369186 One gram sample of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) is decomposed in a bomb calorimeter. The temperature of the calorimeter increased by 6.12 K . The heat capacity of the system is \(1.23 \mathrm{~kJ} / \mathrm{g}^{-1} \mathrm{~K}^{-1}\). What is the molar heat of decomposition for \(\mathrm{NH}_{4} \mathrm{NO}_{3}\).

369187 \(\mathrm{1 \mathrm{~g}}\) of graphite is burnt in a bomb calorimeter in excess of oxygen at \(\mathrm{298 \mathrm{~K}}\) and \(\mathrm{1 \mathrm{~atm}}\). pressure according to the equation
\(\mathrm{\mathrm{C}_{\text {(graphite) }}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}}\)
During the reaction, temperature rises from 298 \(\mathrm{\mathrm{K}}\) to \(\mathrm{299 \mathrm{~K}}\). If the heat capacity of the bomb calorimeter is \(\mathrm{20.7 \mathrm{~kJ} / \mathrm{K}}\), what is the enthalpy change for the above reaction at \(\mathrm{298 \mathrm{~K}}\) and 1 atm?

369188 \(\Delta_{\mathrm{f}} \mathrm{H}^{\circ}\) of hypothetical \(\mathrm{MX}\) is \(-250 \mathrm{~kJ} \mathrm{~mol}^{-1}\) and for \(\mathrm{MX}_{2}\) is \(-600 \mathrm{~kJ} \mathrm{~mol}^{-1}\). The enthalpy of disproportionation of \(\mathrm{MX}\) is \( - 100\,{\rm{x}}\;{\rm{kJ}}\;{\rm{mo}}{{\rm{l}}^{ - 1}}.\) Find the value of x.

369189 \(4 \mathrm{~g}\) of graphite is burnt in a bomb calorimeter of heat capacity \(30 \mathrm{~kJ} \mathrm{~K}^{-1}\) in excess of oxygen at \(1 \mathrm{~atm}\) pressure. The temperature rises from 300 \(\mathrm{K}\) to \(304 \mathrm{~K}\). What is the enthalpy of combustion of graphite \(\left( {in} \right.\left. {{\text{ kJ mo}}{{\text{l}}^{ - 1}}} \right)\) ?

369190 When 0.50 g of unknown carbon compound is burned in the bomb calorimeter, its temperature rises by \({\mathrm{6.76{ }^{\circ} \mathrm{C}}}\). How much energy (in kilojoules) is released during combustion? (Heat capacity of calorimeter \({\mathrm{=3.64 \mathrm{~kJ}^{\circ} \mathrm{C}^{-1} \mathrm{~g}^{-1}}}\) )

369186 One gram sample of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) is decomposed in a bomb calorimeter. The temperature of the calorimeter increased by 6.12 K . The heat capacity of the system is \(1.23 \mathrm{~kJ} / \mathrm{g}^{-1} \mathrm{~K}^{-1}\). What is the molar heat of decomposition for \(\mathrm{NH}_{4} \mathrm{NO}_{3}\).

369187 \(\mathrm{1 \mathrm{~g}}\) of graphite is burnt in a bomb calorimeter in excess of oxygen at \(\mathrm{298 \mathrm{~K}}\) and \(\mathrm{1 \mathrm{~atm}}\). pressure according to the equation
\(\mathrm{\mathrm{C}_{\text {(graphite) }}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}}\)
During the reaction, temperature rises from 298 \(\mathrm{\mathrm{K}}\) to \(\mathrm{299 \mathrm{~K}}\). If the heat capacity of the bomb calorimeter is \(\mathrm{20.7 \mathrm{~kJ} / \mathrm{K}}\), what is the enthalpy change for the above reaction at \(\mathrm{298 \mathrm{~K}}\) and 1 atm?

369188 \(\Delta_{\mathrm{f}} \mathrm{H}^{\circ}\) of hypothetical \(\mathrm{MX}\) is \(-250 \mathrm{~kJ} \mathrm{~mol}^{-1}\) and for \(\mathrm{MX}_{2}\) is \(-600 \mathrm{~kJ} \mathrm{~mol}^{-1}\). The enthalpy of disproportionation of \(\mathrm{MX}\) is \( - 100\,{\rm{x}}\;{\rm{kJ}}\;{\rm{mo}}{{\rm{l}}^{ - 1}}.\) Find the value of x.

369189 \(4 \mathrm{~g}\) of graphite is burnt in a bomb calorimeter of heat capacity \(30 \mathrm{~kJ} \mathrm{~K}^{-1}\) in excess of oxygen at \(1 \mathrm{~atm}\) pressure. The temperature rises from 300 \(\mathrm{K}\) to \(304 \mathrm{~K}\). What is the enthalpy of combustion of graphite \(\left( {in} \right.\left. {{\text{ kJ mo}}{{\text{l}}^{ - 1}}} \right)\) ?

369190 When 0.50 g of unknown carbon compound is burned in the bomb calorimeter, its temperature rises by \({\mathrm{6.76{ }^{\circ} \mathrm{C}}}\). How much energy (in kilojoules) is released during combustion? (Heat capacity of calorimeter \({\mathrm{=3.64 \mathrm{~kJ}^{\circ} \mathrm{C}^{-1} \mathrm{~g}^{-1}}}\) )

369186 One gram sample of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) is decomposed in a bomb calorimeter. The temperature of the calorimeter increased by 6.12 K . The heat capacity of the system is \(1.23 \mathrm{~kJ} / \mathrm{g}^{-1} \mathrm{~K}^{-1}\). What is the molar heat of decomposition for \(\mathrm{NH}_{4} \mathrm{NO}_{3}\).

369187 \(\mathrm{1 \mathrm{~g}}\) of graphite is burnt in a bomb calorimeter in excess of oxygen at \(\mathrm{298 \mathrm{~K}}\) and \(\mathrm{1 \mathrm{~atm}}\). pressure according to the equation
\(\mathrm{\mathrm{C}_{\text {(graphite) }}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}}\)
During the reaction, temperature rises from 298 \(\mathrm{\mathrm{K}}\) to \(\mathrm{299 \mathrm{~K}}\). If the heat capacity of the bomb calorimeter is \(\mathrm{20.7 \mathrm{~kJ} / \mathrm{K}}\), what is the enthalpy change for the above reaction at \(\mathrm{298 \mathrm{~K}}\) and 1 atm?

369188 \(\Delta_{\mathrm{f}} \mathrm{H}^{\circ}\) of hypothetical \(\mathrm{MX}\) is \(-250 \mathrm{~kJ} \mathrm{~mol}^{-1}\) and for \(\mathrm{MX}_{2}\) is \(-600 \mathrm{~kJ} \mathrm{~mol}^{-1}\). The enthalpy of disproportionation of \(\mathrm{MX}\) is \( - 100\,{\rm{x}}\;{\rm{kJ}}\;{\rm{mo}}{{\rm{l}}^{ - 1}}.\) Find the value of x.

369189 \(4 \mathrm{~g}\) of graphite is burnt in a bomb calorimeter of heat capacity \(30 \mathrm{~kJ} \mathrm{~K}^{-1}\) in excess of oxygen at \(1 \mathrm{~atm}\) pressure. The temperature rises from 300 \(\mathrm{K}\) to \(304 \mathrm{~K}\). What is the enthalpy of combustion of graphite \(\left( {in} \right.\left. {{\text{ kJ mo}}{{\text{l}}^{ - 1}}} \right)\) ?

369190 When 0.50 g of unknown carbon compound is burned in the bomb calorimeter, its temperature rises by \({\mathrm{6.76{ }^{\circ} \mathrm{C}}}\). How much energy (in kilojoules) is released during combustion? (Heat capacity of calorimeter \({\mathrm{=3.64 \mathrm{~kJ}^{\circ} \mathrm{C}^{-1} \mathrm{~g}^{-1}}}\) )

369186 One gram sample of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) is decomposed in a bomb calorimeter. The temperature of the calorimeter increased by 6.12 K . The heat capacity of the system is \(1.23 \mathrm{~kJ} / \mathrm{g}^{-1} \mathrm{~K}^{-1}\). What is the molar heat of decomposition for \(\mathrm{NH}_{4} \mathrm{NO}_{3}\).

369187 \(\mathrm{1 \mathrm{~g}}\) of graphite is burnt in a bomb calorimeter in excess of oxygen at \(\mathrm{298 \mathrm{~K}}\) and \(\mathrm{1 \mathrm{~atm}}\). pressure according to the equation
\(\mathrm{\mathrm{C}_{\text {(graphite) }}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}}\)
During the reaction, temperature rises from 298 \(\mathrm{\mathrm{K}}\) to \(\mathrm{299 \mathrm{~K}}\). If the heat capacity of the bomb calorimeter is \(\mathrm{20.7 \mathrm{~kJ} / \mathrm{K}}\), what is the enthalpy change for the above reaction at \(\mathrm{298 \mathrm{~K}}\) and 1 atm?

369188 \(\Delta_{\mathrm{f}} \mathrm{H}^{\circ}\) of hypothetical \(\mathrm{MX}\) is \(-250 \mathrm{~kJ} \mathrm{~mol}^{-1}\) and for \(\mathrm{MX}_{2}\) is \(-600 \mathrm{~kJ} \mathrm{~mol}^{-1}\). The enthalpy of disproportionation of \(\mathrm{MX}\) is \( - 100\,{\rm{x}}\;{\rm{kJ}}\;{\rm{mo}}{{\rm{l}}^{ - 1}}.\) Find the value of x.

369189 \(4 \mathrm{~g}\) of graphite is burnt in a bomb calorimeter of heat capacity \(30 \mathrm{~kJ} \mathrm{~K}^{-1}\) in excess of oxygen at \(1 \mathrm{~atm}\) pressure. The temperature rises from 300 \(\mathrm{K}\) to \(304 \mathrm{~K}\). What is the enthalpy of combustion of graphite \(\left( {in} \right.\left. {{\text{ kJ mo}}{{\text{l}}^{ - 1}}} \right)\) ?

369190 When 0.50 g of unknown carbon compound is burned in the bomb calorimeter, its temperature rises by \({\mathrm{6.76{ }^{\circ} \mathrm{C}}}\). How much energy (in kilojoules) is released during combustion? (Heat capacity of calorimeter \({\mathrm{=3.64 \mathrm{~kJ}^{\circ} \mathrm{C}^{-1} \mathrm{~g}^{-1}}}\) )

369186 One gram sample of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) is decomposed in a bomb calorimeter. The temperature of the calorimeter increased by 6.12 K . The heat capacity of the system is \(1.23 \mathrm{~kJ} / \mathrm{g}^{-1} \mathrm{~K}^{-1}\). What is the molar heat of decomposition for \(\mathrm{NH}_{4} \mathrm{NO}_{3}\).

369187 \(\mathrm{1 \mathrm{~g}}\) of graphite is burnt in a bomb calorimeter in excess of oxygen at \(\mathrm{298 \mathrm{~K}}\) and \(\mathrm{1 \mathrm{~atm}}\). pressure according to the equation
\(\mathrm{\mathrm{C}_{\text {(graphite) }}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}}\)
During the reaction, temperature rises from 298 \(\mathrm{\mathrm{K}}\) to \(\mathrm{299 \mathrm{~K}}\). If the heat capacity of the bomb calorimeter is \(\mathrm{20.7 \mathrm{~kJ} / \mathrm{K}}\), what is the enthalpy change for the above reaction at \(\mathrm{298 \mathrm{~K}}\) and 1 atm?

369188 \(\Delta_{\mathrm{f}} \mathrm{H}^{\circ}\) of hypothetical \(\mathrm{MX}\) is \(-250 \mathrm{~kJ} \mathrm{~mol}^{-1}\) and for \(\mathrm{MX}_{2}\) is \(-600 \mathrm{~kJ} \mathrm{~mol}^{-1}\). The enthalpy of disproportionation of \(\mathrm{MX}\) is \( - 100\,{\rm{x}}\;{\rm{kJ}}\;{\rm{mo}}{{\rm{l}}^{ - 1}}.\) Find the value of x.

369189 \(4 \mathrm{~g}\) of graphite is burnt in a bomb calorimeter of heat capacity \(30 \mathrm{~kJ} \mathrm{~K}^{-1}\) in excess of oxygen at \(1 \mathrm{~atm}\) pressure. The temperature rises from 300 \(\mathrm{K}\) to \(304 \mathrm{~K}\). What is the enthalpy of combustion of graphite \(\left( {in} \right.\left. {{\text{ kJ mo}}{{\text{l}}^{ - 1}}} \right)\) ?

369190 When 0.50 g of unknown carbon compound is burned in the bomb calorimeter, its temperature rises by \({\mathrm{6.76{ }^{\circ} \mathrm{C}}}\). How much energy (in kilojoules) is released during combustion? (Heat capacity of calorimeter \({\mathrm{=3.64 \mathrm{~kJ}^{\circ} \mathrm{C}^{-1} \mathrm{~g}^{-1}}}\) )