The molar heat capacity of water at constant | vedclass

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Question

(C) The relationship between the heat supplied $(q)$,molar heat capacity at constant pressure $(C_p)$,and the temperature change $(\Delta T)$ is given

Vedclass · Accepted Answer

$2.4$

Vedclass · Answer

(C) The relationship between the heat supplied $(q)$,molar heat capacity at constant pressure $(C_p)$,and the temperature change $(\Delta T)$ is given by the formula: $q = n \cdot C_p \cdot \Delta T$Given:$q = 1.0 \, kJ = 1000 \, J$$C_p = 75 \, J \, K^{-1} \, mol^{-1}$Mass of water = $100 \, g$Molar mass of water $(H_2O)$ = $18 \, g \, mol^{-1}$Calculate the number of moles $(n)$:$n = \frac{	ext{mass}}{	ext{molar mass}} = \frac{100 \, g}{18 \, g \, mol^{-1}} = 5.55 \, mol$Substitute the values into the formula:$1000 = (\frac{100}{18}) 	imes 75 	imes \Delta T$$1000 = 5.55 	imes 75 	imes \Delta T$$1000 = 416.67 	imes \Delta T$$\Delta T = \frac{1000}{416.67} \approx 2.4 \, K$Therefore,the increase in temperature is $2.4 \, K$.

The molar heat capacity of water at constant pressure is $75 \, J \, K^{-1} \, mol^{-1}$. When $1.0 \, kJ$ of heat is supplied to $100 \, g$ of water which is free to expand,the increase in temperature of water is (in $, K$)

Similar Questions

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

Specific heat capacity is defined as:

The heat required to raise the temperature of a body by $1 \, K$ is called

The heat required to raise the temperature of $1 \ mol$ of a substance by $1^{\circ}C$ is called:

$C_P$ is always greater than $C_V$ for an ideal gas. Choose the correct option.

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