Calculate the ∆H rxn for the following thermochemical equation: S (s) + 3 2 \frac32 O 2 (g) → SO 3 (s) ΔH rxn = ? When given the following: 2 S (s) + 3 O 2 (g) → 2 SO 3 (s) ΔH rxn = −296.8 kJ

Here we need to calculate the enthalpy of reaction for the following thermochemical equation, when given the following equation below it. So we need to see what changes happened to this original one, and what effect it will have on this delta h of reaction. So notice here this is a 2, but now it's a 1. This was a 3, but now it's 3 over 2. This was a 2, but now it's a 1. The reactants are still reactants, the product is still a product. So we didn't reverse the reaction. What we did though is we divided this entire thing by 2. Well, not this, we divided the original by 2. So if I divided the original equation by 2 that means I need to divide my delta h of reaction also by 2. So I'm gonna divide this by 2, so when I do that my new delta h of reaction will equal negative 148.4 kilojoules. Remember, whatever I divide my thermochemical equation by, I must divide my delta h value by that same number. So here doing that again gives me negative 148.4 kilojoule.

Calculate the ∆Hrxn for the following thermochemical eq...

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Calculate the ∆H_rxn for the following thermochemical equation:
S (s) + $\frac{3}{2}$ O₂ (g) → SO₃ (s) ΔH_rxn = ?
When given the following:
2 S (s) + 3 O₂ (g) → 2 SO₃ (s) ΔH_rxn = −296.8 kJ

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Calculate the ∆Hrxn for the following thermochemical equation:S (s) + 32\frac32 O2 (g) → SO3 (s) ΔHrxn = ?When given the following:2 S (s) + 3 O2 (g) → 2 SO3 (s) ΔHrxn = −296.8 kJ

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Hess's Law practice set

Calculate the ∆H_rxn for the following thermochemical equation:
S (s) + $\frac{3}{2}$ O₂ (g) → SO₃ (s) ΔH_rxn = ?
When given the following:
2 S (s) + 3 O₂ (g) → 2 SO₃ (s) ΔH_rxn = −296.8 kJ