1.Is molar mass always done for one mol of substance?
Let me make up an example:
2H2(g)+O2(g)--> 2H2O When finding molar mas of water would it be 2(2(1.01)+2(16)) or just 2(1.01)+16?
2. I'm not really sure about endergonic exergonic reaction because my teacher is teaching some grade 12 stuff to us. So is this correct decomposition reactions are endergonic so their reverse reaction which is synthesis would be exergonic and dissolving which is a phase change is endergonic?
THE molar mass is the mass of one mole so the molar mass of water is about 18 (16+2).
The mass of TWO moles of water is about 36; that is, 2 x mass of 1 mole or 2 x 18 = 36
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Exergonic reactions are spontaneous. Endergonic reactions are non-spontaneous. If a reaction is exergonic its reverse reaction is endogonic.
1. Molar mass is a term used to describe the mass of one mole of a substance. It represents the mass of a substance in grams when you have one mole of that substance. So, when calculating the molar mass of a compound like water (H2O), you would add up the masses of each individual atom in one molecule of water. In this case, it would be 2(2(1.01) + 16), where 2 represents the coefficient in front of H2O indicating that there are two water molecules.
2. Endergonic and exergonic reactions are terms used to describe whether a reaction absorbs or releases energy, respectively. In a decomposition reaction, bigger molecules are broken down into smaller molecules or atoms, and this process typically requires energy input. So, decomposition reactions are considered endergonic because they absorb energy. On the other hand, the reverse reaction, which is synthesis, involves combining smaller molecules or atoms to form bigger molecules and usually releases energy. Therefore, synthesis reactions are considered exergonic.
Regarding dissolving, it is a physical process that involves the interaction between a solute and a solvent. The dissolution of many substances is typically exergonic, as energy is often released when the solute particles interact with the solvent particles. However, it is important to note that the energetics of dissolving can vary depending on the specific solute and solvent involved, as some dissolutions can be endergonic.
Remember, it's always a good idea to consult your textbook or ask your teacher for clarification on specific concepts to ensure accurate understanding.