When `12.0g` of carbon reacted with oxygen to form `CO` and `CO_(2)` at `25^(@)C` and constant pressure, `75.0kcal` of heat was liberated and no carbon remained . Calculate the mass of oxygen which reacted.
`(DeltaH_(f)^(@)(CO_(2))=-95kcal mol^(-1),DeltaH_(f)^(@)(CO)=-24kcal mol^(-1))`

When 12.0g of C reacted with oxygen to form CO and CO_(2) at 25^(@)C at constant pressure, 313.8 kJ of heat was released and no carbon remained. Calculate the mass of oxygen which reacted. Delta_(f)H^(Theta) (CO,g) =- 110.5 kJ mol^(-1) and Delta_(r)H^(Theta) (CO,g) =- 393.5 kJ mol^(-1)

When 12.0g of C reacted with oxygen to form CO and CO_(2) at 25^(@)C at constant pressure, 313.8 kJ of heat was released and no carbon remained. Calculate the mass of oxygen which reacted. Delta_(f)H^(Theta) (CO,g) =- 110.5 kJ mol^(-1) and Delta_(r)H^(Theta) (CO_(2),g) =- 393.5 kJ mol^(-1)

When 12.0g of carbon (graphite)reacted with oxygen to form CO and CO_(2) at 25^(@)C and constant pressure, 252 kJ of heat was released and no carbon remained. If Delta H_(f)^(0)(CO,g)= -110.5 kJ mol^(-1) and Delta H_(f)^(0)(CO_(2),g)= -393.5 kJ mol^(-1) ,calculate the mass of oxygen consumed.

When 12.0g of carbon (graphite)reacted with oxygen to form CO and CO_(2) at 25^(@)C and constant pressure, 252 kJ of heat was released and no carbon remained. If Delta H_(f)^(0)(CO,g)= -110.5 kJ mol^(-1) and Delta H_(f)^(0)(CO_(2),g)= -393.5 kJ mol^(-1) ,calculate the mass of oxygen consumed.

When 12.0 g of carbon reacted with limited quantity of oxygen, 57.5 kcal of heat was produced, calculate the number of moles of CO produced (Delta_(f)H(CO_(2))=-94.5 cal, Delta_(f)H(CO)= -21.41kcal.

Calculate the heat produced when 3.785 litre of actane (C_(8)H_(18)) reacts with oxygen to form CO & water vapour at 25^(@)C . The density of octane is 0.7025 gm/ml. enthalpy of combustion of C_(8)H_(18) is -1302.7 k Cal/mol. {:(DeltaH_(f)^(@) CO_(2)(g)=-94.05" k Cal mol"^(-1),,,DeltaH_(f)^(@) CO(g)=-26.41" k Cal mol"^(-1),),(DeltaH_(f)^(@) H_(2)O(l)=-68.32" k Cal mol"^(-1),,,DeltaH_(f)^(@) H_(2)O (g)=-57.79" k Cal mol"^(-1)):}

When 2.4g of carbon reacted with X g of oxygen to form CO and CO_2, 50.4 kJ of heat was released and no reactant is left over. Standard heats of formation of carbon monoxide and carbondioxide are -110.5 kJ mol^(-1) and -393.5 kJ mol^(-1) respectively. Calculate X.

The heat of formation of CO and CO_(2) are -26.4kCal and -94 kCal , respectively. Heat of combustion of carbon monoxide will be