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jenyasd209 [6]
2 years ago
5

our throat is dry, and you want the last cough drop in the box to last a long time in your mouth. What should you do? Keep the c

ough drop whole. This maintains the largest surface-to-volume ratio and slows the dissolution of the cough drop. Break the cough drop into little pieces and put them all in your mouth. Since each little piece must be dissolved separately, the drop will last longer. It doesn't matter if the cough drop is in one piece or many pieces; the total amount of cough drop is all that matters. Break the cough drop into little pieces and put them all in your mouth. This decreases the surface-to-volume ratio and slows the dissolution of the cough drop.
Chemistry
1 answer:
Ann [662]2 years ago
8 0

You should keep the cough drop whole. This maintains the largest surface-to-volume ratio and slows the dissolution of the cough drop.

<h3>Delay of drug action</h3>

The action of the drug can be delayed to either reduce adverse effect if the drugs to the body or to enhance its therapeutic purposes.

Because the throat is dry, the therapeutic purposes of the cough drop would only be achieved if it's dissolution is delayed in the mouth.

To do so, the cough drop should be kept whole to maintain the largest surface-to-volume ratio. This would slow the dissolution of the cough drop.

Learn more about drug here:

brainly.com/question/26254731

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How many grams of Cl2 are in 1.20 x 1024 Cl atoms?
Vaselesa [24]
<h3>Answer:</h3>

70.906 g

<h3>Explanation:</h3>

We are given;

  • Atoms of Chlorine = 1.2 × 10^24 atoms

We are required to calculate the mass of Chlorine

  • We know that 1 mole of an element contains atoms equivalent to the Avogadro's number, 6.022 × 10^23.
  • That is , 1 mole of an element = 6.022 × 10^23 atoms
  • Therefore; 1 mole of Chlorine = 6.022 × 10^23 atoms

But since Chlorine gas is a molecule;

  • 1 mole of Chlorine gas = 2 × 6.022 × 10^23 atoms

But, molar mass of Chlorine gas = 70.906 g/mol

Then;

70.906 g Of chlorine gas = 2 × 6.022 × 10^23 atoms

                                          = 1.20 × 10^24 atoms

Thus;

For 1.2 × 10^24 atoms ;

= ( 70.906 g/mol × 1.2 × 10^24 atoms ) ÷ (1.20 × 10^24 atoms)

<h3>=  70.906 g </h3>

Therefore, 1.20 × 10^24 atoms of chlorine contains a mass of 70.906 g

=  

5 0
2 years ago
Sulfur hexafluoride, SF6, is a colorless, odorless, very unreactive gas. Calculate the pressure (in atm) exerted by 2.02 moles o
miss Akunina [59]

Answer:

9.15 atm

Explanation:

Ideal gas equation of state PV=nRT

P in hPa, V in L, n in mol, R is a constant which is 83.1 hpa*L/mol*k, T in kelvin.

Plug in all the number, and we will get:

P*6.21=2.02*83.1*343

P =9271.6(in hpa)=9.15 atm

8 0
2 years ago
24 CO2 (g) + 26 H2O (i ) + 15,026 kJ - 2 C12H26 (i ) + 37 O2 (g) ?<br><br> Endothermic or exothermic
Sindrei [870]

ibsibjbsi has a lot to do about it but it's

7 0
2 years ago
Write the number 345 in scientific notation, with the same number of significant figures:
uranmaximum [27]

Answer:

3.45 x 10^2

Explanation:

345= 3 SF

3.45 x 10^2= 3 SF

8 0
3 years ago
If you have 2.1 liters of hydrogen gas (at STP), what mass of hydrogen gas would you have?
GuDViN [60]

Answer:

0.19 g

Explanation:

Step 1: Given data

Volume of hydrogen at standard temperature and pressure (STP): 2.1 L

Step 2: Calculate the moles corresponding to 2.1 L of hydrogen  at STP

At STP (273.15 K and 1 atm), 1 mole of hydrogen has a volume of 22.4 L if we treat it as an ideal gas.

2.1 L × 1 mol/22.4 L = 0.094 mol

Step 3: Calculate the mass corresponding to 0.094 moles of hydrogen

The molar mass of hydrogen is 2.02 g/mol.

0.094 mol × 2.02 g/mol = 0.19 g

6 0
3 years ago
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