If Cobalt(II)Sulfate is heated too strongly, the following reaction will occur CoSO4 produces CoO(s)+ SO3(g)
If you are heating a sample of CoSO4.6H20 and this reaction occurs along with dehydration, what will happen to the experimental percent water? Explain your answer.
wouldn't some of the water react with Cobalt oxide to form cobalt hydroxide?
To determine what will happen to the experimental percent water, we need to understand the concept of percent composition and how it relates to the reaction. The percent composition of a compound can be calculated by dividing the mass of the element in the compound by the total mass of the compound, and then multiplying by 100. In this case, we are interested in the percent water in the compound CoSO4.6H2O.
The chemical formula "CoSO4 ⋅ 6H2O" indicates that there are six water molecules bonded to each molecule of CoSO4. When we heat this compound, a reaction called dehydration occurs, where water molecules are removed. The reaction produces CoO(s) and SO3(g).
Since the water molecules are removed during the reaction, the total mass of the compound will decrease. However, the mass of the water component specifically will decrease while the mass of the other components stays constant. Therefore, the experimental percent water will decrease.
To determine the exact change in the experimental percent water, we would need to measure the mass of the water component before and after the reaction. By comparing the initial and final values and calculating the percent composition using the new mass, we can determine the change in the experimental percent water.