The enthalpy change for chemical reaction is denoted as `DeltaH^(Theta)` and `DeltaH^(Theta) = H_(P)^(Theta) - H_(R)^(Theta)`. The relation between enthalpy and internal enegry is expressed by equation:
`DeltaH = DeltaU +DeltanRT`
where `DeltaU =` change in internal enegry `Deltan =` change in number of moles, `R =` gas constant.
For the change, `C_("diamond") rarr C_("graphite"), DeltaH =- 1.89 kJ`, if `6g` of diamond and `6g` of graphite are seperately burnt to yield `CO_(2)` the heat liberated in first case is

Options

A. Less than in the second case by `1.89 kJ`
B. Less than in the second case by `11.34 kJ`
C. Less than in the second case by `14.34 kJ`
D. More than in the second case by `0.945 kJ`

Explanation

To solve the problem, we need to determine the heat liberated when 6 g of diamond and 6 g of graphite are separately burnt to yield CO2. We will use the given enthalpy change for the conversion of diamond to graphite and the enthalpy change for the combustion of carbon.

### Step-by-Step Solution:

1. **Identify the reactions:**
- The combustion of graphite can be represented as:
\[
C_{\text{graphite}} + O_2 \rightarrow CO_2
...