I Review I Constants I Periodic Table Standard Enthalpy of Formation at 289 K Substance Formula AH; (kJ/mol) Part A Hydrogen HBr(g) -36.26 Hypochlorous acid (HOCI) can decompose in the gas phase according to the following balanced equation: bromide Hydrogen chloride HCI(g) -92.30 2 HOCI(g) → 2 HCI(g) + O2(g) AH = -31.0 kJ (T = 298 K, P = 1 atm) Hydrogen fluoride HF(g) -268.60 Using the enthalpy of this reaction and data in the following table, calculate the standard enthalpy of formation for HOCI(g). Hydrogen iodide HI(g) 25.9 Methane CH4(g) -74.80 O -123 kJ/mol +61.3 kJ/mol Water vapor H20(g) -241.8 -76.8 kJ/mol -154 kJ/mol O +76.8 kJ/mol Submit Request Answer

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### Standard Enthalpy of Formation at 289 K

| Substance         | Formula | \(\Delta H_f^\circ \) (kJ/mol) |
|-------------------|---------|------------------------------|
| Hydrogen bromide  | HBr(g)  | -36.26                       |
| Hydrogen chloride | HCl(g)  | -92.30                       |
| Hydrogen fluoride | HF(g)   | -268.60                      |
| Hydrogen iodide   | HI(g)   | 25.9                         |
| Methane           | CH\(_4\)(g)| -74.80                     |
| Water vapor       | H\(_2\)O(g)| -241.8                     |

### Part A

Hypochlorous acid (HOCl) can decompose in the gas phase according to the following balanced equation:

\[ 2 \text{ HOCl(g) } \rightarrow 2 \text{ HCl(g) } + \text{ O}_2\text{(g) } \]

\[\Delta H = -31.0 \text{ kJ} \, (T = 298 \text{ K}, P = 1 \text{ atm})\]

Using the enthalpy of this reaction and data in the following table, calculate the standard enthalpy of formation for HOCl(g).

**Options:**

- \(-123 \text{ kJ/mol}\)
- \(+61.3 \text{ kJ/mol}\)
- \(-76.8 \text{ kJ/mol}\)
- \(-154 \text{ kJ/mol}\)
- \(+76.8 \text{ kJ/mol}\)

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Transcribed Image Text:### Standard Enthalpy of Formation at 289 K | Substance | Formula | \(\Delta H_f^\circ \) (kJ/mol) | |-------------------|---------|------------------------------| | Hydrogen bromide | HBr(g) | -36.26 | | Hydrogen chloride | HCl(g) | -92.30 | | Hydrogen fluoride | HF(g) | -268.60 | | Hydrogen iodide | HI(g) | 25.9 | | Methane | CH\(_4\)(g)| -74.80 | | Water vapor | H\(_2\)O(g)| -241.8 | ### Part A Hypochlorous acid (HOCl) can decompose in the gas phase according to the following balanced equation: \[ 2 \text{ HOCl(g) } \rightarrow 2 \text{ HCl(g) } + \text{ O}_2\text{(g) } \] \[\Delta H = -31.0 \text{ kJ} \, (T = 298 \text{ K}, P = 1 \text{ atm})\] Using the enthalpy of this reaction and data in the following table, calculate the standard enthalpy of formation for HOCl(g). **Options:** - \(-123 \text{ kJ/mol}\) - \(+61.3 \text{ kJ/mol}\) - \(-76.8 \text{ kJ/mol}\) - \(-154 \text{ kJ/mol}\) - \(+76.8 \text{ kJ/mol}\) **Submit:** [Submit Button] **Feedback:** [Provide Feedback Link]
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