Respuesta :
Answer:
We need 128 liters of a gaseous hydrogen bromide
Explanation:
Step 1:
Temperature = 58°C
Pressure = 0.891 atm
Volume ofHydrobromic acid we want to prepare is 3.50 L (1.20M)
Step 2: Calculate moles HBr
Moles HBr = molarity * volule
Moles HBr = 1.20 * 3.50 L
Moles HBr = 4.20 moles HBr
Step 3: Calculate volume of Hydrogen bromide
pV = nRT
V=(nRT)/P
⇒ with V = the volume of gaseous hydrogen bromide = ?
⇒with p = the pressure of the gas = 0.891 atm
⇒ with n = the number of moles of hydrogen bromide = 4.2 moles
⇒ with R = the gasconstant = 0.08206 L*atm / mol*K
⇒ with T = the temperature = 58.0 °C = 273 + 58 = 331 Kelvin
V = (4.2*0.08206*331)/0.891
V = 128 L
We need 128 liters of a gaseous hydrogen bromide
The number of the moles can be used in the ideal gas equation to know the volume, pressure and temperature. The volume of HBr required is 128 L.
What is the ideal gas equation?
The ideal gas equation is the hypothetical equation of the gas that depicts the relation of the pressure, volume, temperature and moles of the gas.
Given,
The temperature of hydrogen bromide (T) = 331 Kelvin
The volume of hydrogen bromide (V) = ?
The pressure of hydrogen bromide (P) = 0.891 atm
Gas constant (R) = 0.08206
The number of moles of hydrogen bromide (n) can be calculated as:
[tex]\begin{aligned}\rm moles &= \rm Molarity \times volume\\\\&= 1.20 \;\rm M \times 3.50\;\rm L\\\\&= 4.20\;\rm mol\end{aligned}[/tex]
Now, using the ideal gas equation the volume of the gas can be calculated as:
[tex]\begin{aligned} \rm V &= \rm \dfrac{nRT}{P}\\\\&= \dfrac{4.2 \times 0.08206\times 331}{0.891}\\\\&= 128\;\rm L\end{aligned}[/tex]
Therefore, 128 L of hydrogen bromide will be required.
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