Calculate the standard Gibbs enegry change for the combustion of `alpha-D` glucose at `300K`.
`C_(6)H_(12)O_(6)(s) +6O_(2)(g) rarr 6CO_(2)(g) +6H_(2)O(l)`
Given the standard enthalpies of formation `(kJ mol^(-1))`
`C_(6)H_(12)O_(6) =- 1274.5, CO_(2) =- 393.5, H_(2)O =- 285.8`.
Entropies `(J K mol^(-1))`
`C_(6)H_(12)O_(6) = 212.1, O_(2) = 205.0, CO_(2) =213, H_(2)O = 69.9`

Explanation

To calculate the standard Gibbs energy change for the combustion of α-D-glucose at 300 K, we will follow these steps:

### Step 1: Write the Balanced Chemical Equation
The combustion reaction of α-D-glucose can be written as:
\[ \text{C}_6\text{H}_{12}\text{O}_6(s) + 6\text{O}_2(g) \rightarrow 6\text{CO}_2(g) + 6\text{H}_2\text{O}(l) \]

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