Roughness of the surface and weight of the object.
The number of atoms that are in 0.32 g of copper are
3.01 x10^21 atoms
<u><em>calculation</em></u>
<u><em> </em></u>Step 1: find the number of moles of Copper
moles = mass/molar mass
= 0.32 g /63.5 g/mol=0.005 moles
Step 2: use the Avogadro's constant to determine the number of atom
in 0.005 moles of Cu
that is according to Avogadro's law 1 mole =6.02 x10^23 atoms
0.005 moles=? atoms
by cross multiplication
= (0.005 moles x 6.02 x10^23 atoms) / 1 mole= 3.01 x10 ^21 atoms
i tried my hardest and its not aExplanation:
Answer:
The answer to the question is
The pressure of carbon dioxide after equilibrium is reached the second time is 0.27 atm rounded to 2 significant digits
Explanation:
To solve the question, we note that the mole ratio of the constituent is proportional to their partial pressure
At the first trial the mixture contains
3.6 atm CO
1.2 atm H₂O (g)
Total pressure = 3.6+1.2= 4.8 atm
which gives
3.36 atm CO
0.96 atm H₂O (g)
0.24 atm H₂ (g)
That is
CO+H₂O→CO(g)+H₂ (g)
therefore the mixture contained
0.24 atm CO₂ and the total pressure =
3.36+0.96+0.24+0.24 = 4.8 atm
when an extra 1.8 atm of CO is added we get Increase in the mole fraction of CO we have one mole of CO produces one mole of H₂
At equilibrium we have 0.24*0.24/(3.36*0.96) = 0.017857
adding 1.8 atm CO gives 4.46 atm hence we have
(0.24+x)(0.24+x)/(4.46-x)(0.96-x) = 0.017857
which gives x = 0.031 atm or x = -0.6183 atm
Dealing with only the positive values we have the pressure of carbon dioxide = 0.24+0.03 = 0.27 atm
