Answer:
C. Natural abundance
Explanation:
The percentage of natural occurrence of an isotope of an element on the planet is the natural abundance or the geonormal abundance.
- Proportions of each isotope of an element that occurs naturally is the natural abundance.
- It is represented as a percentage value.
- From the natural abundance, we can determine the relative atomic mass.
- If we know the atomic mass of each of the isotope and their abundances, it is easy to determine their relative atomic masses.
At STP, 1 mol of gas occupies 22.4 L of space.
mol CO2 = 5.0 L * 1 mol/22.4 L = 0.2232 mol
Using the balanced equation, we use stoichiometry to convert our quantities. There are 2 CO2 moles for every mole of O2.
mol O2 = 0.2232 mol CO2 * 1 mol O2 / 2 mol CO2
= 0.1116 mol
Converting back to volume
volume O2 = 0.1116 mol * 22.4 L/1 mol
= 2.5 L
The answer to the question is 2.5 L of oxygen gas.
Answer:
b. endothermic decomposition
Explanation:
Decomposition reaction:
It is the reaction in which one reactant is break down into two or more product.
AB → A + B
Synthesis reaction:
It is the reaction in which two or more simple substance react to give one or more complex product.
A + B → AB
Endothermic reactions:
The type of reactions in which energy is absorbed are called endothermic reactions.
In this type of reaction energy needed to break the bond are higher than the energy released during bond formation.
For example:
C + H₂O + 131 kj/mol → CO + H₂
Thus, in given reaction energy is added and AB compound is decomposed to give A and B so this reaction is endothermic decomposition.
