Answer:
Eletrical
Explanation:
The electric transfers 70% of the input energy to kinetic energy 30% is wasted output energy in the form of thermal energy and sound.
Answer:
NH³
Explanation:
the 3 should be at the bottom of the H
Answer:
1.5 moles
Explanation:
To find the number of moles of HCl in 500 mL of a 3 M solution of HCl, we consider moles in 1 liter/ 1000 mL.
3 moles HCl is contained in 1000 mL
x moles is HCl is contained in 500 mL
Hence the number of moles of HCl in 500 mL is 1.5 moles.
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
