Heat capacity of water is `18 cal-"degree"^(-1)-mol^(-1)`. The quantity of heat needed to rise temperature of 18 g water by `0.2^(@)C` is x cal. Then amount of `CH_(4(g))` to be burnt to produce X cal heat is
`(CH_(4)+2O_(2) rarr CO_(2)+2H_(2)O, Delta H = -200 K.Cal)`

Options

A. `1.8 xx 10^(-3) mol`
B. `3.4xx 10^(-5) mol`
C. `0.0288 g`
D. `0.288 mg`

Explanation

To solve the problem step by step, we will first calculate the quantity of heat needed to raise the temperature of 18 g of water by 0.2°C and then determine how much methane (CH₄) must be burned to produce that amount of heat.

### Step 1: Calculate the amount of heat (Q) required to raise the temperature of water.

The formula to calculate the heat required is:

\[ Q = m \times C \times \Delta T \]

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