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3 years ago

Which of the following shows a Bronsted-Lowry acid reacting?

Chemistry

2 answers:

7nadin3 [17]3 years ago

8 0

<h3>Answer:</h3>

Option-C: HCl + H₂O → H₃O⁺ + Cl⁻

Explanation:

Bronsted-Lowery concept of Acid and Base defines Acid as that specie which tends to donate H⁺ (Hydrogen Ion) and bases are those species which accepts H⁺ from Acids.

In selected option, HCl is reacting as Acid as it donates H⁺ to water (lowery bronsted base).

Also, the correspong acid is converted into conjugate base (i.e. Cl⁻) and base is converted into conjugate acid (i.e. H₃O⁺)

Akimi4 [234]3 years ago

7 0

Answer:

HCl + H2O Right arrow. H3O+ + Cl–

Explanation:D is the answer

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Answer : The pressure of gas will be, 3.918 atm and the combined gas law is used for this problem.

Solution :

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1$ = initial pressure of gas = 3 atm

$P_2$ = final pressure of gas = ?

$V_1$ = initial volume of gas = 1.40 L

$V_2$ = final volume of gas = 0.950 L

$T_1$ = initial temperature of gas = $35^oC=273+35=308K$

$T_2$ = final temperature of gas = $0^oC=273+0=273K$

Now put all the given values in the above equation, we get the final pressure of gas.

$\frac{3atm\times 1.40L}{308K}=\frac{P_2\times 0.950L}{273K}$

$P_2=3.918atm$

Therefore, the pressure of gas will be, 3.918 atm and the combined gas law is used for this problem.

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