The molar heat capacity of water at constant pressure, $C$ , is $75 J K^{- 1} {m o l}^{- 1}$ . When $1.0 K J$ of heat is supplied to $100 g$ of water which is free to expand, the increase in temperature of the water is:

1.2 K

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2.4 K

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4.8 K

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6.6 K

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Solution

The correct option is B $2.4 K$
The relationship between the heat supplied, molar heat capacity at constant volume and the temperature change is

$△ Q = n C_{p} △ T$

we have,
$q = 1 k J = 1000 J$
$number of mole(n)=$ $\frac{100}{18}$

Substitute values in the above expression.
$\Rightarrow 10^{3} = \frac{100}{18} \times 75 \times △ T$
$\Rightarrow △ T = 2.4 K$

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The molar heat capacity of water at constant pressure, C, is 75JK−1mol−1. When 1.0KJ of heat is supplied to 100g of water which is free to expand, the increase in temperature of the water is:

The correct option is B 2.4KThe relationship between the heat supplied, molar heat capacity at constant volume and the temperature change is △Q=nCp△Twe have,q=1kJ=1000Jnumber of mole(n)= 10018Substitute values in the above expression.⇒103=10018×75×△T⇒△T=2.4K

The molar heat capacity of water at constant pressure, $C$ , is $75 J K^{- 1} {m o l}^{- 1}$ . When $1.0 K J$ of heat is supplied to $100 g$ of water which is free to expand, the increase in temperature of the water is: