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Andrej [43]
3 years ago
12

a patient needs 2.0 grams of medication every 6 hours. The medication is given in tablets. Each tablet contains 250mg of medicat

ion. How many tablets must the patiant take per day?
Chemistry
1 answer:
IgorC [24]3 years ago
3 0

Answer:

\large \boxed{32}

Explanation:

\text{Dosage rate} = \dfrac{\text{2.0 g}}{\text{6 h}}

We must convert this measurement to units of "tablets per day".

1. Convert grams to milligrams

\text{Mass} = \text{2.0 g} \times \dfrac{\text{1000 mg}}{\text{1 g}} = \text{2000 mg}

2. Convert milligrams to tablets

\text{No. of tablets} = \text{2000 mg} \times \dfrac{\text{1 tablet}}{\text{250 mg}} = \text{8.0 tablets}

3. Convert hours to days

\text{Time} = \text{6 h} \times \dfrac{\text{1 da}}{\text{24 h}} = \text{ 0.25 da}

4. Calculate the tablets per day

\dfrac{\text{2.0 g}}{\text{6 h}} = \dfrac{\text{8.0 tablets}}{\text{0.25 da}} = \textbf{32 tablets per day}\\\\\text{The patient must take $\large \boxed{\textbf{32 tablets per day}}$}

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In a polymer with crystalline spherulites and the surrounding amorphous, will have a bigger surrounding amorphous with the presence of residual solvent. Which will decrease the melting range of the crystals. The structure found on the interior of the spherulites is pure crystalline polymer, so probably the residual solvent will not be inside them.

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6 0
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8.937g/cm³

Explanation:

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Edge length = √8 * R

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<em>And there are 4 atoms per unit cell</em>

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4 years ago
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5 0
3 years ago
The normal boiling point of ethanol (C2H5OH) is 78.3 oC and its molar enthalpy of vaporization is 38.56 kJ/mol. What is the chan
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Answer:

The  change in entropy in the system is -231.5 J/K

Explanation:

Step 1: Data given

The normal boiling point of ethanol (C2H5OH) is 78.3 °C = 351.45 K

The molar enthalpy of vaporization of ethanol is 38.56 kJ/mol = 38560 J/mol

Mass of ethanol = 97.2 grams

Pressure = 1 atm

Step 2: Calculate the entropy change of vaporization

The entropy change of vaporization = molar enthalpy of vaporization of ethanol / temperature

The entropy change of vaporization = 38560 J/mol / 351.45 K

The entropy change of vaporization = -109.72 J/k*mol

Step 3: Calculate moles of ethanol

Moles ethanol = mass / molar mass ethanol

Moles ethanol = 97.2 grams / 46.07 g/mol

Moles ethanol = 2.11 moles

Step 4: Calculate  change in entropy

For 1 mol = -109.72 J/K*mol

For 2.11 moles = -231.5 J/K

The  change in entropy in the system is -231.5 J/K

7 0
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