Larger nickel–zinc battery systems have been known for over 100 years. Since 2000, development of a stabilized zinc electrode system has made this technology viable and competitive with other commercially available rechargeable battery systems.
Explanation:
element x _ carbon having two shells 2,3
element y _ fluorine atomic no 9 EC 2,7
when carbon react with fluorine it destroyes graphite and form fluorocarbons and thus form covalent bond
hope it helps u
Answer:
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Explanation:
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Answer:
The equilibrium constant for this reaction is 3.2
Explanation:
Step 1: Data given
Number of moles H2S = 1.0 moles
Number of moles H2 = 4.0 moles
Number of moles S2 = 0.80 moles
Volume = 4.0 L
Step 2: The balanced equation
2H2S(g) ⇆ 2H2(g) S2(g)
Step 3: Calculate molarity
[H2] = 4.0 moles / 4.0 L = 1.0 M
[S2]= 0.80 moles / 4.0 L = 0.20 M
[H2S] = 1.0 moles / 4.0 L = 0.25 M
Step 4: Calculate Kc
Kc = [H2]²[S2] / [H2S]²
Kc = (1.0²*0.20)/0.25²
Kc = 0.2 / 0.0625
kC = 3.2
The equilibrium constant for this reaction is 3.2
The standard enthalpy of reaction of the given reaction is -865.71 kJ per mole of N₂H₃CH₃.
<h3>What is the standard molar enthalpy of formation?</h3>
The standard molar enthalpy of formation of a compound is defined as the enthalpy of formation of 1.0 mol of the pure compound in its stable state from the pure elements in their stable states at P = 1.0 bar at a constant temperature.
Let's consider the following equation.
4 N₂H₃CH₃(l) + 5 N₂O₄(l) → 12 H₂O(g) + 9 N₂(g) + 4 CO(g)
We can calculate the standard enthalpy of the reaction using the following expression.
ΔH° = Σnp × ΔH°f(p) - Σnr × ΔH°f(r)
where,
- ΔH° is the standard enthalpy of the reaction.
- n is stoichiometric coefficient.
- ΔH°f is the standard molar enthalpy of formation.
- p are the products.
- r are the reactants.
ΔH° = 12 mol × ΔH°f(H₂O(g)) + 9 mol × ΔH°f(N₂(g)) + 4 mol × ΔH°f(CO(g)) - 4 mol × ΔH°f(N₂H₃CH₃(l)) - 5 mol × ΔH°f(N₂O₄(l))
ΔH° = 12 mol × (-241.81 kJ/mol) + 9 mol × (0 kJ/mol) + 4 mol × (-110.53 kJ/mol) - 4 mol × (54.20 kJ/mol) - 5 mol × (-19.56 kJ/mol)
ΔH° = -3462.84 kJ
In the balanced equation, there are 4 moles of N₂H₃CH₃. The standard enthalpy of reaction per mole of N₂H₃CH₃ is:
-3462.84 kJ / 4 mol = -865.71 kJ/mol
The standard enthalpy of reaction of the given reaction is -865.71 kJ per mole of N₂H₃CH₃.
Learn more about enthalpy here: brainly.com/question/11628413
