Answer:
d
. H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O
Explanation:
a
. 2HgO → 2Hg + O₂,
It is a decomposition reaction, that HgO is decomposed to give Hg and O.
b
. Na₂SO₄ + BaCl₂ → BaSO₄ + 2NaCl,
It is a double replacement reaction where two salts replaces their cations and anions with each others producing 2 new salts.
c
. Zn + 2AgNO₃ → Zn(NO₃)₂ + 2Ag,
It is a single replacement reaction, that Zn replaces Ag from its salt.
d
. H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O
It is acid-base reaction "neutralization reaction" where H₂SO₄ (acid) reacts with KOH (base) producing K₂SO₄ (salt) and water.
<em>d
. H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O</em>
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Answer:
C. An 1s orbital
Explanation:
At the first energy level, the only orbital available to electrons is the 1s orbital, but at the second level, as well as a 2s orbital, there are also orbitals called 2p orbitals.
H₂O + H₂O ⇌ H₃O⁺ + OH⁻
You use two single-barbed arrows pointing in opposite directions (technically rightwards harpoon over leftwards harpoon) <em>to indicate a reversible reactio</em>n.
The first one I god it wrong and he told us the answer
<span>The balanced equation would be 4NH3 + 7O2 --> 4NO2 + 6H2O.
Mass of Ammonia = 43.9 g; Molecular weight of Ammonia NH3 = 17.03056 g/mol.
Mass of Oxygen = 258 g; Molecular weight of Oxygen O2 = 31.998 g/mol.
Calculating the moles of Ammonia NH3 = Mass / Molecular weight of ammonia
= 43.9 g / 17.03 g/mol = 2.578 moles of Ammonia.
Calculating the moles of Oxygen O2 = Mass / Molecular weight of Oxygen
=258 g / 31.998 g/mol = 8.063 moles of Oxygen.
2.578 moles of Ammonia will react with (7/4) x 2.578 moles of Oxygen (from the equation) that is 4.5115 moles of O2 to produce the NO2. Since we have more moles of O2 8.063 moles, Ammonia will be the limiting agent.
Calculating the NO2 produces using the coordinate from the equation
Molecular weight of NO2 = 46.00558 g/mol
Mass of NO2 = (2.578 mol) x (4 mol of NO2 / 4 mol of NH3) x (46.006 g /mol)
Produced NO2 = 118.6 g NO2</span>
