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devlian [24]
3 years ago
12

The drug labetalol has a dose of 300 mg and is administered in 300 mL of an intravenous infusion at a rate of 2 mg/min. Using an

infusion set that delivers 20 drops/mL, calculate the required drip rate in drops/minute.
Chemistry
1 answer:
Evgesh-ka [11]3 years ago
4 0

Answer:

Explanation:

From the given information:

Since 300 ml of intravenous infusion contains 300 mg of drugs;

Then; 1 ml of intravenous infusion contains (x) amount of drugs

(x) amount of drugs = (300 mg × 1 ml)/ 300 ml

(x) amount of drugs = 1 mg.ml

To calculate the drip rate in drops/minutes by applying conversion factors.

rate (\dfrac{ in \ drops }{minute })= \dfrac{2 \ mg }{min } \times \dfrac{20 \ drops}{1 \ ml} \times \dfrac{1 \ ml }{1 \ mg }

rate (\dfrac{ in \ drops }{minute }) = 40 \  drops / min

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<u>Answer:</u> The freezing point of solution is 2.6°C

<u>Explanation:</u>

To calculate the depression in freezing point, we use the equation:

\Delta T_f=iK_fm

Or,

\Delta T_f=i\times K_f\times \frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ in grams}}

where,

\Delta T_f = \text{Freezing point of pure solution}-\text{Freezing point of solution}

Freezing point of pure solution = 5.5°C

i = Vant hoff factor = 1 (For non-electrolytes)

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M_{solute} = Molar mass of solute (anthracene) = 178.23  g/mol

W_{solvent} = Mass of solvent (benzene) = 79 g

Putting values in above equation, we get:

5.5-\text{Freezing point of solution}=1\times 5.12^oC/m\times \frac{7.99\times 1000}{178.23g/mol\times 79}\\\\\text{Freezing point of solution}=2.6^oC

Hence, the freezing point of solution is 2.6°C

8 0
2 years ago
Why are some amino acids described as essential amino acids?
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Answer:

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6 0
3 years ago
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When magnesium (mg) metal is placed in hydrochloric acid (hcl), it forms magnesium chloride (mgcl2) and a gas. what gas is forme
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Magnesium in hydrochloric acid forms H2 (hydrogen) gas according to the balanced chemical equation:
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2 years ago
A 0.216 g sample of an aluminium compound X reacts with an excess of water to produce a single hydrocarbon gas. This gas burns c
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0.216g of aluminium compound X  react with an excess of water water to produce gas. this gas burn completely  in O2  to form H2O and 108cm^3of CO2 only . the volume of CO2 was measured at room temperature and pressure

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