6.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 26. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass
carbon dioxide 20.31g
water 4.16 g
Use this information to find the molecular formula of X

C2H2

Explanation:

Mass of Carbon in CO2 grams gram

Mass of hydrogen in H2O grams gram

We will calculate the % of C and H in the sample  

% C %

% H %

Number of mole of C

Number of mole of H

Fractional share of  C

Fractional share of  H

Empirical Formula = CH

Empirical Mass

Molecular mass

Molecular Formula – CHn  

N

Molecular Formula = C2H2

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

c, liquids evaporate, creating a gas