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Chem Final Unit 1
This will list past important notes from this unit 1 chem work
Question | Answer | ||
---|---|---|---|
How do you calculate formula mass? What do they measure in? | add up atomic masses amu | ||
What are atomic masses equal to? | molar mass (g/mol) | ||
Find the formula mass of NH4NO3. | 80.05 amu | ||
Find the molar mass of NH4NO3. | 80.05 g/mol | ||
Convert 10g NH4NO3 to moles. | 0.1254 mol NH4NO3 | ||
What does molecular mass or molecular weight refer to? | formula mass of a molecular compound | ||
What is the formula for Mass Percent Composition? | divide the mass of element in 1 mole of the compound by the compound's molar mass and multiply the result by 100 | ||
What is the percent composition of CO2? | C = 27.29% O = 72.21% | ||
What is the formula mass of CHCl3? | 60.05 amu | ||
Percent composition of C5H12 | 83.22% C 16.78% H | ||
What is Avogardo's Number? | 1 mole = 6.02*10^23 | ||
What is Avogadro's Number associated with and what is it used for? | associated with a very small particle or atom or a formula unit represented with a compound used for a conversion problem | ||
Convert 5 mole CH4 to molecules. | 3.0*10^24 molecules | ||
Convert 3*10^24 atoms H to mol H. | 5 mol H | ||
Convert 12g He to atoms. | 1.8*10^24 atoms He | ||
What is the same as the number of products? | reactants reactants --> products | ||
Balance BaCl2 + NaOH --> Ba(OH2) + NaCl | BaCl2 + 2NaOH --> Ba(OH)2 + 2NaCl | ||
What is important to know about polyatomic atoms? | If polyatomic atoms are the same on both sides DO NOT separate them | ||
Balance C2H4 + O2 --> CO2 + H2O | C2H4 + 3O2 --> 2CO2 + 2H2O | ||
What are the equations for stoichiometry? | Mol A --> Mol B (mole to mole) Mol A/B --> gB; gA --> mol B (mole ratio) gA --> gB (grams to grams) | ||
Sulfur Dioxide reacts with oxygen gas to form sulfur trioxide. a. If 3.4 moles of sulfur dioxide reacts with excess oxygen gas, how many moles of sulfur trioxide will form? b. How many moles of oxygen gas will react completely with 4.7 moles of sulfure | a. 3.4 mol SO3 b. 2.34 mol O2 | ||
Propane (C3H8) reacts with oxygen gas to form CO2 and H2O. If 38g of water are produced in the reaction, how many moles of CO2 were produced? | 1.58 mol CO2 | ||
What is a synthesis reaction? | A compound is made from simpler materials | A + B --> AB C(s) + O2(g) --> CO2(g) | not always balanced equations |
What is a decomposition reaction? | A compound is broken down into simpler compounds, or all the way down to the elements that made it up. | H2O(l) --> H2(g) + O2(g) | don't have to break things down all the way down into their basic element |
What is a combustion reaction? | A compound containing carbon and hydrogen (and sometimes oxygen) combines with oxygen gas to produce carbon dioxide and water. | CH4(g) + O2(g) --> CO2(g) + H2O(g) | CxHy(O2) + O2 --> CO2 + H2O |
What is a single replacement reaction? | One element that starts out by itself, replaces another element in a compound, kicking it out. | Fe(s) + CuCl2(aq) --> Cu(s) + FeCl2(aq) | A + BC --> B + AC |
What is a double replacement reaction? | The positive and negative ions in 2 compounds switch places. | BaCl2(aq) + NaSo4(aq) --> BaSO4(s) + NaCl(aq) | AB + CD --> AD + BC |
What is the % composition by mass of water in calcium sulfate dihydrate, CaSO4 * 2H2O(s)? | 20.93 H2O | ||
A hydrated salt of calcium chloride was found to have a mass of 5.4668g. After heating the substance for a long time, the mass of the anhydrous salt was measured to be 2.7745g. What was the empirical formula of the hydrated calcium chloride compound? | CaCl2*6H2O | ||
What is there no equal measure of? | reactants | limiting reagent and excess reagent | |
2NH3 + CO2 --> CH4N2O + H2O | excess = NH3 -- 0.294 mol CH4N2O limiting = CO2 -- 0.227 mol CH4N2O | ||
What is the equation for percent yeild? | (actual yield/theoretical yield)*100 | ||
If 15.0g of CH3OH reacts with 10.0g CO, which is the limiting reagent and what is the theoretical yield of CH3COOH? The actual yield is 19.1g. | LR = CO -- 0.357mol CH3COOH Theoretical yield = 21.4 CH3OOH | ||