How much oxygen is formed from 264 g of `CO_(2)` and 216 g of `H_(2)O` ?

Complete combustion of 1.18 g of organic compound gives 2.64 g of CO_(2) & 1.26 g " of " H_(2)O . Find emprical formula of compound ?

Complete combustion of 1.80g of an oxygen containing compound " (C_(x)H_(y)O_(z)) gave 2.64g of CO_(2) and 1.08g of H_(2)O .The percentage of oxygen in the organic compound is:

1.2 g of an organic compound containing C, H and oxygen on combustion gave 2.64 g CO_2 and 1.08 g H_2 O . The mass of oxygen in 1.2 g of the compound is

How much heat is evolved when 12 g of CO reacts with NO_(2) ? This reaction is 4CO(g)+2NO_(2)(g)to4CO_(2)(g)+N_(2)(g),Delta_(r)H^(0)=-1200kJ Write an application of Hess’s law. Does the following reaction represent a thermochemical equation? CH_(4)(g)+2O_(2)(g)toCO_(2)(g)+2H_(2)O(g)Delta,H^(0)=-900kJmol^(-1)

How many moles of methane are required to produce 22 g of CO_(2) (g) + after combustion :- CH_(4)(g) + 2O_(2)(g) + 2H_(2)O(g)

Hydrogen combines with oxygen with oxygen to form H_(2)O in which 16 g of oxygen combine with 2 g of hydrogen. Hydrogen also combines with carbon to form CH_(4) in which 2 g of hydrogen combine with 6 g of carbon. If carbon and oxygen combine togather then they will do show in the ratio of