What volume (L) would be produced from 1.5x1025 molecules of CO2 at STP?

557.7 L

Explanation:

1 mol → 6.02×10²³ molecules at STP produces 22.4L

Therefore, we need to know how many moles are 1.5 ×10²⁵ molecules

( 1.5 ×10²⁵ molecules / 6.02×10²³ molecules) . 1 mol = 24.9 moles

Let's make a rule of three:

1 mol can produce at STP a volume of 22.4 L

24.9 moles may produce at STP a volume of (24.9 . 22.4)/1 = 557.7 L

Let's verify by the Ideal Gases Law

P . V = n . R . T → V = (n . R . T ) / P

STP → Pressure = 1 atm, T = 273 K

V = (24.9 mol . 0.082 L.atm/mol.K . 273 K) / 1 atm → 557.4 L

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.

the density of gold = 19.3 g/cm3

the relation between density and mass and volume is

density = mass / volume

given :

mass of gold = 13 g

density = 13g / volume = 19.3

volume = 13 /19.3 = 0.67 cm^3

thus volume of gold nugget = 0.67 cm^3