How many moles of carbon monoxide gas in 13.7L at STP

0.0611 mol

Explanation:

Use equation:

PV = nRT

Questions tells us that the volume is 13.7 L

The pressure at STP is 1 atm

The temperature at STP is 273 K

The gas constant is 0.0821  atm L

Rearranged to give us n:

n = PV / RT

n = (1 atm) (13.7 L) / (0.0821 atm L ) (273 K)

n = 0.0611 mol (3 sig figs)

h let me think

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.