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.`

When 12.0g of C reacted with a limited quantity of oxygen, 57.5 kcal of heat was produced. Calculate the number of CO and number of moles of CO_(2) produced. Given C +O_(2) rarr CO_(2), Delta_(f)H = - 94.05 kcal C +1//2O_(2) rarr CO, Delta_(f)H =- 21.41 kcal

When 12.0g of C reacted with a limited quantity of oxygen, 57.5 kcal of heat was produced. Calculate the number of CO and number of moles of CO_(2) produced. Given C +O_(2) rarr CO_(2), Delta_(f)H = - 94.05 kcal C +1//2O_(2) rarr CO, Delta_(f)H =- 26.41 kcal

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))

The combustion of 1 mol of benzene takes place at 298 K and 1 atm . After combustion, CO_(2)(g) and H_(2)O(l) are produced and 3267.0 kJ of heat is librated. Calculate the standard entalpy of formation, Delta_(f)H^(Θ) of benzene Given: Delta_(f)H^(Θ)CO_(2)(g) = -393.5 kJ mol^(-1) Delta_(f)H^(Θ)H_(2)O(l) = -285.83 kJ mol^(-1) .

The combustion of 1 mol of benzene takes place at 298 K and 1 atm . After combustion, CO_(2)(g) and H_(2)O(l) are produced and 3267.0 kJ of heat is librated. Calculate the standard entalpy of formation, Delta_(f)H^(Θ) of benzene Given: Delta_(f)H^(Θ)CO_(2)(g) = -393.5 kJ mol^(-1) Delta_(f)H^(Θ)H_(2)O(l) = -285.83 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 12.0g 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 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)

Calculate the heat produced when 3.785 L of octabe reacts with oxygeb to form carbon mono oxide and water vapour at 25^(@)C . (Density of octane is 0.75025 g mL^(-1)). Delta_(comb)H^(Theta)(C_(8)H_(18)) =- 1302.7 kcal, Delta_(f)H^(Theta) (CO_(2)) =- 94.05 kcal, Delta_(f)H^(Theta) (H_(2)O) =- 64.32 kcal, Delta_(f)H^(Theta) (CO) =- 26.41 kcal mo^(-1)