Chemistry, 03.12.2019 00:31 droidd133

Given thath2(g) + f2(g) -> 2hf(g) => ∆h = -546.6 kj . mol-12h2(g) + o2(g) -> 2h20(l) => ∆h = -571.6 kj. mol-1

calculate the value of ∆h for: 2f2(g) + 2h20(l) -> 4hf(g) + o2(g)

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Answer from: Kurlyash

The $\Delta H^o_{rxn}$ for the reaction is -521.6 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 chemical equation for the reaction of fluorine and water follows:

$2F_2(g)+2H_2O(l)\rightarrow 4HF(g)+O_2(g)$ $\Delta H^o_{rxn}=?$

The intermediate balanced chemical reaction are:

(1) $H_2(g)+F_2(g)\rightarrow 2HF(g)$ $\Delta H_1=-546.6kJ$ ( × 2)

(2) $H_2(g)+O_2(g)\rightarrow 2H_2O(g)$ $\Delta H_2=-571.6kJ$

The expression for enthalpy of reaction follows:

$\Delta H^o_{rxn}=[2\times \Delta H_1]+[1\times (-\Delta H_2)]$

Putting values in above equation, we get:

$\Delta H^o_{rxn}=[(2\times (-546.6))+(1\times (571.6))]=-521.6kJ$

Hence, the $\Delta H^o_{rxn}$ for the reaction is -521.6 kJ.

Answer from: Quest

explanation:

Answer from: Quest

1.consider the following balanced equation and answer parts a through. show calculations for each part.

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.

explanation:

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Given thath2(g) + f2(g) -> 2hf(g) => ∆h = -546.6 kj . mol-12h2(g) + o2(g) -> 2h20(l) =&g...

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