Respuesta :
Answer
The pressure inside the cylinder will change to 14.686 atm
Explanation
Given:
Volume, V = 0.500 L
Moles of O2 = 0.150 mol
Temperature, T = 25 °C = (25 + 273.15 K) = 298.15 K
Step-by-step solution:
The first step is to calculate the pressure exerted by O2 using ideal gas equation:
[tex]\begin{gathered} PV=nRT \\ \end{gathered}[/tex]Plugging the values of the parameters into the formula:
[tex]\begin{gathered} P\times0.500\text{ }L=0.150\text{ }mol\times0.0821\text{ }atm•L/mol•K\times298.15K \\ \\ P=\frac{3.67171725\text{ }atm.L}{0.500L}=7.343\text{ }atm \end{gathered}[/tex]The pressure exerted by O2 = 7.343 atm
If 0.150 mol of sulfur dioxide, SO2 was added to the oxygen gas already in the cylinder, then the pressure inside the cylinder will change by a factor of 2. That is:
Total pressure will be = 2 x 7.343 atm = 14.686 atm
Or the total pressure can be calculated using the ideal equation above, and putting n = 0.150 mol + 0.150 mol = 0.3 mol
[tex]\begin{gathered} P\times0.500\text{ }L=0.30\text{ }mol\times0.0821\text{ }atm•L/mol•K\times298.15K \\ \\ P=\frac{7.3434345\text{ }atm.L}{0.500L}=14.686\text{ }atm \end{gathered}[/tex]