Units Of Measurement Flashcards

0
Q

International system of units (SI)

A

Meters, kilos, degrees Celsius

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1
Q

American units

A

Feet, pounds, degrees Fahrenheit

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2
Q

1 m =

A

100 cm = 10^3 mm = 10^6 μm

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3
Q

1 g =

A

10^3 mg = 10^6 μg

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4
Q

1 m^3 =

A

1000 L

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5
Q

A waste water effluent of 1000 L/hr contains 6 μg/L. What is the mass in g of mercury discharged per day?

A

(6 μg/L) x (1 mg/1000 μg) x (1g/1000mg) = 6x10^-6 g/L

(6x10^-6 g/L) x (1000 L /hr) x (24 hr/ day) = 0.144 g/day

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6
Q

1 mg/L =

A

1 ppm

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7
Q

1 μg/L =

A

1 ppb

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8
Q

Concentration units for gases

A

1) volumetric terms (ppmv)
2) percent by volume (%)
3) mass per unit volume (mg/m^3, μg/m^3)

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9
Q

Conversion for gases between ppmv & percent by volume (%)

A

1 ppmv= 10^-4 %

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10
Q

Express 0.8 ppmv as percent by volume (%)

A

1 ppmv/ 10^-4 = 0.8 ppmv/ X,

X= 0.8 x 10^-4 %

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11
Q

Converting btw ppmv & mg/m^3 for gases

A

Mg/m^3 = ((mol weight x ppmv)/ 22.414) x (273.15/actual temp) x (actual pressure/1 ATM)

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12
Q

Standard temperature and pressure (STP):

A

0 degrees Celsius & 1atm

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13
Q

Convert the concentration of ozone (O3) at 0.08 ppmv to mg/m^3, at 25C, 1atm, mol weight of O3 = 48 g/mol

A

Mg/m^3= ((48 x 0.08)/22.414) x (273.15/273.15 +25) x (1atm/1atm)

=0.157 mg/m^3

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14
Q

The Idea Gas Law: PV = nRT

A
P: pressure (ATM)
V: volume (L)
n: mass (mol)
R: ideal gas constant (0.082056 L x ATM x K^-1 x mol^-1)
T: temperature (K)
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15
Q

1 mol of an ideal gas occupies what volume?

A

22.414 L

16
Q

Calculate the mass (g) of SO2 within a volume of 2m^2 at 20C & 1.2 ATM

  • mol weight of SO2: 64g/mol
  • temp: 20C + 273 = 293K
  • volume: 2m^3 = 2000L
A

n= PV/RT, (1.2 ATM x 2000L)/ (0.08205 LxatmxK^-1xmol^-1x 293K)
n= 99.83 moles
99.83 mol x ((16x2)+32)g/mol = 6389g