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Alexeev081 [22]
3 years ago
5

At a certain temperature the vapor pressure of water is 32 torr. The pressure of the gas in a soda bottle (carbonated water) is

measured to be 890 torr. What is the pressure (in torr) of the carbon dioxide in the soda bottle?
Chemistry
1 answer:
jekas [21]3 years ago
8 0

<u>Answer:</u> The partial pressure of carbon dioxide is 858 torr

<u>Explanation:</u>

Dalton's law of partial pressure states that the total pressure of the system is equal to the sum of partial pressure of each component present in it.

To calculate the partial pressure of hydrogen gas, we use the law given by Dalton, which is:

P_T=p_{CO_2}+p_{H_2O}

We are given:

Total pressure of the carbonated drink, P_T = 890 torr

Vapor pressure of water, p_{H_2O} = 32 torr

Putting values in above equation, we get:

890=p_{CO_2}+32\\\\p_{CO_2}=890-32=858torr

Hence, the partial pressure of carbon dioxide is 858 torr.

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Answer :

The molar mass of ibuprofen is, 206.29 g/mole.

The number of moles of ibuprofen in a single tablet is, 0.000969 moles

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Solution : Given,

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1) Now we have to calculate the molar mass of ibuprofen.

Molar mass of ibuprofen, C_{13}H_{18}O_2 = (13\times 12.01)+(18\times 1.01)+(2\times 15.99)=206.29g/mole

The molar mass of ibuprofen = 206.29 g/mole

2) Now we have to calculate the moles of ibuprofen.

Formula used : Moles=\frac{Mass}{\text{ Molar mass}}

Given : Mass of ibuprofen = 200 mg = 0.2 g         (1 mg = 1000 g)

\text{ Moles of ibuprofen}=\frac{\text{ Mass of ibuprofen}}{\text{ Molar mass of ibuprofen}}=\frac{0.2g}{206.29g/mole}=0.000969moles

The moles of ibuprofen = 0.000969 moles

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Number of tablets in one dose = 2

Total number of tablets in 4 doses = 4 × 2 = 8

Number of moles of ibuprofen in 8 tablets =

\text{ Number of moles of ibuprofen in 1 tablet}\times \text{ Total number of tablets}=0.000969\times 8=0.007752moles

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