A student claims that the reaction of hydrogen and oxygen to form
water is evidence supporting the claim that mass is conserved in a
chemical reaction. The chemical equation the student uses for the reaction is H2 + O2 --> H2O. Does this evidence support the claim? Why or why not? *
Yes, it supports the claim because all the elements in the reactants appear in the product
No, it does not support the claim because it is not a closed system.
Yes, it supports the claim because the reaction equation is balanced.
No, it does not support the claim because the reaction equation is not balanced.
Yes, it supports the claim because the reaction equation is balanced.
To determine whether the evidence supports the claim that mass is conserved in a chemical reaction, we need to consider the conservation of atoms in the reaction. The reaction equation provided, H2 + O2 -> H2O, is balanced because the same number of atoms of each element are present on both sides of the equation.
In the reactants, we have 2 hydrogen atoms and 2 oxygen atoms. In the product, we have 2 hydrogen atoms and 1 oxygen atom. This means that all the elements (hydrogen and oxygen) present in the reactants are also present in the product. Therefore, the reaction demonstrates the conservation of mass because none of the atoms are created or destroyed during the reaction.
Therefore, the evidence of the reaction between hydrogen and oxygen to form water supports the claim that mass is conserved in a chemical reaction.