Ethane burns in oxygen to form `CO_2` and `H_2O` according to the equation :
`2C_2H_6 + 7O_2 rarr 4CO_2 + 6H_2O`
If 1250 cc of oxygen is burnt with 300 cc of ethane. Calculate :
the volume of unused `O_2`.

Balance the equations : C_2H_4 + O_2 to CO_2 + H_2O

1500 cm^(3) of oxygen was burnt with 300 cm^(3) of ethane (C_(2)H_(6)) . calculate the volume of unused oxygen.

Balance the equations : C_2H_4+O_2 to CO_2 + H_2O

Given 2 C _(2) H _(6) + 7 O _(2) to 4 CO _(2) + 6 H _(2)O 200 cc of O _(2) was burnt with 400 cc of ethane, Calculate the volume of CO _(2) formed and unused O _(2).

Ethane burns in oxygen by the following equation: 2C_(2)H_(6)+7O_(2) rarr 4CO_(2) + 6H_(2)O 2.5L of ethane are burnt in excess of oxygen at 27^(@)C and 1 atm pressure. Calculate how many litres of CO_(2) are formed. at 50^(@)C and 1.5 atm?

Ethane burns in oxygen by the following equation: 2C_(2)H_(6)+7O_(2) rarr 4CO_(2) + 6H_(2)O 2.5L of ethane are burnt in excess of oxygen at 27^(@)C and 1 atm pressure. Calculate how many litres of CO_(2) are formed. at 27^(@)C and 1.0 atm?

H_(2)S burns in O_(2) to form

Butane (C_(4)H_(10)) gas burns in oxygen to give carbon dioxide and water according to the reaction. 2C_(4)H_(10) (g) + 13O_(2)(g) rarr 8 CO_(2)(g) + 10H_(2)O(l) When 5.0 L of butane ware burnt in excess of oxygen at 67^(@)C and 2 bar pressure, calculate the dioxide evolved.

Isobutane (C_(4)H_(10)) undergoes combustion in oxygen according to the following reaction: 2C_(4)H_(10)(g)+13O_(2)(g) rarr 8CO_(2)(g)+10H_(2)O(e) When 10.00 L of isobutane is burnt at 27^(@)C and 1 bar pressure, calculate the volume of CO_(2) produced at 120^(@)C and 4.0 bar pressure.

Complete and balance the chemical equation: "_____" + 5O_2 to 4CO_2 + 2H_2O + heat