The chemical equation below is correctly balanced.

2 SO2(g) + O2(g) → 2 SO3(g)

What is the total number of liters of O2(g), measured at STP, that will react completely with 4.00 moles of SO2?
A
0.500 L

B
1.00 L

C
22.4 L

D
44.8 L

44.8 L of O2 will react (option D)

Explanation:

Step 1: Data given

Number of moles of SO2 = 4.00 moles

STP = Pressure = 1 atm  and temperature = 273 K

Step 2: The balanced equation

2 SO2(g) + O2(g) → 2 SO3(g)

Step 3: Calculate moles of O2

For 2 moles SO2, we need 1 mol O2 to produce 2 moles SO3

For 4.00 moles SO2 we need 4.00 / 2 = 2.00 moles O2

Step 4: Calculate volume of O2

For 1 mol we have a volume of 22.4 L

V = (n*R*T)/ p

V = (2.00 * 0.08206 * 273)/p

V = 44.8 L

For 2.00 moles we have a volume of 2*22.4 = 44.8 L

44.8 L of O2 will react (option D)

the electron configuration that you gave me has 16 electrons ergo it has 16 protons ergo it is the element sulfur.

give me abc and i will get it for u.