369173 A sample of oxygen gas expands its volume from \(\mathrm{3 \mathrm{~L}}\) to \(\mathrm{5 \mathrm{~L}}\) against a constant pressure of \(\mathrm{3 \mathrm{~atm}}\). If the work done during expansion is used to heat \(\mathrm{10 \mathrm{~mol}}\) of water initially present at \(\mathrm{290 \mathrm{~K}}\), its final temperature will be (specific heat capacity of water \({\rm{ = 4}}{\rm{.184}}{\mkern 1mu} {\rm{J}}{\mkern 1mu} {{\rm{K}}^{{\rm{ - 1}}}}{{\rm{g}}^{{\rm{ - 1}}}}{\rm{,1}}\;{\rm{L}}\;{\mkern 1mu} {\rm{atm = 101}}{\rm{.3}}{\mkern 1mu} {\rm{J}}\))

369174 The number of \(\mathrm{\mathrm{kJ}}\) of heat necessary to raise the temperature of \(\mathrm{60.0 \mathrm{~g}}\) of aluminium from \(\mathrm{35^{\circ} \mathrm{C}}\) to \(\mathrm{55^{\circ} \mathrm{C}}\), is, Molar heat capacity of \(\mathrm{\mathrm{Al}}\) is \(\mathrm{24 \mathrm{~J}}\) \(\mathrm{\mathrm{mol}^{-1} \mathrm{~K}^{-1}}\).

369175 0.06 mole of \(\mathrm{\mathrm{KNO}_{3}}\) solid is added to \(\mathrm{100 \mathrm{~cm}^{3}}\) of water at \(\mathrm{298 \mathrm{~K}}\). The enthalpy of \({\rm{KN}}{{\rm{O}}_{\rm{3}}}\left( {{\rm{aq}}} \right)\) solution is \(\mathrm{35.8 \mathrm{~kJ} \mathrm{~mol}^{-1}}\). After the solute is dissolved the temperature of the solutions will be

369176 Work done in the expansion of an ideal gas from \({\rm{4}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) to \({\rm{6}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) against a constant external pressure of \(\mathrm{2.5 \mathrm{~atm}}\) was used to heat up 1 mole of water at \(\mathrm{20^{\circ} \mathrm{C}}\). The final temperature of water will be (Take specific heat of water as\({\rm{4}}{\rm{.2J}}{{\rm{g}}^{{\rm{ - 1}}}}\;{{\rm{K}}^{{\rm{ - 1}}}}\))

369177 A block of Telfon plastic weighing \(\mathrm{16 \mathrm{~g}}\) was heated to \(\mathrm{90^{\circ} \mathrm{C}}\) and then put into a calorimeter containing \(\mathrm{50.0 \mathrm{~g}}\) of water at \(\mathrm{20^{\circ} \mathrm{C}}\). The system reached a temperature at \(\mathrm{30^{\circ} \mathrm{C}}\). The specific heat of water is \(\mathrm{4.18 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}}\) and the calorimeter constant was \(\mathrm{12.0 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}}\). What is the specific heat of the Telfon, in units of \(\mathrm{\mathrm{J} / \mathrm{g}^{\circ} \mathrm{C}}\) ?

369173 A sample of oxygen gas expands its volume from \(\mathrm{3 \mathrm{~L}}\) to \(\mathrm{5 \mathrm{~L}}\) against a constant pressure of \(\mathrm{3 \mathrm{~atm}}\). If the work done during expansion is used to heat \(\mathrm{10 \mathrm{~mol}}\) of water initially present at \(\mathrm{290 \mathrm{~K}}\), its final temperature will be (specific heat capacity of water \({\rm{ = 4}}{\rm{.184}}{\mkern 1mu} {\rm{J}}{\mkern 1mu} {{\rm{K}}^{{\rm{ - 1}}}}{{\rm{g}}^{{\rm{ - 1}}}}{\rm{,1}}\;{\rm{L}}\;{\mkern 1mu} {\rm{atm = 101}}{\rm{.3}}{\mkern 1mu} {\rm{J}}\))

369174 The number of \(\mathrm{\mathrm{kJ}}\) of heat necessary to raise the temperature of \(\mathrm{60.0 \mathrm{~g}}\) of aluminium from \(\mathrm{35^{\circ} \mathrm{C}}\) to \(\mathrm{55^{\circ} \mathrm{C}}\), is, Molar heat capacity of \(\mathrm{\mathrm{Al}}\) is \(\mathrm{24 \mathrm{~J}}\) \(\mathrm{\mathrm{mol}^{-1} \mathrm{~K}^{-1}}\).

369175 0.06 mole of \(\mathrm{\mathrm{KNO}_{3}}\) solid is added to \(\mathrm{100 \mathrm{~cm}^{3}}\) of water at \(\mathrm{298 \mathrm{~K}}\). The enthalpy of \({\rm{KN}}{{\rm{O}}_{\rm{3}}}\left( {{\rm{aq}}} \right)\) solution is \(\mathrm{35.8 \mathrm{~kJ} \mathrm{~mol}^{-1}}\). After the solute is dissolved the temperature of the solutions will be

369176 Work done in the expansion of an ideal gas from \({\rm{4}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) to \({\rm{6}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) against a constant external pressure of \(\mathrm{2.5 \mathrm{~atm}}\) was used to heat up 1 mole of water at \(\mathrm{20^{\circ} \mathrm{C}}\). The final temperature of water will be (Take specific heat of water as\({\rm{4}}{\rm{.2J}}{{\rm{g}}^{{\rm{ - 1}}}}\;{{\rm{K}}^{{\rm{ - 1}}}}\))

369177 A block of Telfon plastic weighing \(\mathrm{16 \mathrm{~g}}\) was heated to \(\mathrm{90^{\circ} \mathrm{C}}\) and then put into a calorimeter containing \(\mathrm{50.0 \mathrm{~g}}\) of water at \(\mathrm{20^{\circ} \mathrm{C}}\). The system reached a temperature at \(\mathrm{30^{\circ} \mathrm{C}}\). The specific heat of water is \(\mathrm{4.18 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}}\) and the calorimeter constant was \(\mathrm{12.0 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}}\). What is the specific heat of the Telfon, in units of \(\mathrm{\mathrm{J} / \mathrm{g}^{\circ} \mathrm{C}}\) ?

369173 A sample of oxygen gas expands its volume from \(\mathrm{3 \mathrm{~L}}\) to \(\mathrm{5 \mathrm{~L}}\) against a constant pressure of \(\mathrm{3 \mathrm{~atm}}\). If the work done during expansion is used to heat \(\mathrm{10 \mathrm{~mol}}\) of water initially present at \(\mathrm{290 \mathrm{~K}}\), its final temperature will be (specific heat capacity of water \({\rm{ = 4}}{\rm{.184}}{\mkern 1mu} {\rm{J}}{\mkern 1mu} {{\rm{K}}^{{\rm{ - 1}}}}{{\rm{g}}^{{\rm{ - 1}}}}{\rm{,1}}\;{\rm{L}}\;{\mkern 1mu} {\rm{atm = 101}}{\rm{.3}}{\mkern 1mu} {\rm{J}}\))

369174 The number of \(\mathrm{\mathrm{kJ}}\) of heat necessary to raise the temperature of \(\mathrm{60.0 \mathrm{~g}}\) of aluminium from \(\mathrm{35^{\circ} \mathrm{C}}\) to \(\mathrm{55^{\circ} \mathrm{C}}\), is, Molar heat capacity of \(\mathrm{\mathrm{Al}}\) is \(\mathrm{24 \mathrm{~J}}\) \(\mathrm{\mathrm{mol}^{-1} \mathrm{~K}^{-1}}\).

369175 0.06 mole of \(\mathrm{\mathrm{KNO}_{3}}\) solid is added to \(\mathrm{100 \mathrm{~cm}^{3}}\) of water at \(\mathrm{298 \mathrm{~K}}\). The enthalpy of \({\rm{KN}}{{\rm{O}}_{\rm{3}}}\left( {{\rm{aq}}} \right)\) solution is \(\mathrm{35.8 \mathrm{~kJ} \mathrm{~mol}^{-1}}\). After the solute is dissolved the temperature of the solutions will be

369176 Work done in the expansion of an ideal gas from \({\rm{4}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) to \({\rm{6}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) against a constant external pressure of \(\mathrm{2.5 \mathrm{~atm}}\) was used to heat up 1 mole of water at \(\mathrm{20^{\circ} \mathrm{C}}\). The final temperature of water will be (Take specific heat of water as\({\rm{4}}{\rm{.2J}}{{\rm{g}}^{{\rm{ - 1}}}}\;{{\rm{K}}^{{\rm{ - 1}}}}\))

369177 A block of Telfon plastic weighing \(\mathrm{16 \mathrm{~g}}\) was heated to \(\mathrm{90^{\circ} \mathrm{C}}\) and then put into a calorimeter containing \(\mathrm{50.0 \mathrm{~g}}\) of water at \(\mathrm{20^{\circ} \mathrm{C}}\). The system reached a temperature at \(\mathrm{30^{\circ} \mathrm{C}}\). The specific heat of water is \(\mathrm{4.18 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}}\) and the calorimeter constant was \(\mathrm{12.0 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}}\). What is the specific heat of the Telfon, in units of \(\mathrm{\mathrm{J} / \mathrm{g}^{\circ} \mathrm{C}}\) ?

369173 A sample of oxygen gas expands its volume from \(\mathrm{3 \mathrm{~L}}\) to \(\mathrm{5 \mathrm{~L}}\) against a constant pressure of \(\mathrm{3 \mathrm{~atm}}\). If the work done during expansion is used to heat \(\mathrm{10 \mathrm{~mol}}\) of water initially present at \(\mathrm{290 \mathrm{~K}}\), its final temperature will be (specific heat capacity of water \({\rm{ = 4}}{\rm{.184}}{\mkern 1mu} {\rm{J}}{\mkern 1mu} {{\rm{K}}^{{\rm{ - 1}}}}{{\rm{g}}^{{\rm{ - 1}}}}{\rm{,1}}\;{\rm{L}}\;{\mkern 1mu} {\rm{atm = 101}}{\rm{.3}}{\mkern 1mu} {\rm{J}}\))

369174 The number of \(\mathrm{\mathrm{kJ}}\) of heat necessary to raise the temperature of \(\mathrm{60.0 \mathrm{~g}}\) of aluminium from \(\mathrm{35^{\circ} \mathrm{C}}\) to \(\mathrm{55^{\circ} \mathrm{C}}\), is, Molar heat capacity of \(\mathrm{\mathrm{Al}}\) is \(\mathrm{24 \mathrm{~J}}\) \(\mathrm{\mathrm{mol}^{-1} \mathrm{~K}^{-1}}\).

369175 0.06 mole of \(\mathrm{\mathrm{KNO}_{3}}\) solid is added to \(\mathrm{100 \mathrm{~cm}^{3}}\) of water at \(\mathrm{298 \mathrm{~K}}\). The enthalpy of \({\rm{KN}}{{\rm{O}}_{\rm{3}}}\left( {{\rm{aq}}} \right)\) solution is \(\mathrm{35.8 \mathrm{~kJ} \mathrm{~mol}^{-1}}\). After the solute is dissolved the temperature of the solutions will be

369176 Work done in the expansion of an ideal gas from \({\rm{4}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) to \({\rm{6}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) against a constant external pressure of \(\mathrm{2.5 \mathrm{~atm}}\) was used to heat up 1 mole of water at \(\mathrm{20^{\circ} \mathrm{C}}\). The final temperature of water will be (Take specific heat of water as\({\rm{4}}{\rm{.2J}}{{\rm{g}}^{{\rm{ - 1}}}}\;{{\rm{K}}^{{\rm{ - 1}}}}\))

369177 A block of Telfon plastic weighing \(\mathrm{16 \mathrm{~g}}\) was heated to \(\mathrm{90^{\circ} \mathrm{C}}\) and then put into a calorimeter containing \(\mathrm{50.0 \mathrm{~g}}\) of water at \(\mathrm{20^{\circ} \mathrm{C}}\). The system reached a temperature at \(\mathrm{30^{\circ} \mathrm{C}}\). The specific heat of water is \(\mathrm{4.18 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}}\) and the calorimeter constant was \(\mathrm{12.0 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}}\). What is the specific heat of the Telfon, in units of \(\mathrm{\mathrm{J} / \mathrm{g}^{\circ} \mathrm{C}}\) ?

369173 A sample of oxygen gas expands its volume from \(\mathrm{3 \mathrm{~L}}\) to \(\mathrm{5 \mathrm{~L}}\) against a constant pressure of \(\mathrm{3 \mathrm{~atm}}\). If the work done during expansion is used to heat \(\mathrm{10 \mathrm{~mol}}\) of water initially present at \(\mathrm{290 \mathrm{~K}}\), its final temperature will be (specific heat capacity of water \({\rm{ = 4}}{\rm{.184}}{\mkern 1mu} {\rm{J}}{\mkern 1mu} {{\rm{K}}^{{\rm{ - 1}}}}{{\rm{g}}^{{\rm{ - 1}}}}{\rm{,1}}\;{\rm{L}}\;{\mkern 1mu} {\rm{atm = 101}}{\rm{.3}}{\mkern 1mu} {\rm{J}}\))

369174 The number of \(\mathrm{\mathrm{kJ}}\) of heat necessary to raise the temperature of \(\mathrm{60.0 \mathrm{~g}}\) of aluminium from \(\mathrm{35^{\circ} \mathrm{C}}\) to \(\mathrm{55^{\circ} \mathrm{C}}\), is, Molar heat capacity of \(\mathrm{\mathrm{Al}}\) is \(\mathrm{24 \mathrm{~J}}\) \(\mathrm{\mathrm{mol}^{-1} \mathrm{~K}^{-1}}\).

369175 0.06 mole of \(\mathrm{\mathrm{KNO}_{3}}\) solid is added to \(\mathrm{100 \mathrm{~cm}^{3}}\) of water at \(\mathrm{298 \mathrm{~K}}\). The enthalpy of \({\rm{KN}}{{\rm{O}}_{\rm{3}}}\left( {{\rm{aq}}} \right)\) solution is \(\mathrm{35.8 \mathrm{~kJ} \mathrm{~mol}^{-1}}\). After the solute is dissolved the temperature of the solutions will be

369176 Work done in the expansion of an ideal gas from \({\rm{4}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) to \({\rm{6}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) against a constant external pressure of \(\mathrm{2.5 \mathrm{~atm}}\) was used to heat up 1 mole of water at \(\mathrm{20^{\circ} \mathrm{C}}\). The final temperature of water will be (Take specific heat of water as\({\rm{4}}{\rm{.2J}}{{\rm{g}}^{{\rm{ - 1}}}}\;{{\rm{K}}^{{\rm{ - 1}}}}\))

369177 A block of Telfon plastic weighing \(\mathrm{16 \mathrm{~g}}\) was heated to \(\mathrm{90^{\circ} \mathrm{C}}\) and then put into a calorimeter containing \(\mathrm{50.0 \mathrm{~g}}\) of water at \(\mathrm{20^{\circ} \mathrm{C}}\). The system reached a temperature at \(\mathrm{30^{\circ} \mathrm{C}}\). The specific heat of water is \(\mathrm{4.18 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}}\) and the calorimeter constant was \(\mathrm{12.0 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}}\). What is the specific heat of the Telfon, in units of \(\mathrm{\mathrm{J} / \mathrm{g}^{\circ} \mathrm{C}}\) ?