All options are as follow,
<span>A. PbS + O2→ PbO + SO</span>₂<span>
B. PbS + 2O</span>₂<span>→ PbO + 2SO</span>₂<span>
C. 2PbS + 2O</span>₂<span>→ 2PbO + 2SO</span>₂<span>
D. 2PbS + 3O</span>₂<span>→ 2PbO + 2SO</span>₂<span>
E. 3PbS + 3O2→ 2PbO + 2SO2
Option A is not balanced because the number of oxygen atoms are greater at right hand side.
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Option B is not balanced because the number of oxygen are less at right hand side and number of sulfur atoms are greater at right hand side.
Option C is not balanced because the number of oxygen atoms are greater at right hand side.
Option D is Balanced, all elements are balanced at both sides.
Option E is not balanced because number of Lead and Sulfur atoms are greater at right hand side.
Result:
Equation in Option D is balanced and correct answer.
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Answer:
Explanation:
The best choice to prepare a buffer of pH 9.0 is a conjugate acid/base pair in which the acid has pKₐ = 9.0 ± 1.
Let's examine each of the choices.
A. NH₃/NH₄Cl
For NH₃, = pK_b = 4.75
For NH₄⁺, pKₐ 14.00 - 4.75 = 9.25
B. HCHO₂/NaCHO₂
For HCHO₂, pKₐ = 3.74
C. C₅H₅N/ C₅H₅NHCl
For C₅H₅N, = pK_b = 8.76
For C₅H₅N⁺, pKₐ 14.00 – 8.76 = 5.21
D. HNO₂/NaNO₂
For HNO₂, pKₐ = 3.33
The only acid with a pKₐ close to 9.0 is the ammonium ion.
The best buffer to prepare a buffer with pH 9.0 is
Answer:
F
Explanation:
nonmetal doesn't conduct, is shiny and silver and is solid. Hope this helps :)
Answer:
- <u><em>34 g of NH₃ </em></u><em>will be produced from the reaction of 28 g of N₂ with 25 g of H₂.</em>
Explanation:
1) <u>Balanced chemical equation</u>
- N₂ (g) + 3H₂ (g) → 2NH₃(g)
2) <u>Stoichiometric (theoretical ) mole ratios</u>
- 1 mol N₂ (g) : 3mol H₂ (g) : 2 mol NH₃(g)
3) <u>Number of moles of each reactant</u>
- number of moles = mass in grams / atomic mass
- number of moles of N₂ = 28 g / 28 g/mol = 1 mol
- number of moles of H₂: 25 g / 2 g/mol = 12.5 mol
4)<u> Limiting reactant</u>
Since the stoichiometry states that 1 mol of N₂ reacts with 3 moles of H₂, the given mass of N₂ will react completely with the given amount of H₂, and the calculations must be done with the 28 g (1 mol) of N₂ as the limiting reactant.
5) <u>Yield</u>
Set the proportion with the mole ratios:
1 mol H₂ / 2 mol NH₃ = 1 mol H₂ / x ⇒ x = 2 mol NH₃
6) <u>Convert to grams</u>
- mass in grams = number of moles × molar mass = 2 mol × 17 g/mol = 34 g.
Answer: <em>the reaction of 28 g of N₂ with 25 g of H₂ will produce 34 g of NH₃</em>
Answer:
carbonic acid
Explanation:
Carbonic acid refers to the natural existent acid in our atmosphere which is produced when water reacts with water vapor and it makes rain naturally acid. As a result, rainwater is always acidic. On the other hand, acid rain occurs when precipitation contains a higher than normal acidity and a pH lower than 5.0.