The pressure that would be needed is 5.06 atm.
What is pressure?
Pressure is the force exerted perpendicular to any object.
The mass of disulfur monoxide gas is 175 g
Volume is 16,600 ml
Temperature is 195
Step 1: Calculating the moles
[tex]\rm Number\;of \;moles= \dfrac{mass}{molar\;mass}\\\\\rm Number\;of \;moles= \dfrac{175}{80 g/mol} = 2.1875\; moles[/tex]
Step2 : calculating the pressure
By the formula of PV= NRT
V = 16600mL = 16600/1000 = 16.6L
Temp. = 195°C + 273 = 468K
r = gas constant os 0.082atm.L/Kmol
Putting the value in the equation
[tex]\rm P \times 16.6 = 2.1875 \times 0.082 \times 468\\\\P =\dfrac{ (2.1875 \times 0.082 \times 468) }{16.6} = 5.06 atm[/tex]
Thus, the pressure is 5.06 atm.
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