The standard enthalpy required to completely decompose 1.00 g of tin (II)chloride into tin and chlorine is ± KJ.

To determine the standard enthalpy change (ΔH) for the decomposition of tin(II) chloride (SnCl₂) into its elements (tin and chlorine), we need to find the enthalpy change for the following reaction:

\[ \text{SnCl}_2 (s) \rightarrow \text{Sn} (s) + \text{Cl}_2 (g) \]

The standard enthalpy change of formation (ΔH_f°) for a compound can be used to calculate the enthalpy change of the reaction. The ΔH_f° values are typically found in standard tables. The enthalpy change of the reaction is calculated using the formula:

\[ \Delta H_{\text{reaction}}^\circ = \sum \Delta H_f^\circ \text{(products)} - \sum \Delta H_f^\circ \text{(reactants)} \]

Here, we assume standard conditions (298 K, 1 atm). 

1. Look up the standard enthalpy of formation (ΔH_f°) for each species involved:
   - \(\Delta H_f^\circ (\text{SnCl}_2 (s)) = -350.9 \, \text{kJ/mol}\)
   - \(\Delta H_f^\circ (\text{Sn} (s)) = 0 \, \text{kJ/mol}\) (standard state)
   - \(\Delta H_f^\circ (\text{Cl}_2 (g)) = 0 \, \text{kJ/mol}\) (standard state)

2. Calculate the enthalpy change for the reaction:

\[ \Delta H_{\text{reaction}}^\circ = [\Delta H_f^\circ (\text{Sn} (s)) + \Delta H_f^\circ (\text{Cl}_2 (g))] - [\Delta H_f^\circ (\text{SnCl}_2 (s))] \]

\[ \Delta H_{\text{reaction}}^\circ = [0 + 0] - [-350.9] \]

\[ \Delta H_{\text{reaction}}^\circ = 350.9 \, \text{kJ/mol} \]

3. To find the enthalpy change for 1.00 g of SnCl₂, first determine the molar mass of SnCl₂:
   - Sn: 118.71 g/mol
   - Cl: 35.45 g/mol × 2 = 70.90 g/mol
   - Total molar mass of SnCl₂ = 118.71 + 70.90 = 189.61 g/mol

4. Calculate the number of moles in 1.00 g of SnCl₂:

\[ \text{moles of SnCl}_2 = \frac{1.00 \, \text{g}}{189.61 \, \text{g/mol}} = 0.00527 \, \text{mol} \]

5. Finally, calculate the enthalpy change for 1.00 g of SnCl₂:

\[ \Delta H = 0.00527 \, \text{mol} \times 350.9 \, \text{kJ/mol} = 1.85 \, \text{kJ} \]

So, the standard enthalpy required to completely decompose 1.00 g of tin(II) chloride into tin and chlorine is approximately ± 1.85 kJ.

Would you like further details or have any questions?

Here are 5 questions you might ask:
1. How do you find the standard enthalpy of formation for a compound?
2. What is the significance of the standard state in enthalpy calculations?
3. Can you explain how to balance chemical equations for enthalpy calculations?
4. How does the enthalpy change relate to the stability of compounds?
5. What are some practical applications of enthalpy calculations in chemistry?

**Tip:** Always make sure to use the correct units and conversion factors when performing thermochemical calculations. This ensures accuracy in your results.

Learn how to calculate the standard enthalpy change for decomposing 1.00 g of tin(II) chloride into tin and chlorine. This problem involves thermochemical calculations using standard enthalpy of formation values and stoichiometric principles. Suitable for undergraduate-level chemistry students.

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