(C) Given:Weight of aluminium $(w) = 54 \ g$Temperature difference $(\Delta T) = 60^{\circ}C - 40^{\circ}C = 20 \ K$ (or $20^{\circ}C$)Molar heat capa

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(C) Given:Weight of aluminium $(w) = 54 \ g$Temperature difference $(\Delta T) = 60^{\circ}C - 40^{\circ}C = 20 \ K$ (or $20^{\circ}C$)Molar heat capacity of aluminium $(C_m) = 24 \ J \ mol^{-1} \ K^{-1}$Atomic mass of $Al$ $(M) = 27 \ g \ mol^{-1}$Number of moles of $Al$ $(n) = \frac{w}{M} = \frac{54}{27} = 2 \ mol$Heat required $(Q) = n \times C_m \times \Delta T$$Q = 2 \times 24 \times 20 = 960 \ J$Hence,option $(C)$ is the correct answer.

Class 11 Chemistry Thermodynamics Heat capacity

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The heat required to raise the temperature of $54 \ g$ of aluminium from $40^{\circ}C$ to $60^{\circ}C$ in $J$ is (molar heat capacity of aluminium in this temperature range is $24 \ J \ mol^{-1} \ K^{-1}$; atomic weight of $Al$ is $27$).

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A
$480$
B
$800$
C
$960$
D
$1280$

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At constant volume,$4 \; mol$ of an ideal gas when heated from $300 \; K$ to $500 \; K$ changes its internal energy by $5000 \; J$. The molar heat capacity at constant volume is ............... $J \; mol^{-1} \; K^{-1}$

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What is heat capacity?

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$4.48 \ L$ of an ideal gas at $1 \ atm$ and $273 \ K$ requires $12 \ cal$ to raise the temperature by $15 \ ^\circ C$ at constant volume. The $C_p$ of the gas is $... \ cal \ mol^{-1} K^{-1}$.

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The heat required to raise the temperature of $54 \ g$ of aluminium from $40^{\circ}C$ to $60^{\circ}C$ in $J$ is (molar heat capacity of aluminium in this temperature range is $24 \ J \ mol^{-1} \ K^{-1}$; atomic weight of $Al$ is $27$).

Similar Questions

For the reaction ${H_2}_{(g)} + \frac{1}{2}{O_2}_{(g)} \to {H_2}O(\ell)$,given $\Delta C_P = 7.63 \, cal/deg$ and $\Delta H_{25\,^{\circ}C} = 68.3 \, Kcal$,find the value of $\Delta H$ at $100\,^{\circ}C$ (in $Kcal$).

What is the value of ${\left[ {\partial U/\partial T} \right]_V}$ for $He$ gas?

At constant volume,$4 \; mol$ of an ideal gas when heated from $300 \; K$ to $500 \; K$ changes its internal energy by $5000 \; J$. The molar heat capacity at constant volume is ............... $J \; mol^{-1} \; K^{-1}$

What is heat capacity?

$4.48 \ L$ of an ideal gas at $1 \ atm$ and $273 \ K$ requires $12 \ cal$ to raise the temperature by $15 \ ^\circ C$ at constant volume. The $C_p$ of the gas is $... \ cal \ mol^{-1} K^{-1}$.

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