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Conversion Problems

Conversion Problems. SI Units (System Internationale`): Mass = kilograms = kg Length = meters = m. Volume = dm 3 = 1 L Time = seconds = s. Conversion Problems. SI Units (System Internationale`): Mole - amount of substance (mol). Candele - intensity of light (cd)

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Conversion Problems

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  1. Conversion Problems • SI Units (System Internationale`): • Mass = kilograms = kg • Length = meters = m. • Volume = dm3 = 1 L • Time = seconds = s.

  2. Conversion Problems • SI Units (System Internationale`): • Mole - amount of substance (mol). • Candele - intensity of light (cd) • Ampere - electric current (A) • Temperature - kelvin (K)

  3. Conversion Problems • SI Units (System Internationale`): • Base units vs Derived Units • Derived units involve the mathematical manipulation of base units.

  4. Conversion Problems • Metric prefixes vs. base units: • Know: Giga(G), Mega(M), kilo(k), deci(d), centi(c), milli(m), micro(m), nano(n).

  5. Conversion Problems • Percent Error: • Percent Error = • [|lab value - accepted value| / accepted value ]* 100%

  6. Conversion Problems • Factor Analysis: • No Choice: conversion problems MUST be done using this method. Please always show your work.

  7. Conversion Problems • Process: • Start with what they give you. • Multiply by a fraction.

  8. Conversion Problems • Process: • The starting unit goes in the opposite part of the next fraction(ex. top to bottom). • The new unit goes in the remaining part of the fraction.

  9. Conversion Problems • Process: • Always convert back to the base unit. • Use a conversion factor. • Cancel out the starting unit.

  10. Conversion Problems • Process: • Multiply. Divide (do the math)

  11. Conversion Problems • Convert: • Prefix to base unit • Base unit to prefix • Prefix to prefix.

  12. Scientific Notation • Short hand notation: • Coefficient • Exponent • ex.3.2E7

  13. Scientific Notation • Legal coefficients: • Must be a digit between 1-9 in the one’s column followed by the decimal. • Exponents can be positive or negative (whole numbers).

  14. Scientific Notation • Converting from scientific notation to the number. • Converting from the number to scientific notation. • Calculations involving scientific notation and units.

  15. Scientific Notation • Using your calculator: • Do not use the 10 to the x function! You will become a victim of the algebraic order of operations. (Use E/EXP)

  16. Significant Figures • Accuracy vs Precision • Accuracy refers to the correctness of the measurement. • Precision refers to reproducibility.

  17. Significant Figures • How should data be reported? • 1.) Must reflect the level of accuracy or sophistication of the measuring device. (estimate the next digit)

  18. Significant Figures • Applying Sig Figs • 2.) Applies only to measured quantities. • 3.) Counting numbers have an infinite amount of sig figs.

  19. Significant Figures • Rules: • 1.) All non zero numbers are significant

  20. Significant Figures • Rules: • 2.) Trailing zeros to the left of the decimal are not significant. • 3.) Trailing zeros to the right of the decimal are significant.

  21. Significant Figures • Rules: • 4.) Leading zeros to the right of the decimal are NOT significant.

  22. Significant Figures • Rules: • 5.) Zeros between significant digits are significant. • 6.) Calculations should be expressed based on the least sophisticated measurement.

  23. Significant Figures • Rules: • 7.) Exact numbers are infinitely significant. • 8.) Addition and subtraction is handled differently than multiplication and division.

  24. Significant Figures • Note: • To round, always consider the next digit. • Sometimes Sig. Figs. are best expressed in scientific notation.

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