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The standard enthalpies fo formation of ...

The standard enthalpies fo formation of `CO_(2) (g), H_(2) O (1)`, and glucose (s) at `25^(@)C` are `- 400 kJ mol^(-1), - 300 kJ mol^(-)`, and `- 1300 kJ mol^(-1)`, respectively. The standard enthalply of combustion per gram of glucose at `25^(@)C` is

A

`+ 16.11 kJ`

B

`- 16.11 kJ`

C

`+ 2900 kJ`

D

`- 2900 kJ`

Text Solution

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The correct Answer is:
To find the standard enthalpy of combustion per gram of glucose at 25°C, we will follow these steps: ### Step 1: Write the combustion reaction of glucose The combustion reaction of glucose (C₆H₁₂O₆) can be represented as: \[ C_6H_{12}O_6 (s) + 6 O_2 (g) \rightarrow 6 CO_2 (g) + 6 H_2O (l) \] ### Step 2: Use the standard enthalpy of formation values We know the standard enthalpies of formation for the substances involved: - \( \Delta H_f^\circ \) for \( CO_2 (g) = -400 \, \text{kJ/mol} \) - \( \Delta H_f^\circ \) for \( H_2O (l) = -300 \, \text{kJ/mol} \) - \( \Delta H_f^\circ \) for \( C_6H_{12}O_6 (s) = -1300 \, \text{kJ/mol} \) ### Step 3: Calculate the enthalpy change for the combustion reaction Using the formula: \[ \Delta H_{reaction} = \sum (\Delta H_f^\circ \text{ of products}) - \sum (\Delta H_f^\circ \text{ of reactants}) \] For the products: - \( 6 \times \Delta H_f^\circ (CO_2) + 6 \times \Delta H_f^\circ (H_2O) \) - \( = 6 \times (-400) + 6 \times (-300) \) - \( = -2400 - 1800 = -4200 \, \text{kJ} \) For the reactants: - \( \Delta H_f^\circ (C_6H_{12}O_6) + 6 \times \Delta H_f^\circ (O_2) \) - Since \( O_2 \) is in its standard state, its enthalpy of formation is 0. - \( = -1300 + 0 = -1300 \, \text{kJ} \) Now, substituting these values into the reaction enthalpy equation: \[ \Delta H_{reaction} = -4200 - (-1300) \] \[ = -4200 + 1300 = -2900 \, \text{kJ} \] ### Step 4: Calculate the enthalpy of combustion per gram of glucose We know that the enthalpy change calculated is for 1 mole of glucose (180 g). To find the enthalpy of combustion per gram: \[ \text{Enthalpy of combustion per gram} = \frac{-2900 \, \text{kJ}}{180 \, \text{g}} \] \[ = -16.11 \, \text{kJ/g} \] ### Final Answer The standard enthalpy of combustion per gram of glucose at 25°C is: \[ \boxed{-16.11 \, \text{kJ/g}} \]

To find the standard enthalpy of combustion per gram of glucose at 25°C, we will follow these steps: ### Step 1: Write the combustion reaction of glucose The combustion reaction of glucose (C₆H₁₂O₆) can be represented as: \[ C_6H_{12}O_6 (s) + 6 O_2 (g) \rightarrow 6 CO_2 (g) + 6 H_2O (l) \] ...
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The standard enthalpies of formation of CO_(2)(g), H_(2)O(l) and glucose (s)at 25^(@)C are -400 kJ //mol, - 300 kJ//mol and -1300kJ//mol respectively.The standard enthalpy of combustion per gram of glucose at 25^(@)C is

The standard enthalpies of formation of CO_(2)(g),H_(2)O(l) and glucose(s) at 25^(@)C are -400 kJ/mol. -300kJ/mol and -1300 kJ/mol, respectively. The standard enthalpy of cumbusion per gram of glucose at 25^(@)C is

Knowledge Check

  • The standard enthalpy of formation of CO_(2)(g) , H_(2)O(l) and glucose (s) at 25^(@)C are -400.0 kJ mol^(-1),-300.0 kJ mol^(-1) and -1300.0 kJ mol^(-1) respectively. The standard enthalpy of combustion per gram of glucose at 25^(@)C is

    A
    `+ 2900 kJ`
    B
    `- 2900 kJ`
    C
    `- 16.11 kJ`
    D
    `+ 16.11 kJ`
  • The standard enthalpies of formation of CO_(2)(g), H_(2)O(l) and glucose (s) at 25^(@)C are -400 kJ/mol, -300 kJ/mol and -1300 kJ/mol, respectively. The standard enthalpy of combustion per gram of glucose at 25^(@)C is :

    A
    `+2900 kJ`
    B
    `-2900 kJ`
    C
    `-16.11 kJ`
    D
    `+16.11 kJ`
  • The standard enthalpies of formation of CO_(2)(g), H_(2)O(l) and glucose(s) at 25^(@)C are -400kJ//mol, -300 kJ//mol and -1300 kJ//mol , respectively. The standard enthalpy of combustion per gram of glucose at 25^(@)C is

    A
    `+2900 kJ`
    B
    `-2900 kJ`
    C
    `-16.11 kJ`
    D
    `+16.11 kJ`
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