Help a brother out!!! please!!!Nitroglycerin, C3H5N3O9 decomposes to form N2,CO2,H2O, and O2

4(C3H5N3O9)-> 6N2+12O2+10H20+O2

a)How many grams of water would be produced if 75g of nitroglycerin decompose?
b)The creation of 3.89 moles of C02 would require how many grams of nitroglycerin
TY!

Correction!! in the question its **12CO2**

Nitroglycerin = NG

mols NG = grams/molar mass = ?
Use the coefficients in the balanced equation to convert mols NG to mols H2O.
Now convert mols H2O to grams. g = mols x molar mass

b.
Convert 3.89 mols CO2 to mols NG using the coefficients.
Then g NG = mols NG x molar mass NG

a) To determine how many grams of water would be produced if 75g of nitroglycerin decomposes, we need to use a balanced chemical equation and molar ratios.

First, let's calculate the molar mass of nitroglycerin (C3H5N3O9):
C = 12.01 g/mol
H = 1.01 g/mol
N = 14.01 g/mol
O = 16.00 g/mol

Molar mass of nitroglycerin = (3 * 12.01) + (5 * 1.01) + (3 * 14.01) + (9 * 16.00) = 227.09 g/mol

Now, we need to determine the molar ratio between nitroglycerin and water in the balanced chemical equation:
4(C3H5N3O9) -> 6N2 + 12O2 + 10H2O + O2

From the equation, we can see that for every 4 moles of nitroglycerin, 10 moles of water are produced.
So, the molar ratio between nitroglycerin and water is 4:10.

To calculate the number of moles of nitroglycerin, we use the equation:
Moles = Mass (g) / Molar mass (g/mol)

Moles of nitroglycerin = 75 g / 227.09 g/mol = 0.33 mol

Now, we can use the molar ratio to determine the moles of water produced:
Moles of water = Moles of nitroglycerin * (10/4) = 0.33 mol * (10/4) = 0.825 mol

Finally, we can calculate the mass of water produced:
Mass of water = Moles of water * Molar mass of water

Molar mass of water (H2O) = 2 * 1.01 + 16.00 = 18.02 g/mol

Mass of water = 0.825 mol * 18.02 g/mol = 14.84 g

Therefore, approximately 14.84 grams of water would be produced if 75 grams of nitroglycerin decomposes.

b) To calculate the grams of nitroglycerin required to produce 3.89 moles of CO2, we follow a similar process.

First, let's determine the molar ratio between nitroglycerin and CO2 in the balanced chemical equation:
4(C3H5N3O9) -> 6N2 + 12O2 + 10H2O + O2

From the equation, we can see that for every 4 moles of nitroglycerin, 6 moles of CO2 are produced.
So, the molar ratio between nitroglycerin and CO2 is 4:6.

To calculate the moles of nitroglycerin required, we use the equation:
Moles = Moles of CO2 * (4/6)

Moles of nitroglycerin = 3.89 mol * (4/6) = 2.59 mol

Finally, we can calculate the mass of nitroglycerin required:
Mass = Moles of nitroglycerin * Molar mass

Mass of nitroglycerin = 2.59 mol * 227.09 g/mol = 587.85 g

Therefore, approximately 587.85 grams of nitroglycerin would be required to produce 3.89 moles of CO2.