Answer:
Both reactions are acid-base reactions
Explanation:
An acid base reaction is a reaction that occurs between an acid and a base. This reaction often leads to the formation of a salt in the process. The nature of the salt depends on the type of acid and base that reacted in the process.
Both HNO3 and H2SO4 are strong acids. However, ammonia is a weak base. The acid base reaction between ammonia and these strong acids is shown below;
HNO3(aq) + NH3(aq) ------>NH4NO3(aq)
H2SO4(aq) + 2NH3(aq) ----> (NH4)2SO4(aq)
Answer:
d) 2.7 mol
Explanation:
limit reagent is H2:
∴ Mw H2 = 2.016 g/mol
∴ Mw N2 = 28.0134 g/mol
⇒ moles NH3 = (4.0 moles H2)×(2 mol NH3/3mol H2)
⇒ moles NH3 = 2.666 mol
⇒ moles NH3 ≅ 2.7 mol
Explanation:
Gases are very less denser also, they've negligible intermolecular force of attraction between the particles of the gas. So, they all are free to roam seperately and hence making a negligible volume for which they become heavy settle down.
Answer:
2.68
Explanation:
At the solution, the number of moles of each substance (acid and conjugate base) is the volume multiplied the concentration
nHNO₂ = 0.50 L * 0.85 mol/L = 0.425 mol
nNO₂⁻ = 0.50 L * 0.61 mol/L = 0.305 mol
At the buffer, the substances are in equilibrium. When HBr is added, it dissociantes in H⁺ and Br⁻, and the H⁺ will react with NO₂⁻ to form more HNO₂. So, NO₂⁻ will be consumed and HNO₂ will be formed at a 1:1:1 reaction:
nH⁺ = nHBr = 0.15 mol
nNO₂⁻ = 0.305 - 0.15 = 0.155 mol
nHNO₂ = 0.425 + 0.15 = 0.575 mol
The pH of a buffer can be calculated by the Handerson-Halsebach equation:
pH = pKa + log[A⁻]/[HA]
Where [A⁻] is the concentration of the conjugate base, and [HA], the concentration of the acid. Because the volume is the same, it can be used the number of moles:
pH = 3.25 + log (0.155/0.575)
pH = 2.68
Sulfur dioxide(SO2)
Diphosphorus Pentachloride(P2Cl5)
Dinitrogen tetroxide(N204)
