Each mole of butane needs 6.5 moles of oxygen, so 13 moles of oxygen is required for 2 moles of butane in a complete combustion
Options are as follow,
A. P₄O₁₀
B. PCl₅
C. Ca₃(PO₄)₂
<span>D. KH</span>₂PO₃
Answer;
The correct option is Option-D (KH₂PO₃).
Explanation:
Oxidation number of Phosphorous is calculated as,
As the normal oxidation number of K is +1, H is +1 and O is -2 so,
KH₂PO₃ = 0
0 shows that the molecule is neutral. Now puttion values of all elemnts except P,
(+1) + (+1)₂ + P + (-2)₃ = 0
+1 + 2 + P - 6 = 0
+3 + P - 6 = 0
+3 + P = +6
P = +6 - 3
P = +3
Answer:
- <em><u>The third chice: 0.0750 M Na₂SO₄</u></em>
Explanation:
Assume 100% ionization:
<em><u>1) 0.100 M solution K₂SO₄</u></em>
- K₂SO4 (aq) → 2K⁺ (aq) + SO₄²⁻ (aq)
- Mole ratios: 1 mol K₂SO4 : 2 mol K⁺ + 1 mol SO₄²⁻ (aq) : 3 mol ions. This is 1 : 3
- At constant volume, the mole ratios are equal to the concentration ratios (M).
- 1 M K₂SO₄: 3 M ions = 0.100 M K₂SO₄ / x ⇒ x = 0.300 M ions
This means, that you have to find which of the choices is a solution that contains the same 0.300 M ion concentration.
<u>2) 0.0800 M Na₂CO₃</u>
- Na₂CO₃ (aq) → 2 Na⁺ + CO₃⁻
- 1 M Na₂CO₃ / 3 M ions = 0.0800M / x ⇒ x = 0.0267 M ions
This is not equal to 0.300 M, so this solution would not contain the same total concentration as a 0.100 M solution of K₂SO₄, and is not the right answer.
<u>3) 0.100 M NaCl </u>
- 1 M NaCl / 2 M ions = 0.100 M NaCl / x ⇒ x = 0.200 M ions
This is not equal to 0.300 M ion, so not a correct option.
<u>4) 0.0750 M Na₃PO₄</u>
- 1 M Na₃PO₄ / 4 M ions = 0.0750 M Na₃PO₄ / x ⇒ x = 0.300 M ions
Hence, this ion concentration is equal to the ion concentration of a 0.100 M solution of K₂SO₄, and is the correct choice.
<u>5) 0.0500 M NaOH </u>
- 1 M NaOH / 2 mol ions = 0.0500 M NaOH / x ⇒ x = 0.100 M ions
Not equal to 0.300 M, so wrong choice.
Strontium Phosphate is made from that thing
405 PHz
I might be wrong because that might be for 0.74 nm. We will see with out people answers
