For silver, $C_{p} (J K^{- 1} m o l^{- 1}) = 23 + 0.01 T$ . If the temperature (T) of $3 moles$ of silver is raised from $300 K to 1000 K$ at $1 atm$ pressure, the value of $Δ H$ will be close to:

16 kJ

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21 kJ

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62 kJ

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13 kJ

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Solution

The correct option is C $62 kJ$
Given: n = 3
$T_{1} = 300; T_{2} = 1000$

$C_{p} = 23 + 0.01 T$

$Δ H a n d C_{p}$

$Δ H = T_{2} \int T_{1} n C_{p} d T$

$= Δ H = n 1000 \int 300 (23 + 0.01 T) d T$

$= 3 [23 (1000 - 300) [+ \frac{0.01}{2} (1000^{2} - 300^{2})]]$

$= 3 [16100 + 4550]$

$= 3 \times 20650 = 61950 J$

$\approx 62 kJ$

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Similar questions

Q. For silver

C_{p} (J K^{- 1} m o l^{- 1}) = 23 + 0.01 T

. If the temperature (T) of 3 moles of silver is raised from 300 K to 1000 K at 1 atm pressure, the value of

Δ H

will be close to:

For silver, $C_{p} (J K^{- 1} m o l^{- 1}) = 23 + 0.01 T$ . If the temperature $(T)$ of moles of silver is raised from $300 K$ to $1000 K$ at $1 atm$ pressure, the value of $Δ H$ will be close to:

Q. For silver,

C_{p} (J K^{- 1} m o l^{- 1}) = 23 + 0.01 T

. If the temperature (T) of moles of silver is raised from 300 K to 1000K at 1 atm pressure, the value of

Δ H

will be close to:

Q. For silver

C_{p} (J K^{- 1} m o l^{- 1}) = 23 + 0.01 T

. If the temperature (T) of 3 moles of silver is raised from 300 K to 1000 K at 1 atm pressure, the value of

Δ H

will be close to:

Three mole of Ag is heated from 300 K to 1000 K. Calculate ΔH when P = 1 atm and $C_{P} = 23 + 0.01 T .$

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For silver, Cp(JK−1mol−1)=23+0.01T. If the temperature (T) of 3 moles of silver is raised from 300 K to 1000 K at 1atm pressure, the value of ΔH will be close to:

The correct option is C 62 kJGiven: n = 3 T1=300;T2=1000 Cp=23+0.01T ΔHandCp ΔH=T2∫T1nCpdT =ΔH=n1000∫300(23+0.01T)dT =3[23(1000−300)[+0.012(10002−3002)]] =3[16100+4550] =3×20650=61950 J ≈62 kJ

For silver, $C_{p} (J K^{- 1} m o l^{- 1}) = 23 + 0.01 T$ . If the temperature (T) of $3 moles$ of silver is raised from $300 K to 1000 K$ at $1 atm$ pressure, the value of $Δ H$ will be close to: