For the reaction shown, calculate how many moles of NO2 form when each amount of reactant completely reacts. 2N2O5g = 4NO2g+O2g

I am assuming that the first question must be converted to grams and the second question must be converted to kilograms

I just need to know how to convert I guess to grams and kilograms to get the answer. And then I am not to sure I am even asking the right questions. But the way I am presenting the questions to you is how it was presented to me. Actually the first two question was 1.6 moles and 6.2 moles N205 and that was easy but the last two question that I am asking you for help with is different instead of moles its grams and kilo grams.

Please help it will be most appreciated.

11.0 g N2O5
1.70 kg N205

You always work in mols with stoichiometry problems (actually there is one type problem that you don't need to convert to mols but converting to mols will always work).

mol = grams/molar mass
If in kg, then kg x 1000 = g, then mols = g/molar mass.

To convert the given amounts of N2O5 into moles, you can use the molar mass of N2O5. The molar mass of N2O5 is calculated as follows:

N = 14.01 g/mol
O = 16.00 g/mol

Molar mass of N2O5 = 2(N) + 5(O) = 2(14.01 g/mol) + 5(16.00 g/mol) = 108.02 g/mol

1. Given 11.0 g N2O5:
To convert grams to moles, use the formula:

moles = mass / molar mass

moles = 11.0 g / 108.02 g/mol ≈ 0.102 mol

Therefore, when 11.0 g of N2O5 reacts completely, it forms approximately 0.102 moles of NO2.

2. Given 1.70 kg N2O5:
To convert kilograms to grams, multiply by 1000:

1.70 kg * 1000 g/kg = 1700 g

To convert grams to moles, use the formula:

moles = mass / molar mass

moles = 1700 g / 108.02 g/mol ≈ 15.75 mol

Therefore, when 1.70 kg (or 1700 g) of N2O5 reacts completely, it forms approximately 15.75 moles of NO2.

To convert from moles to grams, you need to use the molar mass of the substance. The molar mass of a substance is the mass of one mole of that substance and is expressed in grams per mole (g/mol). You can find the molar mass of a compound by adding up the atomic masses of all the elements in that compound.

For the first question, calculating how many moles of NO2 form when 11.0 g of N2O5 completely reacts:
1. Determine the molar mass of N2O5. Nitrogen (N) has a molar mass of 14.01 g/mol, and oxygen (O) has a molar mass of 16.00 g/mol.
Molar mass of N2O5 = (2 * molar mass of N) + (5 * molar mass of O) = (2 * 14.01 g/mol) + (5 * 16.00 g/mol) = 108.02 g/mol

2. Convert the mass of N2O5 to moles using the formula: moles = mass / molar mass.
Moles of N2O5 = 11.0 g / 108.02 g/mol = 0.102 moles

3. The balanced equation tells us that for every 2 moles of N2O5, 4 moles of NO2 are formed.
Since the ratio is 2:4, we can multiply the moles of N2O5 by the stoichiometric coefficient ratio to find the moles of NO2.
Moles of NO2 = 0.102 moles N2O5 * (4 moles NO2 / 2 moles N2O5) = 0.204 moles NO2

Therefore, when 11.0 g of N2O5 completely reacts, 0.204 moles of NO2 form.

For the second question, calculating how many moles of NO2 form when 1.70 kg of N2O5 completely reacts:

1. Convert the mass of N2O5 from kilograms to grams. Since 1 kilogram equals 1000 grams, multiply the given mass by 1000.
Mass of N2O5 = 1.70 kg * 1000 g/kg = 1700 g.

2. Follow the previous steps from question 1 to calculate the moles of NO2 using the mass of N2O5 (1700 g) instead of the moles.

Therefore, when 1.70 kg (1700 g) of N2O5 completely reacts, you will calculate the moles of NO2 using the steps mentioned above.