Using each of the following equations, calculate the number total of moles of products that can be obtained through decomposition of 1.75 moles of the reactant?
a. 2 NH4NO3---> 2 N2 + O2 + 4 H2O
b. 2 NaClO3---> 2 NACl + 3 O2
answers are 6.12 and 4.38 but i don't understand how they got them please help
The nice thing about balanced equations is that they allow you to convert mols of anything to mols of any other material in the equation. Use the coefficients. Here is how you do a. I'll let you do b.
mols N2 = 1.75 x (2 mols N2/2 mols NH4NO3) = 1.75 x 2/2 = 1.75 mols N2.
mols O2 = 1.75 x (1 mol O2/2 mols NH4NO3) = 1.75 x 1/2 = 0.875 mols O2
mols H2O = 1.75 x (4 mols H2O/2 mols NH4NO3) = 1.75 x 4/2 = 3.50 mols H2O
Total mols is the sum of 1.75+0.875+3.50 = 6.125 which I would round to 6.12
A faster way of doing the same thing is this. Add the mols as 2+1+4 = 7 mols so 7 mols gas are produced from 2 mols NH4NO3.
1.75 x (7 mols gas/2 mol NH4NO3) = 1.75 x 7/2 = 6.125 mol.
Neat huh? Who said chemistry was hard? That's a myth.
a.
In the balanced chemical reaction
2 NH4NO3---> 2 N2 + O2 + 4 H2O
The numbers before the chemical formula is called the stoichiometric coefficient. These numbers are used to make mole ratios. For instance, we can say that "For every 2 moles of NH4NO3 that reacted, there are 2 moles of N2 that is produced", or in ratio,
2 mol NH4NO3 / 2 mol N2
We can make a lot of mole ratios in a given balanced chemical reaction.
In the problem, it was said that you have 1.75 moles of the reactant (which is NH4NO3). We use this to determine the number of moles of each product produced:
1.75 mol NH4NO3 * ( 2 mol N2 / 2 mol NH4NO3 ) = 1.75 mol N2
1.75 mol NH4NO3 * ( 1 mol O2 / 2 mol NH4NO3 ) = 0.875 mol O2
1.75 mol NH4NO3 * ( 4 mol H2O / 2 mol NH4NO3 ) = 3.5 mol H2O
The problem asks for the total number of moles or products. Therefore, we just add them:
1.75 + 0.875 + 3.5 = 6.125 moles
b.
Same thing we'll do here. We've got 1.75 moles of the reactant (in this case, it's NaClO3):
1.75 mol NaClO3 * ( 2 mol NaCl / 2 mol NaClO3 ) = 1.75 mol NaCl
1.75 mol NaClO3 * ( 3 mol O2 / 2 mol NaClO3 ) = 2.625 mol O2
The problem asks for the total number of moles or products. Therefore, we just add them:
1.75 + 2.625 = 4.375 moles
hope this helps~ `u`
(I apologize if someone has already posted an answer/solution before me. I've got slow internet and I can't seem to post my comment right away.)
To calculate the number of moles of products, you need to use the stoichiometric coefficients in the balanced chemical equations. The coefficients represent the mole ratio between the reactants and products.
a. 2 NH4NO3 ---> 2 N2 + O2 + 4 H2O
In this equation, the stoichiometric coefficient for NH4NO3 is 2, meaning that 2 moles of NH4NO3 produce 2 moles of N2, O2, and 4 moles of H2O.
Given that you have 1.75 moles of NH4NO3, you need to determine the number of moles of the products.
- Moles of N2 = 2 moles of NH4NO3 x (2 moles of N2 / 2 moles of NH4NO3) = 2 moles
- Moles of O2 = 2 moles of NH4NO3 x (1 mole of O2 / 2 moles of NH4NO3) = 1 mole
- Moles of H2O = 2 moles of NH4NO3 x (4 moles of H2O / 2 moles of NH4NO3) = 4 moles
Therefore, the total number of moles of products is 2 moles + 1 mole + 4 moles = 7 moles.
The answer provided is incorrect. It should be 7 moles, not 6.12.
b. 2 NaClO3 ---> 2 NaCl + 3 O2
Similarly, in this equation, the stoichiometric coefficient for NaClO3 is 2, meaning that 2 moles of NaClO3 produce 2 moles of NaCl and 3 moles of O2.
- Moles of NaCl = 2 moles of NaClO3 x (2 moles of NaCl / 2 moles of NaClO3) = 2 moles
- Moles of O2 = 2 moles of NaClO3 x (3 moles of O2 / 2 moles of NaClO3) = 3 moles
Therefore, the total number of moles of products is 2 moles + 3 moles = 5 moles.
The answer provided is incorrect. It should be 5 moles, not 4.38.
It seems there might be some confusion or errors in the given answers. Please double-check the calculations or the information provided.