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aliina [53]
3 years ago
10

Compare (a) the number of drops and (b) the length of time, in minutes, required to deliver 50 mL of intravenous solutions when

using a microdrip set, at 60 drops/mL, and a standard administration set, at 15 drops/mL, if in each case one drop is to be administered per second.
Chemistry
1 answer:
Marina CMI [18]3 years ago
7 0

Explanation:

Volume of intravenous solution to be delivered = 50 mL

1) Rate of drops per milliliter of the solution = r = 60 drops/mL

Number of drops delivered :

60 drops/mL\times 50 mL = 3000 drops

Time required to deliver 3000 drops = t

Rate of drop solution with respect to time = R = 1 drop/second

\frac{3000 drop}{t}=1 drop/s

t = 3000 seconds = 50 minutes (1 min = 60 seconds)

Number of drops delivered 3000.

50 minutes are required to deliver 50 mL of intravenous solutions.

2) Rate of drops per milliliter of the solution = r = 15 drops/mL

Number of drops delivered :

15 drops/mL\times 50 mL = 750 drops

Time required to deliver 750 drops = t

Rate of drop solution with respect to time = R = 1 drop/second

\frac{750 drop}{t}=1 drop/s

t = 750 seconds = 12.5 minutes (1 min = 60 seconds)

Number of drops delivered 750 .

12.5 minutes are required to deliver 50 mL of intravenous solutions.

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Answer:

5.06 atm

Explanation:

Step 1:

Data obtained from the question. This includes:

Mass of S2O = 175g

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Temperature (T) = 195°C

Pressure (P)

Step 2:

Determination of the number of mole of S2O in 175g of S2O.

Mass of S2O = 175g

Molar Mass of S2O = (32x2) + 16 = 64 + 16 = 80g/mol

Number of mole of S2O =.?

Number of mole = Mass/Molar Mass

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Step 3:

Conversion to appropriate units.

It is essential to always express the various variables in the right units of measurement in order to obtain the desired answer in the right units.

For volume:

1000mL = 1L

Therefore, 16600mL = 16600/1000 = 16.6L

For temperature:

Temperature (Kelvin) = temperature (celsius) + 273

Temperature (celsius) = 195°C

Temperature (Kelvin) = 195°C + 273 = 468K

Step 4:

Determination of the pressure.

The pressure can be obtained by the application of the ideal gas equation. This is illustrated below:

Volume (V) = 16.6L

Temperature (T) = 468K

Number of mole (n) = 2.1875 moles

Gas constant (R) = 0.082atm.L/Kmol

Pressure (P) =

PV = nRT

P x 16.6 = 2.1875 x 0.082 x 468

Divide both side by 16.6

P = (2.1875 x 0.082 x 468) /16.6

P = 5.06 atm

Therefore, the pressure is 5.06 atm

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