Answer: 1.2 x 10^-17 microounces
Explanation:
Ounce = 28.5G microounce = 28.5*10^-6g
3.4*10^-25 kg = 3.4*10^-22 g = (3.4/2.85)*10^(-22+5) = 1.2*10-17
Mass:20g
Mole=20/[2(23)+16]
=0.32 mil
Answer:
You need to make sure the number of atoms of each element on the reactant side is equal to the number of atoms of each element on the product side. In order make both sides equal, you will need to multiply the number of atoms in each element until both sides are equal. :)
Answer:
Unbalanced
Explanation:
The balanced equation would be:
C3H8 + <u> 5 </u>O2 ---> <u> 4 </u>H2O + <u> 3 </u>CO2
Answer:
58.7g
Explanation:
From the reaction equation, we can see that 3 moles of oxygen yielded 2 moles of carbon (iv) oxide. Let's keep this for later.
Now, we calculate the actual number of moles of oxygen reacted. This can be calculated as follows.
The number of moles of oxygen reacted = mass of oxygen reacted ÷ molar mass of oxygen molecule.
The mass of oxygen reacted is 64g. Now, the molar mass of the oxygen molecule can be calculated from the atomic mass of the oxygen atom. The atomic mass of the oxygen atom is 16 a.m.u .Hence the molar mass = 2 × 16 = 32g/mol.
The number of moles is thus 64 ÷ 32 = 2 moles.
We now calculate the number of moles of Carbon iv oxide yielded.
As said from the beginning of the equation, 3 moles oxygen yielded 2 moles 2 moles CO2. Hence, moles oxygen will yield (2 ×2) ÷ 3 = 4/3 moles O2.
Now we calculate the mass of CO2 yielded.
The mass is = number of moles of CO2 yielded × molar mass of CO2.
Molar mass of CO2 = 12 + 2(16) = 44g/mol.
The mass is thus = 4/3 × 44 = 58.66667g
