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2 years ago

Which substance can be classified as an Arrhenius Acid?

Chemistry

2 answers:

xxMikexx [17]2 years ago

7 0

Answer:

B

Explanation:

An Arrhenius Acid is a substance that dissociates in water to form Hydrogen (H⁺) ions.

Let's write the dissociation reactions of each of the options :

⇒ KF = K⁺ + F⁻

⇒ HF = H⁺ + F⁻

⇒ KOH = K⁺ + OH⁻

⇒ LiH = Li⁺ + H⁻

Only HF forms a Hydrogen ion on dissociation, hence it is the Arrhenius Acid.

Gelneren [198K]2 years ago

5 0

Answer:

Explanation:

Arrhenius acids are the substances that when dissolved in water are capable to give an H+ ion

Here

HF on dissolving into water releases H+ and F- ion so it's a Arrhenius acid

Option B

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2 years ago

Given these reactions, X ( s ) + 1 2 O 2 ( g ) ⟶ XO ( s ) Δ H = − 668.5 k J / m o l XCO 3 ( s ) ⟶ XO ( s ) + CO 2 ( g ) Δ H = +

qwelly [4]

Answer: The $\Delta H^o_{rxn}$ for the reaction is -1052.8 kJ.

Explanation:

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The given chemical reaction follows:

$X(s)+\frac{1}{2}O_2(g)+CO_2(g)\rightarrow XCO_3(s)$ $\Delta H^o_{rxn}=?$

The intermediate balanced chemical reaction are:

(1) $X(s)+\frac{1}{2}O_2(g)\rightarrow XO(s)$ $\Delta H_1=-668.5kJ$

(2) $XCO_3(s)\rightarrow XO(s)+CO_2$ $\Delta H_2=+384.3kJ$

The expression for enthalpy of the reaction follows:

$\Delta H^o_{rxn}=[1\times \Delta H_1]+[1\times (-\Delta H_2)]$

Putting values in above equation, we get:

$\Delta H^o_{rxn}=[(1\times (-668.5))+(1\times (-384.3))=-1052.8kJ$

Hence, the $\Delta H^o_{rxn}$ for the reaction is -1052.8 kJ.

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