The balanced chemical equation for combustion of `CH_4` is `CH_4(g) + 2O_2(g) -- CO_(2(g)) + 2H_2O (l) Calculate the amount of water formed by the combustion of 32g of `CH_4`?

Calculate the amount of water (g) produced by the combustion of 16 g of methane.

The balanced chemical equation of a reaction (at STP) is given below. 2H_(2((g))+O_(2(g))rarr2H_2O_((g)) : Calculate the mass of water formed as a result of the reaction (a).

The balanced chemical equation of a reaction (at STP) is given below. 2H_(2((g))+O_(2(g))rarr2H_2O_((g)) : Calculation the volume of oxygen required to combine completely with 224L of the hydrogen at STP.

1.5 g of H_2 react with 14.5 g of O_2 to form water Calculate the amount of water that is formed in the reaction.

3 g of H_2 is mixed with 29 g of O_2 to yield water. Calculate the maximum amount of water that can be formed.

Justify the following reaction is redox reaction 4NH_3(g) + 5O_2 (g) to 4NO (g) + 6H_2O (g)

Calculate the amount of CO_2 produced when 2 moles of carbon are burned in l6 g of O_2

Calculate the standard enthalpy change for the reaction CH_4(g) +2O_2(g) rarr CO_2(g)+2H_2O(l) Given that the standard enthalpies of formation of CH_4(g),CO_2(g), and H_2O(l) are -74.8 kJ mol^-1, -393.5 kJ mol^-1 and -285.8 kJ mol^-1 respectively.

Calculate the molecular mass of the following: H_2O , CO_2 , CH_4