Increasing the pressure will increase the reaction rate because it will force the particles to be closer together, and so the likelihood of particles colliding increases. Increasing the temperature can also increase the rate of a reaction because the particles will be more energised and more likely to move around and collide.
We use the equation for the standard enthalpy change of formation:
ΔHoreaction=∑ΔHof(products)−∑ΔHof(Reactants)
to calculate for the enthalpy for the reaction
2NaOH(s)+CO2(g)→Na2CO3(s)+H2O(l)
We now have
ΔHoreaction = { ΔHfo[Na2CO3(s)] + ΔHfo[H2O(l)] } - { ΔHfo[NaOH(s)] +
ΔHfo[CO2(g)] }
where we use the following Enthalpy of Formation (∆Hfo) values:
Substance ΔHf∘ (kJ/mol)
CO2(g) −393.509
H2O(l) −285.830
Na2CO3(s) −1130.68
NaOH(s) −425.609
and taking note of the coefficients of the products and the reactants,
ΔHoreaction = [1*(−1130.68) + 1*(−285.830)] − [2*(−425.609) + 1*(−393.509)]
= -1416.51 - (-1244.727)
= -171.783 kJ/mol
≈ -171.8 kJ/mol as our enthalpy for the given reaction.
Now considering the reaction
Na2CO3(s)→Na2O(s)+CO2(g) with enthalpy of reaction ΔHoreaction=321.5kJ/mol
we also use the equation for the standard enthalpy change of formation:
ΔHoreaction = ∑ΔHof(products)−∑ΔHof(Reactants)ΔHoreaction
= { ΔHfo[Na2O(s)] + ΔHfo[CO2(g)] } - { ΔHfo[Na2CO3(s)] }
to solve for the enthalpy of formation of Na2O(s):
ΔHfo[Na2O(s)] = ΔHoreaction - ΔHfo[CO2(g)] + ΔHfo[Na2CO3(s)]
Since the coefficients are all 1,
ΔHfo[Na2O(s)] = 321.5 - (-393.509) + (-1130.68)
ΔHfo[Na2O(s)] = -415.671 kJ/mol ≈ -415.7 kJ/mol
Answer:
ClO⁻ + HC₂H₃O₂ ⇄ HClO + C₂H₃O₂⁻
Explanation:
Sodium hypochlorite is a strong electrolyte that ionizes in sodium cation and hypochlorite anion.
NaClO(aq) ⇒ Na⁺(aq) + ClO⁻(aq)
ClO⁻ is a base that reacts with acetic acid (HC₂H₃O₂) from vinegar (neutralization reaction).
ClO⁻ + HC₂H₃O₂ ⇄ HClO + C₂H₃O₂⁻
Answer:
-
Explanation:
Water molecules pull the sodium and chloride ions apart, breaking the ionic bond that held them together. After the salt compounds are pulled apart, the sodium and chloride atoms are surrounded by water molecules, as this diagram shows. Once this happens, the salt is dissolved, resulting in a homogeneous solution.