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1.372g g of urea is burned in a bomb calorimeter with a net heat capacity of 5.00 kJ/K. A temperature rise of 2.95 K is observed. What volume change will occur if the combustion of 1 mole of urea was carried out at constant pressure of 1 atm. And what is the value of the enthalpy change in kJ/mole.

1.372g g of urea is burned in a bomb calorimeter with a net heat capacity of 5.00 kJ/K. A temperature rise of 2.95 K is observed. What volume change will occur if the combustion of 1 mole of urea was carried out at constant pressure of 1 atm. And what is the value of the enthalpy change in kJ/mole. 
 

Grade:12

1 Answers

Vikas TU
14149 Points
3 years ago

Bomb calorimetry is utilized to decide the enthalpy of ignition, combH, for hydrocarbons: 
Cp = wh/mt 
Cp = 1.372 x 5.00/60.6 ( mass of solute) * 2.95 
0.3394l volume chane willoccur. 
Particular warmth at consistent weight 
H= Enthalpy of arrangement 
T= Change in temperature 
W= mass of solute 
M= atomic mass of solute 

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