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makkiz [27]
3 years ago
10

For the following reactions, the ΔH° rxn is not equal to ΔH° f for the product except for ________.

Chemistry
1 answer:
kirill [66]3 years ago
5 0

Answer:

The correct option is: e. 2C(s, graphite) + 2H₂(g) → C₂H₄ (g)

Explanation:

The standard enthalpy of the reaction (\Delta H_{r}^{\circ}) is the change in enthalpy associated with a given chemical reaction. It can be calculated by the standard enthalpies of formation of the products and reactants.

\Delta H_{r}^{\circ} = \sum \Delta H_{f}^{\circ} (Products) - \sum \Delta H_{f}^{\circ} (reactants)

The standard enthalpy of formation (\Delta H_{f}^{\circ}) <u><em>of an elements that is present in its standard state is zero.</em></u>

Therefore,

a. H₂O (l) + 1/2 O₂ (g) → H₂O₂(l)

\Delta H_{r}^{\circ} = \left [\Delta H_{f}^{\circ} (H_{2}O_{2}, l) \right ] - \left [\Delta H_{f}^{\circ} (H_{2}O, l)+ 1/2\times \Delta H_{f}^{\circ} (O_{2}, g)\right]

Here, the \Delta H_{f}^{\circ} (O_{2}, g) = 0 kJ/mol

→ \Delta H_{r}^{\circ} = \left [\Delta H_{f}^{\circ} (H_{2}O_{2}, l) \right ] - \left [\Delta H_{f}^{\circ} (H_{2}O, l)\right] \neq \Delta H_{f}^{\circ} (Products)

b. N₂ (g) + O₂ (g) → 2NO (g)

\Delta H_{r}^{\circ} = \left [2\times \Delta H_{f}^{\circ} (NO, g) \right ] - \left [\Delta H_{f}^{\circ} (N_{2}, g)+\Delta H_{f}^{\circ} (O_{2}, g)\right]

Here, the \Delta H_{f}^{\circ} (O_{2}, g) = \Delta H_{f}^{\circ} (N_{2}, g)= 0 kJ/mol

→ \Delta H_{r}^{\circ} = \left [2\times \Delta H_{f}^{\circ} (NO, g) \right ] \neq \Delta H_{f}^{\circ} (Product, NO)

c. 2H₂ (g) + O₂ (g) → 2H₂O (g)

\Delta H_{r}^{\circ} = \left [2\times \Delta H_{f}^{\circ} (H_{2}O, g) \right ] - \left [2\times \Delta H_{f}^{\circ} (H_{2}, g)+\Delta H_{f}^{\circ} (O_{2}, g)\right]

Here, the \Delta H_{f}^{\circ} (O_{2}, g) = \Delta H_{f}^{\circ} (H_{2}, g)= 0 kJ/mol

→ \Delta H_{r}^{\circ} = \left [2\times \Delta H_{f}^{\circ} (H_{2}O, g) \right ] \neq \Delta H_{f}^{\circ} (Product, H_{2}O)

d. 2H₂ (g) + O₂ (g) → 2H₂O (l)

\Delta H_{r}^{\circ} = \left [2\times \Delta H_{f}^{\circ} (H_{2}O, l) \right ] - \left [2\times \Delta H_{f}^{\circ} (H_{2}, g)+\Delta H_{f}^{\circ} (O_{2}, g)\right]

Here, the \Delta H_{f}^{\circ} (O_{2}, g) = \Delta H_{f}^{\circ} (H_{2}, g)= 0 kJ/mol

→ \Delta H_{r}^{\circ} = \left [2\times \Delta H_{f}^{\circ} (H_{2}O, l) \right ] \neq \Delta H_{f}^{\circ} (Product, H_{2}O)

e. 2C(s, graphite) + 2H₂(g) → C₂H₄ (g)

\Delta H_{r}^{\circ} = \left [\Delta H_{f}^{\circ} (C_{2}H_{4}, g) \right ] - \left [2\times \Delta H_{f}^{\circ} (C, s graphite)+2\times \Delta H_{f}^{\circ} (H_{2}, g)\right]

Here, the \Delta H_{f}^{\circ} (C, s, graphite) = \Delta H_{f}^{\circ} (H_{2}, g)= 0 kJ/mol

→ \Delta H_{r}^{\circ} = \left [\Delta H_{f}^{\circ} (C_{2}H_{4}, g) \right ] = \Delta H_{f}^{\circ} (Product, C_{2}H_{4})

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The chemical formula for the compound containing 8.6 mol of sulfur and 3.42 mol of phosphorus is P₂S₅

<h3>How do I determine the formula of the compound?</h3>

From the question given above, the following data were obatined:

  • Sulphur (S) = 8.6 moles
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The chemical formula of the compound can be obtained as follow:

Divide by their molar mass

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Divide by the smallest

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Thus, the chemical formula is P₂S₅

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