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pav-90 [236]
3 years ago
13

Which compounds are the Bronsted- Lowry bases in the equilibrium?

Chemistry
2 answers:
elena-s [515]3 years ago
6 0

Answer : Option D) H_{2}BO_{3}^{-} and C_{2}O_{4}^{2-}.

Explanation : The acid base theory of Bronsted-Lowry, stated the definition of acids and bases on the basis of conjugated.

The fundamental concept of this theory states that when an acid and a base reacts with each other, the acid forms its conjugate base, and the base forms its conjugate acid by exchanging the proton.

So, in the given reaction;

HC_{2}O_{4}^{-} + H_{2}BO_{3}^{-}  H_{3}BO_{3} + C_{2}O_{4}^{2-}

It is firstly observed that the species H_{2}BO_{3}^{-} is accepting a proton from the acid, therefore this is one of the bases.

Secondly,C_{2}O_{4}^{2-} accepts the proton and forms the reactant again in the reversible reaction.

Therefore, these are the correct options.

H_{2}BO_{3}^{-} and C_{2}O_{4}^{2-}

Butoxors [25]3 years ago
4 0
Its D for plato. 
by other people who asked




 
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Determine the number of significant figures in each of the following
Otrada [13]

Answer:

A. 3 Significant Figures

B. 6 Significant Figures

C. 2 Significant Figures

D. 4 Significant Figures

E. 4 Significant Figures

F. 5 Significant Figures

Explanation:

5 0
2 years ago
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2. A. 66 grams B. 33 grams c. 132 grams. D
Sonbull [250]

Answer:

Option A. 66 g

Explanation:

We'll begin by writing the balanced equation for the reaction. This is given below:

CH₄ + 2O₂ —> CO₂ + 2H₂O

Next, we shall determine the mass of CH₄ that reacted and the mass of CO₂ produced from the balanced equation. This is illustrated below:

Molar mass of CH₄ = 12 + (4×1)

= 12 + 4 = 16 g/mol

Mass of CH₄ from the balanced equation = 1 × 16 = 16 g

Molar mass of CO₂ = 12 + (16×2)

= 12 + 32 = 44 g/mol

Mass of CO₂ from the balanced equation = 1 × 44 = 44 g

SUMMARY:

From the balanced equation above,

16 g of CH₄ reacted to produce 44 g of CO₂.

Finally, we shall determine the theoretical yield of CO₂. this can be obtained as follow:

From the balanced equation above,

16 g of CH₄ reacted to produce 44 g of CO₂.

Therefore, 24 g of CH₄ will react to produce = (24 × 44) /16 = 66 g of CO₂.

Thus, the theoretical yield of CO₂ 66 g

8 0
3 years ago
How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?4247.56.56
neonofarm [45]

Answer:

6 half-lives are required for the concentration of reactant to decrease to 1.56% of its original value.

Explanation:

Using integrated rate law for first order kinetics as:

[A_t]=[A_0]e^{-kt}

Where,

[A_t] is the concentration at time t

[A_0] is the initial concentration

Given:

Concentration is decreased to 1.56 % which means that 0.0156 of [A_0] is decomposed. So,

\frac {[A_t]}{[A_0]} = 0.0156

Thus,

\frac {[A_t]}{[A_0]}=e^{-k\times t}

0.0156=e^{-k\times t}

kt = 4.1604

The expression for the half life is:-

Half life = 15.0 hours

t_{1/2}=\frac {ln\ 2}{k}

Where, k is rate constant

So,  

k=\frac {ln\ 2}{t_{1/2}}

\frac{4.1604}{t}=\frac {ln\ 2}{t_{1/2}}

t = 6\times t_{1/2}

<u>6 half-lives are required for the concentration of reactant to decrease to 1.56% of its original value.</u>

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3 years ago
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What does the sun do to generate energy?
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Hope this helps!
5 0
3 years ago
Read 2 more answers
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