survey of chemistry laboratory i chem 1151l empirical formula of zinc chloride
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SURVEY OF CHEMISTRY LABORATORY I CHEM 1151L EMPIRICAL FORMULA OF ZINC CHLORIDE. CAUTION!!!. BE SURE TO WEAR SAFETY GLASSES AT ALL TIMES IN THE LABORATORY NO EXCEPTIONS TO THIS RULE!. EMPIRICAL FORMULA OF ZINC CHLORIDE. Students will determine - PowerPoint PPT PresentationTRANSCRIPT
SURVEY OF CHEMISTRY LABORATORY I
CHEM 1151L
EMPIRICAL FORMULA OF ZINC CHLORIDE
CAUTION!!!CAUTION!!!BE SURE TO WEAR SAFETY GLASSES AT
ALLTIMES IN THE LABORATORY
NO EXCEPTIONS TO THIS RULE!
Students will determine
- the empirical formula of zinc chloride by
a process known as synthesis
- the empirical formula from their data
- the empirical formula from the class average
It is best to perform several experiments and obtain average values for the result
EMPIRICAL FORMULA OF ZINC CHLORIDE
- The lowest whole number ratio of atoms present in a compound
- the lowest whole number ratio of moles of atoms in a compound
For example
- The molecular formula of glucose is C6H12O6
- The empirical formula is CH2O
EMPIRICAL FORMULA
Can be determined by the following methods
Analysis
- A compound is broken down into its element
- The mount of each element present is accurately determined
Synthesis
- Prepared from accurately measured amounts of each of its
elements
EMPIRICAL FORMULA
- Determine the mass of each element found in the formula
(may be grams or percentage composition by mass)
- Convert each mass to moles using the atomic masses of the appropriate elements
- Divide each mole amount by the smallest number of moles
- Round each mole ratio to the nearest integer
- Write the whole numbers as subscripts in the formula
EMPIRICAL FORMULA
EMPIRICAL FORMULA
mol231.6g/mol12.01
g74.83 mol97.24
g/mol1.01
g25.17
000.1mol 6.231
mol 6.231 007.4
mol 6.231
mol 24.97
Assume 100.0 g sample
% of each element equals grams
C H
1.000 ≈ 1 4.007 ≈ 4
Empirical Formula: CH4
Determine the empirical formula of a compound whose composition is determined to be 74.83% carbon and 25.17% hydrogen
ZINC METAL
- Mass about 1 gram of zinc metal
- Record this mass
EVAPORATING DISH
- Mass a clean, dry evaporating dish
- Record this mass
HYCHLORIC ACID
- Use the automatic dispensing bottle
- Dispense 10 mL of 12 M hydrochloric acid (HCl) directly
into the evaporating dish
HYCHLORIC ACID + ZINC METAL
- Carefully add the zinc to the dish containing the HCl
- Must be done in the hood
- Allow all of the zinc to dissolve
EVAPORATE LIQUID
- Gently warm solution on a hotplate
- Must be done in the hood
- Avoid spattering
- A white powdery substance (zinc chloride) will form
COOL AND MASS PRODUCT
- Avoid melting of zinc chloride
- Take the dish off the hotplate when content is dried enough
- Allow the dish to cool
COOL AND MASS PRODUCT
- Mass the dish and the zinc chloride
- Record the mass
CALCULATIONS
- Complete your calculations on the data sheet
- Report the percent by mass of each element to the instructor before leaving the lab
- The class average is needed to complete the lab report