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agasfer [191]
3 years ago
11

A particulate matter sampler was operated for 24 hours at a flowrate of 1.4 m3 min-1. The starting weight of the filter paper be

fore sampling was 2.05 grams. At the end of the sampling period, the filter's weight was 3.84 grams, and the gain in weight was due completely to the particulate matter that had collected on the surface of the filter paper during air sampling. Determine the particulate matter concentration, in micrograms per cubic meter (expressed to one decimal place), for the given sampling time.
Chemistry
1 answer:
tekilochka [14]3 years ago
7 0

Answer:

887.89 μg/m³

Explanation:

Given:

Duration of mass flow = 24 hours = 24 × 60 = 1440 minutes

Flowrate = 1.4 m³/min

starting weight of the filter paper before sampling = 2.05 grams

Filter's weight = 3.84 grams

Now,

Mass of the particular matter collected

= Mass of filter after 24 hours - Initial weight of the filter

= 3.84 - 2.05

= 1.79

Now,

The total volume passing through filter = Flowerate × Time

= 1.4 × 1440

= 2016 m³

Particulate matter concentration = \frac{\textup{Mass of particulare matter collected}}{\textup{Volume of the sample}}

or

Particulate matter concentration = \frac{\textup{1.79}}{\textup{2016}}

or

Particulate matter concentration = 0.0008878 g/m³

also,

1 gram = 10⁶ micrograms

thus,

Particulate matter concentration = 0.0008878 × 10⁶ μg/m³

= 887.89 μg/m³

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GREYUIT [131]

Answer:

Al + MnO4- + 2H2O → Al(OH)4- + MnO2

Explanation:

First of all, we out down the skeleton equation;

Al + MnO4- → MnO2 + Al(OH)4-

Secondly, we write the oxidation and reduction equation in basic medium;

Oxidation half equation:Al + 4H2O + 4OH- → Al(OH)4- + 4H2O + 3e-

Reduction half equation:MnO4- + 4H2O + 3e- → MnO2 + 2H2O + 4OH-

Thirdly, we add the two half reactions together to obtain:

Al + MnO4- + 8H2O + 4OH- + 3e- → Al(OH)4- + MnO2 + 6H2O + 3e- + 4OH-

Lastly, cancel out species that occur on both sides of the reaction equation;

Al + MnO4- + 8H2O→ Al(OH)4- + MnO2 + 6H2O

The simplified equation now becomes;

Al + MnO4- + 2H2O → Al(OH)4- + MnO2

4 0
3 years ago
How does this graph illustrate Boyle’s law?
bazaltina [42]
Do you have a picture of the graph?
5 0
3 years ago
A 996.9 g sample of ethanol undergoes a temperature change of -70.98 °C while releasing 62.9
Volgvan

Answer:

c=3.71\ J/g^{\circ} C

Explanation:

Given that,

Mass of sample, m = 996.9 g

The change in temperature of the sample, \Delta T=-70.98^{\circ}C

Heat produced, Q = 62.9  calories = 263173.6 J

The heat released by a sample due to change in temperature is given by :

Q=mc\Delta T

Where

c is the specific heat capacity

So,

c=\dfrac{Q}{m\Delta T}\\\\c=\dfrac{263173.6}{996.9\times 70.98}\\\\c=3.71\ J/g^{\circ} C

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3 0
4 years ago
How many moles of oxygen are in 3.0 moles of C6H12O6?
Morgarella [4.7K]
1 mole C₆H₁₂O₆ ------------- 6 moles oxygen
3 moles C₆H₁₂O₆ ----------- X
X = (3×6)/1

X = 18 moles
5 0
3 years ago
Compounds A and B are colorless gases obtained by combining sulfur with oxygen. Compound A results from combining 6.00 g of sulf
sukhopar [10]

Answer:

1.5

Explanation:

Given that :

Compound A and B are formed from Sulfur + Oxygen.

Compound A :

6g sulfur + 5.99g Oxygen

Compound B:

8.6g sulfur + 12.88g oxygen

Comparing the ratios :

Compound A:

S : O = 6.00 : 5.99

S/0 = 6.0g S / 5.99g O

Compound B :

S : O = 8.60 : 12.88

S / O = 8.60g S / 12.88g O

Mass Ratio of A / mass Ratio of B

(6.0g S / 5.99g O) ÷ (8.60g S / 12.88g O)

(6.0 g S / 5.99g O) × (12.88g O / 8.60g S)

(6 × 12.88) / (5.99 × 8.60)

= 77.28 / 51.514

= 1.50017

= 1.5

4 0
4 years ago
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