Answer:
−2399.33 kJ
Explanation:
If NH₄NO₃ reacts with fuel oil to give a ΔH of -7198 for every 3 moles of NH₄NO₃
What is the enthalpy change for 1.0 mole of NH₄NO₃ in this reaction
∴ For every 1 mole, we will have of the total enthaply of the 3 moles
so, to determine the 1 mole; we have:
= −2399.33 kJ
∴ the enthalpy change for 1.0 mole of NH₄NO₃ in this reaction = −2399.33 kJ
0.010 M solution of hydrochloric acid, HCl has a pH of 2.00 but a 0.010 M solution of acetic acid, HCH₃COO, is 3.37 is because HCl dissociates more.
<h3>Dissociation</h3>This is the separation of ions of an ionic compound when it dissolves.
<h3>Hydrogen ion concentration of HCl</h3>Since 0.010 M solution of hydrochloric acid, HCl has a pH of 2.00 its hydrogen ion concentration is gotten from
pH = -log[H⁺]
So,
So, [H⁺] = 10⁻²
<h3>Hydrogen ion concentration of HCH₃COO</h3>Also, since 0.010 M solution of acetic acid, HCH₃COO, has a pH of 3.37, its hydrogen ion concentration is gotten from
pH = -log[H⁺]
So,
So, [H⁺] = 10⁻³°³⁷ = 0.000427 = 4.27 × 10⁻⁴
Since the hydrogen ion concentration of HCl is 10⁻² and the hydrogen ion concentration of HCH₃COO is 4.27 × 10⁻⁴, we see that HCl dissociates more than HCH₃COO.
So, 0.010 M solution of hydrochloric acid, HCl has a pH of 2.00 but a 0.010 M solution of acetic acid, HCH₃COO, is 3.37 is because HCl dissociates more.
Learn more about dissociation here: