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.

Question

Vikas TU · Answer

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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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.

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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.

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