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3 years ago

There are 0.3 moles of xenon gas in a 0.5-liter container at 30 degrees C. What is the pressure exerted by the xenon gas

Chemistry

2 answers:

zhenek [66]3 years ago

4 0

Answer : The pressure of the gas is, 14.925 atm

Solution :

using ideal gas equation,

$PV=nRT$

where,

n = number of moles of gas = 0.3 mole

P = pressure of the gas = ?

T = temperature of the gas = $30^oC=273+30=303K$

R = gas constant = 0.0821 Latm/moleK

V = volume of the gas = 0.5 L

Now put all the given values in the above equation, we get the pressure of the gas.

$P\times (0.5L)=(0.3mole)\times (0.0821L.atm/mole.K)\times (303K)$

$P=14.925atm$

Therefore, the pressure of the gas is, 14.925 atm

Kaylis [27]3 years ago

3 0

PV = nRT
P = (nRT)/V
P = (0.3 mol × 0.08206 atm-l/(mol-K) × (273.15 + 30) K)/(0.5 l)
P = 14.9258934 atm

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klemol [59]

Answer: The percentage yield of aspirin is 38.02 %.

Explanation:

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$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

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Given mass of salicylic acid $(C_7H_6O_3)$ = 10.09 g

Molar mass of salicylic acid $(C_7H_6O_3)$ = 138.12 g/mol

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$\text{Moles of salicylic acid}=\frac{10.09g}{138.12g/mol}=0.0730mol$

The chemical equation for the formation of aspirin follows:

$C_7H_6O_3+C_4H_6O_3\rightarrow C_9H_8O_4+CH_3COOH$

As, acetic anhydride is present in excess. So, it is considered as an excess reagent.

Thus, salicylic acid is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of salicylic acid produces 1 mole of aspirin.

So, 0.0730 moles of salicylic acid will produce = $\frac{1}{1}\times 0.0730=0.0730mol$ of aspirin

Now, calculating the mass of aspirin from equation 1, we get:

Molar mass of aspirin = 180.16 g/mol

Moles of aspirin = 0.073 moles

Putting values in equation 1, we get:

$0.073mol=\frac{\text{Mass of aspirin}}{180.16g/mol}\\\\\text{Mass of aspirin}=13.15g$

To calculate the percentage yield of aspirin, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Experimental yield of aspirin = 5.0 g

Theoretical yield of aspirin = 13.15 g

Putting values in above equation, we get:

$\%\text{ yield of aspirin}=\frac{5.0g}{13.15g}\times 100\\\\\% \text{yield of aspirin}=38.02\%$

Hence, the percent yield of aspirin is 38.01 %.

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