.
![\text{ Moles of }NH_3=\frac{\text{ Mass of }NH_3}{\text{ Molar mass of }NH_3}=\frac{1.7g}{17g/mole}=0.1moles](https://tex.z-dn.net/?f=%5Ctext%7B%20Moles%20of%20%7DNH_3%3D%5Cfrac%7B%5Ctext%7B%20Mass%20of%20%7DNH_3%7D%7B%5Ctext%7B%20Molar%20mass%20of%20%7DNH_3%7D%3D%5Cfrac%7B1.7g%7D%7B17g%2Fmole%7D%3D0.1moles)
The given balanced reaction is,
![N_2(g)+3H_2(g)\rightarrow 2NH_3(g)](https://tex.z-dn.net/?f=N_2%28g%29%2B3H_2%28g%29%5Crightarrow%202NH_3%28g%29)
From the reaction, we conclude that
As, 2 moles of ammonia produced from 1 mole of nitrogen
So, 0.1 moles of ammonia produced from
moles of nitrogen
The moles of nitrogen = 0.05 moles
Now we have to calculate the mass of nitrogen.
![\text{ Mass of nitrogen}=\text{ Moles of nitrogen}\times \text{ Molar mass of nitrogen}](https://tex.z-dn.net/?f=%5Ctext%7B%20Mass%20of%20nitrogen%7D%3D%5Ctext%7B%20Moles%20of%20nitrogen%7D%5Ctimes%20%5Ctext%7B%20Molar%20mass%20of%20nitrogen%7D)
![\text{ Mass of nitrogen}=(0.05moles)\times (28g/mole)=1.4g](https://tex.z-dn.net/?f=%5Ctext%7B%20Mass%20of%20nitrogen%7D%3D%280.05moles%29%5Ctimes%20%2828g%2Fmole%29%3D1.4g)
Therefore, the mass of nitrogen must be react is, 1.4 g.