chem lab process LOL (kill me pls)

stoichiometry example

(how many grams of N₂ are necessary to produce 7.5g of NH₃) N₂ + 3H₂ → 2NH₃

2NH₃ = 7.5g NH₃/14g + 3.03g = 0.441 mol

0.411 mol NH₃ × 1 mol N₂/2 mol NH₃ = 0.221 mol N₂

0221 mol * (2 × 14)g/1 mol = 0.618g of N₂

empirical formula steps

1. convert to mol

2. divide by smallest # of mol

3. round answer to nearest whole #

stoichiometry steps

1. convert to moles,

2. multiply # of moles in previous answer by mole of specified element over # of compound in given equation

3. take that answer and convert it to grams (make sure to multiply by how many are present in equation)

expected % mass loss steps

1. take the weight of initial compound (multiply by # of compound present)

2. take weight of mass loss (CO₂ and/or H₂O)

3. divide weight of mass loss by initial weight and multiply by 100

calculate % of mass of given element in compound steps

1. find mass of specified element(s)

2. divide that mass by the mass of the whole compound

3. multiply your answer by 100

standard deviation steps

1. take sum of all the long decimals squared

2. divide that by # of trials minus 1

3. square root the whole fraction

limiting reagent steps

1. convert given elements to mols

2. multiply the answers by # of reactant present over # of specified compound in equation

3. whichever is smaller is your answer

calculation of compound in initial mixture

1. find mass of specified compound within equation

2. find weight of “mass loss” (CO₂ or H₂O)

3. find mass loss with given weights (initial and weight after heating)

4. multiply the actual mass loss by the mass of specified compound over the weight of “mass loss”

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to find the remaining compound:

1. subtract initial mass by the mass of the previous answer (compound)