Laws Of Chemical Combinations

Step 1: Understanding the statement. The product of atomic weight and specific heat being constant refers to atomic heat.
Step 2: Identifying the law. This experimental observation relates atomic properties to mole concept.
Step 3: Conclusion. This relation is associated with Avogadro’s law.

Step 1: Mass loss on ignition. Mass of water lost = 1.520 - 0.995 = 0.525 g
Step 2: Oxygen-hydrogen ratio. Equivalent weight of metal is calculated using oxygen combination.
Step 3: Final calculation. Using stoichiometric relation, equivalent weight comes out to be 9.

Step 1: CO and CO are formed by the same elements (C and O).
Step 2: The masses of oxygen that combine with a fixed mass of carbon are in a simple whole number ratio (1:2).

For H₂CO₃: C:H:O = 12:2:48 = 6:1:24

Step 1: Convert mass ratio to mole ratio: C: (6)/(12)=0.5, H: (1)/(1)=1, O: (24)/(16)=1.5 Step 2: Simplify: 0.5:1:1.5 = 1:2:3 Step 3: Empirical formula: CH₂O₃ Step 4: This corresponds to carbonic acid: HO-(C=O)-OH