It comes to from the chemical reaction itself. Exothermic reaction release heat because the energy level of the products is lower than that of the reactants. Therefore, the net enthalpy change of the reaction is negative (-), meaning heat or light (or any other form of energy) is released into the environment. An example of an exothermic reaction is the combustion of fuel.
Answer:
X 154
Check solution in explanation
Explanation:
Average atomic mass = ( mass 1× abudance) + ( mass 2× abudance)+ ( mass 3× abudance) / 100
(149×13.8)+(152×44.9) +(154×41.3)/100
2056.2 + 6824.8 + 6360.2/100
=152.412
Answer:
most likely water
Explanation:
most likely it is water, however pressure plays a role, if you are at sea level the boiling point of water is 100°C but if you are on Mt. Everest it is 71°C, assuming she is slightly above sea level it is water.
We are given with the percentage composition of oxygen in an oxide from phosphorus and oxygen equal to 43.6 percent. that is the phosphorus is equal to 56.4 percent. we divide each with the molar mass and divide each with the smaller quantity. P then is equal to 1 and O is equal to 1.5. In this case, the empirical formula is P2O3.
Answer:
Nothing is happening.
Explanation:
As written, nothing is going on. H2+O2+H2O represents a mixture of H2, O2, and H2O. We aren't even given the states, so they may all be gases, liquids/solids, or dissolved gases in a liquid (water).
If we had H2+O2 → H2O, we could say that hydrogen and oxygen are combining to form H2O, water. We should note, however, that the chemical equation is not balanced. There are two oxygen atoms on the reactant side, but only one on the product side. A balanced equation would read:
2H2 + O2 → 2H2O
It would be nice to indicate the physical states, such as:
2H2(g) + O2(g) → 2H2O(l)
Two gases, oxygen and hydrogen, combine to form liquid water.
Also missing from this equation is the energy that may be consumed, or released in this reaction. It would be nice to know, for example, that this reaction releases a lot of energy. Otherwise, we might wind up in the local headlines.
