What will be the enthalpy change of conversion of graphite into diamond? Given C graphite, ΔcombH=-391.25 kj; Cdiamond, ΔcombH=-393.12 kj

Question

What will be the enthalpy change of conversion of graphite into diamond? Given C graphite, ΔcombH=-391.25 kj; Cdiamond, ΔcombH=-393.12 kj (A) zero (B) -391.25 kj (C) -393.12 kj (D) -1.87 kj

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/b53ac62dc752b7cc16a1ff34e044cc62-.jpeg" /> Δ H = -393.12 - (-391.25) = -1.87 kj

Q. What will be the enthalpy change of conversion of graphite into diamond?
Given
$C_{g r a p hi t e,} Δ_{co mb} H = - 391.25 kj$ ;
$C_{d iam o n d,} Δ_{co mb} H = - 393.12 kj$

zero

$- 391.25 kj$

$- 393.12 kj$

$- 1.87 kj$

$Δ H = - 393.12 - (- 391.25) = - 1.87 kj$

Q. What will be the enthalpy change of conversion of graphite into diamond? Given Cgraphite,​Δcomb​H=−391.25kj; Cdiamond,​Δcomb​H=−393.12kj

zero

−391.25kj

−393.12kj

−1.87kj

ΔH=−393.12−(−391.25)=−1.87kj

Q. What will be the enthalpy change of conversion of graphite into diamond?
Given
$C_{g r a p hi t e,} Δ_{co mb} H = - 391.25 kj$ ;
$C_{d iam o n d,} Δ_{co mb} H = - 393.12 kj$

$- 391.25 kj$

$- 393.12 kj$

$- 1.87 kj$

$Δ H = - 393.12 - (- 391.25) = - 1.87 kj$