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Radda [10]
2 years ago
10

Aspirin is a medicine for use by adults.

Chemistry
1 answer:
kogti [31]2 years ago
4 0
<span>Aspirin is the prototypical analgesic used in the treatment of mild to moderate pain. It has anti-inflammatory and antipyretic properties and acts as an inhibitor of cyclooxygenase which results in the inhibition of the biosynthesis of prostaglandins. Aspirin also inhibits platelet aggregation and is used in the prevention of arterial and venous thrombosis. (From Martindale, The Extra Pharmacopoeia, 30th ed, p5)</span>
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What does radiochemical dating do
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Radiometric dating, often called radioactive dating, is a technique used to determine the age of materials such as rocks.

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Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfr
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Answer:

a. 4 C_3H_5N_3O_9 (l)\rightarrow 6N_2 (g) + O_2 (g) + 10 H_2O (g) + 12 CO_2 (g)

b. 146.0 g

Explanation:

Question 1 (a). Just as the problem states, liquid nitroglycerin decomposes into nitrogen gas N_2, oxygen gas O_2, water vapor H_2O and carbon dioxide CO_2. Let's write the decomposition of nitroglycerin into these 4 components:

C_3H_5N_3O_9 (l)\rightarrow N_2 (g) + O_2 (g) + H_2O (g) + CO_2 (g)

Now we need to balance the equation. Firstly, notice we have 3 carbon atoms on the left and 1 on the right, so let's multiply carbon dioxide by 3:

C_3H_5N_3O_9 (l)\rightarrow N_2 (g) + O_2 (g) + H_2O (g) + 3 CO_2 (g)

Now, we have 3 nitrogen atoms on the left and 2 on the right, so let's multiply nitrogen on the right by \frac{3}{2}:

C_3H_5N_3O_9 (l)\rightarrow \frac{3}{2}N_2 (g) + O_2 (g) + H_2O (g) + 3 CO_2 (g)

We have 5 hydrogen atoms on the left, 2 on the right, so let's multiply the right-hand side by \frac{5}{2}:

C_3H_5N_3O_9 (l)\rightarrow \frac{3}{2}N_2 (g) + O_2 (g) + \frac{5}{2} H_2O (g) + 3 CO_2 (g)

Finally, count the oxygen atoms. We have a total of 9 on the left. On the right we have (excluding oxygen molecule):

\frac{5}{2} + 6 = 8.5

This leaves 9 - 8.5 = 0.5 = \frac{1}{2} of oxygen. Since oxygen is diatomic, we need to take one fourth of it to get one half in total:

C_3H_5N_3O_9 (l)\rightarrow \frac{3}{2}N_2 (g) + \frac{1}{4} O_2 (g) + \frac{5}{2} H_2O (g) + 3 CO_2 (g)

To make it look neater without fractional coefficients, multiply both sides by 4:

4 C_3H_5N_3O_9 (l)\rightarrow 6N_2 (g) + O_2 (g) + 10 H_2O (g) + 12 CO_2 (g)

Question 2 (b). Now we can make use of the balanced chemical equation and apply it for the context of this separate problem. We're given the following variables:

V_{CO_2} = 41.0 L

T = -14.0^oC + 273.15 K = 259.15 K

p = 1 atm

Firstly, we may find moles of carbon dioxide produced using the ideal gas law pV = nRT.

Rearranging for moles, that is, dividing both sides by RT (here R is the ideal gas law constant):

n_{CO_2} = \frac{pV_{CO_2}}{RT} = \frac{1 atm\cdot 41.0 L}{0.08206 \frac{L atm}{mol K}\cdot 259.15 K} = 1.928 mol

According to the stoichiometry of the balanced chemical equation:

4 C_3H_5N_3O_9 (l)\rightarrow 6N_2 (g) + O_2 (g) + 10 H_2O (g) + 12 CO_2 (g)

4 moles of nitroglycerin (ng) produce 12 moles of carbon dioxide. From here we can find moles o nitroglycerin knowing that:

\frac{n_{ng}}{4} = \frac{n_{CO_2}}{12} \therefore n_{ng} = \frac{4}{12}n_{CO_2} = \frac{1}{3}\cdot 1.928 mol = 0.6427 mol

Multiplying the number of moles of nitroglycerin by its molar mass will yield the mass of nitroglycerin decomposed:

m_{ng} = n_{ng}\cdot M_{ng} = 0.6427 mol\cdot 227.09 g/mol = 146.0 g

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