An alkene upon combustion produces `CO_(2)(g)"and"H_(2)O(g).` In this combustion process if there is no volume change, then, the no. of C atoms per molecule of alkene will be:

A gaseous alkane on complete combustion gives CO_(2) and H_(2)O . If the ratio of moles O_(2) needed for combustion and moles of CO_(2) formed is 5:3 find out the formula of alkane.

The combustion of benzene (l) gives CO_(2)(g) and H_(2)O(l) . Given that heat of combustion of benzene at constant volume is –3263.9 kJ mol^(–1) at 25^(@)C , heat of combustion (in kJ mol^(–1) ) of benzene at constant pressure will be (R = 8.314 JK–1 mol–1)

4.4 gms of a hydrocarbon on complete combustion produced 13.2 gms of CO_(2) and 7.2 gms of H_(2)O . How many moles of oxygen is consumed per mole of hydrocarbon in the combustion?

The heat of combustion of H_(2)(g) at constant pressure and 300k is -280kJ mol^(-1) . What will be the heat of combustion at constant volume and at 300K ?

The combustion of benzene(/) gives CO_2(g) and H_2O(l) Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol^(-1) at 25^@C , heat of combustion (in kJ mol^(-1) ) of benzene at constant pressure will be (R = 8.314 JK^(-1) 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) .

1.5 g of ethane (C_(2)H_(6)) on complete combustion gave 4.4 g of CO_(2) and 2.7 g of H_(2)O . Show that the results are in accordance to the law of conservation of mass.

6g of a hydrocarbon on combustion in excess of oxygen produces 17.6g of CO_(2) and 10.8g of H_(2)O . The data illustrates the law of :

A sample of gaseous hydrocarbon occupying 1.12 "litre" at NTP , when completely burnt in air produced 2.2 g CO_(2) and 1.8 g H_(2)O . Calculate the weight of hydrocarbon taken and the volume of O_(2) at NTP required for its combustion.

The combustion reaction occuring in an automobile is 2C_(8)H_(18)+25O_(2)(g) to16CO_(2)(g)+18H_(2)O(g) This reaction is accompanied with signs of change in enthalpy, entropy and gibbs free energy