Chemistry Question Mole Conversion To G

Mole conversions?? (chemistry question..help!)?

To convert grams to moles, you have to find the molar mass of the element and divide.
To find the molar mass, you take the atomic weight of the element. If it's a compound, add all of the weights together... but you don't have to worry about that for now!
So iron. Find Fe on the Periodic Table. Its atomic weight should be 55.85 grams.
Take your amount, which is 525 g, and divide it by the molar mass, 55.85 g to get the moles.
Here's a more visual way to think of it:

525 g Fe x 1 mole/55.85 g.

The units cancel out, leaving the units as moles.
The answer is 9.40 moles. Leave the 0 at the end, because it's a significant figure.


For moles to atoms, you have to multiply by Avogadro's Number, which is 6.02*10^23.
So...
.50 mole Li x 6.02*10^23/1 mole.
The answer is 3.0*10^23.
You don't need to find the molar mass in this one, since it's already in moles.


I hope this helped...!
Now go blossom into what my chem teacher calls a "GACC", A Good And Careful Chemist! :]

Chemistry Questions about Mole and gram conversion?

Explain the answers in complete sentences (just paraphrase and I can make sentences)
Styrofoam (C8H8)

If you obtain 10.0 g of each substance (sugar, NaCl, and Styrofoam) will each sample have the same number of moles? Explain answer.

If you obtain 10.0 g of each substance (sugar, NaCl, and Styrofoam) will each sample have the same number of particles? Explain answer.

If you obtain 10.0 moles of each substance (sugar, NaCl, and Styrofoam) will each sample have the same number of particles? Explain your answer.

The Law of conservation of matter states the mass is conserved (stays the same).
Calculate the molar mass of each of the reactants and products in the following chemical reaction.
C12H22)11+O2->CO2+H2O

calculate the total mass of the reactants and compare it to the total mass of the products, are they equal?

If mass is not conserved, how can you fix this problem in the equation? Show how you would do so.

Chemistry question(Mole conversions)!!!?

The formula unit mass (molar mass) = 1 Na @ 22.990 + 1 Cl @ 35.453 = 58.443 g
3.55 mole x 58.443 g/mole = 207 g

Chemistry Mole Conversion Questions?

1 mole of any molecule has 6.O22x10^23 molecules
1 mole of any atom has 6.022x10^23 atoms
6.022x10^23 is called avagadros number

So 1 mole C3H8 has 6.022x10^23 molecules of C3H8

BUT 1 molecule of C3H8 consists of
3 atoms of C
8 atoms of H

So 1 mole C3H8 has
3 moles C atoms
8 moles H atoms

moles = mass / molar mass
molar mass C3H8 = (3 x 12) + (8 x 1) = 44 g/mol
moles C3H8 = 44 g / 44 g/mol
= 1.0 moles of C3H8

Therefore you have 3 moles of C

number molecules = moles x 6.022x10^23
= 1.8x10^24 atoms of C

Chem questions (mole conversions)?

just some questions for those who can chem (:

1) a 28.9-L sample of NO2 at STP will have what mass?
2) how many moles of NaBr are 307.3g NaBr
3) an experiment calls for 0.30 miles of CaCl2. this is equivalent to how many grams?
4) an experiment calls for 0.48 miles of Mg(OH)2. this is equivalent to how many grams?
5) a 34.1L sample of SO3 at STP will have what mass?
6) a sample of 0.52 moles of NO2 occupies what volume (in liters) at STO
7) a sample of CH4 occupies a volume of 27.6L at STP. how many miles of CH4 are present in this sample?

please show how you did them!!!!

thank you!! (:

Chemistry- grams to moles conversion?

Copper = 63.546g in 1 mol
Therefore:
0.40g = 0.40/63.546 = 0.0063 mol
0.31g = 0.31/63.546 = 0.0049 mol

Chemistry Mole Conversions?

Jerome was asked to preform the following chemical reaction. He placed 5.0g of zinc metal into a bottle and covered the mouth of the bottle with a 2 hole stopper. He poured 150ml of 2.0M HCL through the funnel onto the zinc.
1. write a balanced equation for this reaction between the zinc and the acid?
2.Identify the reaction?
3.Calculate the number of moles of zinc that jerome placed in the bottle at the beginning of the experiment ?
4.if all the zinc reacts, the number of moles of zinc consumed will be the same as the number of moles of H2(gas) produced? How many molecules of hydrogen gas will be produced in this reaction?
5. Calculate the Volume of the Hydrogen gas produced in this reaction at STP? (At STP, 1mol of gas occupies 22.4L)
6. Calculate the mass of hydrogen that will be collected in the inverted bottle?
7.Predict the mass of hydrogen that would have been produced if jerome had started with twice the original mass of zinc? Assume that all of the zinc would react?

~ Please if you can Answer this please do its an extra credit thing and i have to bring my 65% D up to a C pleaseee if you can do anything THANKYOU THANKYOU ((: