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27 Cards in this Set
- Front
- Back
Addition of HNO3 to Copper |
Causes copper metal to slowly dissolve and produce a brown gas. |
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Cu(NO3)2 + NaOH |
Metathesis Reaction, solution turns bright blue. Products are Cu(OH)s + 2NaNO3 (aq) |
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Washing and Decanting CuO and water |
Removes excess NaNO3 and impurities |
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When you add H2SO4, what copper compound is now present? |
Copper (II) sulfate |
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CuSO4 (aq) + Zn (s) |
Produces hydrogen gas, Zn2+ ions and SO4 2- ions are present in the solution. *When acid is added to a metal, hydrogen gas is produced |
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Possible Sources of Error in Copper Experiment |
1. Not drying sample completely, so SO4 is still present 2. Other elements are mixed in with copper |
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Percent Yield Formula |
(Actual Yield / Theoretical Yield) * 100% |
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Relationship between pressure and volume of a gas at constant temperature |
As volume decreases, pressure increases |
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Relationship between temperature and pressure of a gas at a constant volume |
As temperature increases, pressure increases |
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Ideal Gas Law |
PV = nRT |
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Accepted Value of R |
0.0821 |
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Number of Moles of a Substance |
Equals the mass of the substance in grams, m, divided by the molar mass, M |
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Molar Mass Related to Ideal Gas Law |
PV = (m/M)RT M = (mRT)/PV |
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Van der Waals Equation |
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(N^2a)/v^2 |
Correction to pressure, takes into account intermolecular attractions |
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Nb |
Correction for the finite volume of the molecules |
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Atmospheric Pressure |
Pressure of O2 + Pressure H2O vapor |
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Purpose of Equalizing Clamp |
To produce atmospheric pressure inside the bottle and test tube |
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Opening pinch clamp |
Water flows into beaker. If the system remains airtight and has no leaks, tube A will remain filled with water |
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Volume of water displaced |
Equal to volume of oxygen produced |
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Difference in mass between the tube plus the contents and the original mass of the tube plus MnO2 and KClO3 |
Mass of oxygen produced |
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a for O2 |
1.360 |
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a for O2 |
1.360 |
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b for O2 |
31.83 |
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Cause for derivation from ideal gas behavior |
Attractive forces between molecules |
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If an insufficient amount of liquid unknown had been used, how would the value of the experimental molar mass been affected? |
The liquid wouldn't occupy the whole container and the volume in the formula would be greater than it actually is and there would be a smaller molar mass |
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Major sources of error in determining molar mass |
Too big hole in aluminum, inaccurate temp reading, inaccurate volume measured, inaccurate weight measured |