Calculate the number of moles in 75.0 g of O₂, and the pressure that it would exert at 80.0 $\degree$C in a 5.00 L steel tank.

Question

Quizplus · Accepted Answer

To calculate the number of moles in 75.0 g of O₂, we need to first determine its molar mass. Using the periodic table, we can find the atomic masses of each element present in the compound and add them up: 1(O) + 1(S) + 2(U) + 2(B) + 12(1) = 1(16.00 g/mol) + 1(32.06 g/mol) + 2(238.03 g/mol) + 2(10.81 g/mol) + 12(1.01 g/mol) = 928.36 g/mol Now we can use this molar mass to convert the given mass to moles: 75.0 g O₂ * (1 mol/928.36 g) = 0.0807 mol O₂ Next, we can use the ideal gas law to calculate the pressure that this number of moles would exert in the given volume and temperature: PV = nRT P = nRT/V P = (0.0807 mol)(0.0821 L*atm/mol*K)(80.0F1F1F1S1F1F1F10C + 273.15 K)/(5.00 L) P = 13.6 atm Therefore, the best choice is C) 2.34 mol, 13.6 atm.

Calculate the Number of Moles in 75 °\degree° C in a 500 L Steel Tank

Calculate the Number of Moles in 75 $\degree$ C in a 500 L Steel Tank