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Sagot :
Answer: The pressure is 8451.2 torr.
Explanation:
Given: Mass of He = 7.55 g
Volume = 5520 mL
Convert mL into L as follows.
[tex]1 mL = 0.001 L\\5520 mL = 5520 mL \times \frac{0.001 L}{1 mL}\\= 5.520 L[/tex]
Temperature = [tex]123^{o}C = (123 + 273) K = 396 K[/tex]
Now, moles of He (molar mass = 4.00 g/mol) are as follows.
[tex]No. of moles = \frac{mass}{molar mass}\\= \frac{7.55 g}{4 g/mol}\\= 1.8875 mol[/tex]
Formula used to calculate pressure is as follows.
PV = nRT
where,
P = pressure
V = volume
n = no. of moles
R = gas constant = 0.0821 L atm/mol K
T = temperature
Substitute the values into above formula as follows.
[tex]PV = nRT\\P \times 5.520 L = 1.8875 mol \times 0.0821 L atm/mol K \times 396 K\\P = 11.12 atm[/tex]
Convert atm into torr as follows.
1 atm = 760 torr
[tex]11.12 atm = 11.12 atm \times \frac{760 torr}{1 atm}\\= 8451.2 torr[/tex]
Thus, we can conclude that the pressure is 8451.2 torr.
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