4 g of graphite is burnt in a bomb calorimeter of heat capacity 30 kJ K -1. In excess of oxygen at 1 atm pressure the temperature rises from 300 K to 304 K. What is the enthalpy of combustion of graphite (in kJ mol -1 )?

Question

4 g of graphite is burnt in a bomb calorimeter of heat capacity 30 kJ K -1. In excess of oxygen at 1 atm pressure the temperature rises from 300 K to 304 K. What is the enthalpy of combustion of graphite (in kJ mol -1 )? (A) 360 (B) 1440 (C) -360 (D) -1440

Tardigrade Admin · Accepted Answer

C +1 / 2 O 2 arrow CO Δ H =30 × 4 × 3 kJ mol =360 kJ mol -1

Q. $4 g$ of graphite is burnt in a bomb calorimeter of heat capacity $30 k J K^{- 1}$ . In excess of oxygen at 1 atm pressure the temperature rises from $300 K$ to $304 K$ . What is the enthalpy of combustion of graphite (in $k J m o l^{- 1}$ )?

360

1440

-360

-1440

$C + 1/2 O_{2} \to CO$
$Δ H = 30 \times 4 \times 3 k J m o l = 360 k J m o l^{- 1}$

Q. 4g of graphite is burnt in a bomb calorimeter of heat capacity 30kJK−1. In excess of oxygen at 1 atm pressure the temperature rises from 300K to 304K. What is the enthalpy of combustion of graphite (in kJmol−1 )?

360

1440

-360

-1440

C+1/2O2​→CO ΔH=30×4×3kJmol=360kJmol−1

Q. $4 g$ of graphite is burnt in a bomb calorimeter of heat capacity $30 k J K^{- 1}$ . In excess of oxygen at 1 atm pressure the temperature rises from $300 K$ to $304 K$ . What is the enthalpy of combustion of graphite (in $k J m o l^{- 1}$ )?

$C + 1/2 O_{2} \to CO$
$Δ H = 30 \times 4 \times 3 k J m o l = 360 k J m o l^{- 1}$