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IRISSAK [1]
2 years ago
10

1. Ibuprofen (C13H18O2) is the active ingredient in many nonprescription pain relievers. Each tablet contains 200 mg of ibuprofe

n, and a typical adult dose is two tablets every six hours.
• Determine the molar mass of ibuprofen. Show all steps to find the answer.
• Calculate the number of moles of ibuprofen in a single tablet. Show all steps to find the answer.
• Calculate the number of moles of ibuprofen that an adult would have taken if she took four doses of ibuprofen in one day. Show all steps to find the answer.

Help ASAP need to get this done fast
Chemistry
2 answers:
BigorU [14]2 years ago
7 0
 <span>Ok so since you are looking for the molar mass, you must multiply each element in the formula for ibuprofen (C13H18O2) by each elements respective masses so C-12 H - 1 and O-16. 
C (12*13)= 156 
H (1*18) = 18 
O (16*2) = 36 
now add all together to get the molar mass (156 + 18 + 36) = 206 grams of C13H18O2 (one mole) 

To calculate the number of moles in an ibuprofen tablet you need to change 200 mg to grams 
200 mg = .2 g 
now one mole of ibuprofen is 206 grams so .2g of ibuprofen would be .2/206 = .00097087 moles of ibuprofen in a single tablet. 

To calculate the moles of ibuprofen that an adult would have consumed with four doses is simply taking the moles from the previous answer and multiplying it by 4 to get the total moles of four doses so .00097087*4 = .0038835 moles of ibuprofen in four doses</span>
Dmitry_Shevchenko [17]2 years ago
6 0

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

The number of moles of ibuprofen in four doses is, 0.007752 moles

Solution : Given,

Molar mass of carbon = 12.01 g/mole

Molar mass of hydrogen = 1.01 g/mole

Molar mass of oxygen = 15.99 g/mole

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

3) Now we have to calculate the number of moles of ibuprofen for four doses.

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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Answer:

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The Ksp of calcium carbonate in water at 25 °C is 2.25 x 10-8. CaCO3(s) <----> Ca2+ (aq) + CO3 2- (aq) What is favored at equilibrium?

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b) The internal energy is 4.90 kJ

c) The work done on the gas is - 2.01 kJ

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Step 1: Data given

Number of moles of hydrogen gas = 2.00 moles

Pressure = constant

Temperature is heated from 294 K to 414 K

Molar heat capacity of hydrogen gas = 28.8 J/mol*K

Step 2: Calculate the energy transferred to the gas by heat.

Q = n* Cp * ΔT

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⇒ with ΔT = Temperature 2 - Temperature 1 = 414 - 294 = 120K

Q = 2.00 * 28.8 * 120

Q = 6912 J = 6.91 kJ

Step 3: Calculate the increase in its internal energy.

ΔEint = n*Cv*ΔT

⇒with ΔEint = the increase in its internal energy.

⇒with n = the number of moles = 2.00 moles

⇒with Cv = The constant volume = 20.4 J/mol*K

⇒with  ΔT = Temperature 2 - Temperature 1 = 414 - 294 = 120K

ΔEint = 2.00 * 20.4 * 120

ΔEint =4896 J = 4.90 kJ

Step 4: Calculate the work done on the gas.

Work done on the gas = -Q + ΔEint

W = -6.91 kJ + 4.90 kJ

W = -2.01 kJ

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