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1.2.1 Molar Mass - Emilie (Example (C = 1(12.01) = 12.01 (O = 2(16.00) =…
1.2.1 Molar Mass - Emilie
Example
Carbon Dioxide (CO2)
C = 1(12.01) = 12.01
O = 2(16.00) = 32.00
CO2 = (32.00 + 12.01) = 44.01 g/mol
I can statements
https://docs.google.com/document/d/1H_tiUSO6AQScejS2BOE6sSV_yxVLSnX-cwF4J3T3k1E/edit
Example
Aluminium nitrate (Al(NO3)3)
Al = 1(26.98) = 26.98
N = 3(14.01) = 42.03
O = 6(16.00) = 96.00
(Al(NO3)3) = (26.98 + 42.03 + 96.00) = 165.01 g/mol
Significant Figures
The term Significant Figures refers to the number of important digits in the coefficient of an expression in scientific notation.
Rule #2
Any zeros between two significant figures are important
Example: 406, four and six are significant, hence 0 is too
Rule #3
A final zero or trailing zeros in the decimal portion ONLY are significant.
Example: 0.00500 -> the last two zeros are significant, the first three zeros are not significant
Rule #1
Non-zero digits are always important
Example: 26.98 has four significant figures ; 7.34 has three significant figures
Adding and subtracting sig figs
Step #1
Count the number of significant figures in the decimal portion of each number in the problem. (The digits to the left of the decimal place are not used to determine the number of decimal places in the final answer.)
Step #2
Add or subtract in the normal fashion.
Step #3
Round the answer to the LEAST number of places in the decimal portion of any number in the problem.
WARNING: These rules are different for multiplying and dividing
Calculating Molar Mass