On what law is stoichiometry based, and how do the calculations support this law?
See this old answer and links.
In practice, you are not even going to get that. Losses invariably occur on handling. And note that this is an experimental result, that is rationalized by our particle view of chemical reactivity. We don't have to rely on calculations; we do have to rely on experiment.
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Stoichiometry is based on the law of conservation of mass. The calculations involve balancing chemical equations and using mole ratios to determine the quantitative relationship between reactants and products in a chemical reaction, ensuring that mass is conserved. The mole ratios derived from balanced equations are crucial for converting between reactants and products in stoichiometric calculations.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- How many millimeters of .230 M Na2S are needed to react with 30.00 mL of .513 M AgNO3, according to the following balanced equation? Na2S (aq) + 2AgNO3 (aq) ---> 2NaNO3 (aq) + Ag2S (s)
- A dirty and impure sample that weighs 43.4 g contains a certain percentage of magnesium nitride. Magnesium nitride reacts with water.The sample is exposed to an excess of water to give 32.9 g Mg(OH)2. What percentage of Mg3N2is in the original sample?
- Why are mole ratios central to solving stoichiometry problems?
- How many grams of metal oxide could be produced from 7.461 g of magnesium?
- One liter of sulfur vapor, S8(g) , at 600 ˚ C and 1.00 atm is burned in excess pure O2 to give SO2, measured at the same temperature and pressure. What mass of SO2 gas is obtained?

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