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lara [203]
2 years ago
14

According to the Brensted-Lowry model write the equation for provided acid showing

Chemistry
1 answer:
Taya2010 [7]2 years ago
3 0

Answer:

i dont know sorry

Explanation:

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An acetylide anion is more stable than either a vinylic or alkyl anion due to Group of answer choices the greater stability of a
sashaice [31]

Answer:

the stabilization of the negative charge in orbitals with higher s character

Explanation:

Acetylide anion is a carbon anion compound or popularly called carbanion. Now Acetylide anion is sp hybridized. However acetylide anion tends to be more acidic as we move from sp³ to sp, hence acidicity increases, which makes sp to have the highest acidity and become the most  stable.

So, we can conclude that the acetylide anion is more acidic due to the stabilization of the negative charge in orbitals with higher s character and  as the s character increases, acidic nature of acetylide anion also increases.

5 0
2 years ago
Equal molar quantities of Ca2 and EDTA (H4Y) are added to make a 0.010 M solution of CaY2- at pH 10. The formation constant for
abruzzese [7]

Answer:

the concentration of free Ca2⁺ in this solution is 7.559 × 10⁻⁷

Explanation:

Given the data in the question;

Ca^{2+ + y^{4- ⇄  CaY^{2-

Formation constant Kf

Kf = CaY^{2- / ( [Ca^{2+][y^{4-] ) = 5.0 × 10¹⁰

Now,

[y^{4-] = \alpha _4CH_4Y; ∝₄ = 0.35

so the equilibrium is;

Ca^{2+ + H_4Y ⇄  CaY^{2- + 4H⁺

Given that; CH_4Y = Ca^{2+     { 1 mol Ca^{2+  reacts with 1 mol H_4Y  }

so at equilibrium, CH_4Y = Ca^{2+ = x

∴

Ca^{2+ + y^{4- ⇄  CaY^{2-

x        + x         0.010-x

since Kf is high, them x will be small so, 0.010-x is approximately 0.010

so;

Kf = CaY^{2- / ( [Ca^{2+][y^{4-] ) =  CaY^{2- / ( [Ca^{2+][\alpha _4CH_4Y] )  = 5.0 × 10¹⁰

⇒ CaY^{2- / ( [Ca^{2+][\alpha _4CH_4Y] )  = 5.0 × 10¹⁰

⇒ 0.010 / ( [x][ 0.35 × x] )  = 5.0 × 10¹⁰

⇒ 0.010 / 0.35x²  = 5.0 × 10¹⁰

⇒ x² = 0.010 / ( 0.35 × 5.0 × 10¹⁰ )

⇒ x² = 0.010 / 1.75 × 10¹⁰

⇒ x² = 0.010 / 1.75 × 10¹⁰

⇒ x² = 5.7142857 × 10⁻¹³

⇒ x = √(5.7142857 × 10⁻¹³)

⇒ x = 7.559 × 10⁻⁷

Therefore, the concentration of free Ca2⁺ in this solution is 7.559 × 10⁻⁷

8 0
2 years ago
2Al + 6HCl → 2AlCl3 + 3H2<br> If 85.0 grams of HCl react, how many moles of H2 are produced?
Murrr4er [49]

Answer:

1.17 mol

Explanation:

Step 1: Write the balanced equation

2 Al + 6 HCl → 2 AlCl₃ + 3 H₂

Step 2: Calculate the moles corresponding to 85.0 g of HCl

The molar mass of HCl is 36.46 g/mol.

85.0 g × 1 mol/36.46 g = 2.33 mol

Step 3: Calculate the number of moles of H₂ produced from 2.33 moles of HCl

The molar ratio of HCl to H₂ is 6:3.

2.33 mol HCl × 3 mol H₂/6 mol H₂ = 1.17 mol H₂

8 0
2 years ago
Complete the mechanism for the reaction of 2-butanol in sulfuric acid at 140 °C by adding any missing atoms, bonds, charges, non
Svetlanka [38]

Answer:

2-Butene

Explanation:

The first step is the <u>ionization</u> of the acid to produce the hydronium ion. Then the OH will attack this ion to produce a <u>charged species</u> that can be stabilized when <u>H2O is produced</u>.

Then an <u>elimination</u> takes place to produce the more <u>substituted alkene</u> 2-butene and the <u>hydronium ion</u> is gain produced.

4 0
3 years ago
if you started with 2.34 grams of methane and 8.32 grams of oxeygyn and the combustion reaction went to completion how many gram
Romashka-Z-Leto [24]

Answer:

Mass of CO₂ produced  = 5.72 g

Explanation:

Given data:

Mass of methane = 2.34 g

Mass of oxygen = 8.32 g

Mass of CO₂ produced = ?

Solution:

Chemical equation:

CH₄ + 2O₂    →      CO₂ + 2H₂O

Number of moles of methane:

Number of moles = mass/molar mass

Number of moles =  2.34 g/ 16 g/mol

Number of moles = 0.146 mol

Number of moles of oxygen:

Number of moles = mass/molar mass

Number of moles =  8.32 g/ 32 g/mol

Number of moles = 0.26 mol

Now we will compare the moles of carbon dioxide with oxygen and methane.

                         CH₄             :              CO₂

                           1                 :              1

                        0.146            :           0.146

                         O₂                :               CO₂

                          2                 :                   1

                     0.26                :              1/2×0.26 = 0.13 mol

Less number of moles of CO₂ are produced by oxygen thus oxygen will react as limiting reactant.

Mass of CO₂:

Mass = number of moles × molar mass

Mass = 0.13 mol ×  44 g/mol

Mass = 5.72 g

4 0
2 years ago
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