NH4NO3(s) ¡æ N2O(g) + 2H2O(§¤).
How much water is produced if 22.9 g of N2O is produced in this reaction? Answer in units of g
I converted grams of N2O to mol. Then I did a mol ratio getting mol of H2O. Then I converted mol of H2O to grams. I got 18.736363. Is this correct?
Yes but that's too many significant figures.
To determine the amount of water produced in the reaction, you correctly followed the steps of converting grams of N2O to moles, using the mole ratio to find moles of H2O, and then converting moles of H2O to grams. However, your final answer of 18.736363 grams seems to have too many decimal places.
Let's go through the calculations step by step:
1. Convert grams of N2O to moles:
You need to know the molar mass of N2O, which consists of two nitrogen atoms (N) with a molar mass of 14.01 g/mol each, and one oxygen atom (O) with a molar mass of 16.00 g/mol.
Molar mass of N2O: (2 * 14.01 g/mol) + 16.00 g/mol = 44.02 g/mol.
Now, divide the given mass of N2O (22.9 g) by the molar mass of N2O to get moles:
Moles of N2O = 22.9 g / 44.02 g/mol = 0.5208 mol (approx.)
2. Use the mole ratio to find moles of H2O:
From the balanced equation, we can see that for every 1 mole of N2O, 2 moles of H2O are produced.
So, moles of H2O = 0.5208 mol * 2 = 1.0416 mol (approx.)
3. Convert moles of H2O to grams:
The molar mass of water (H2O) is 18.02 g/mol (2 hydrogen atoms * 1.01 g/mol + 1 oxygen atom * 16.00 g/mol).
Now, multiply the moles of H2O by the molar mass of H2O:
Grams of H2O = 1.0416 mol * 18.02 g/mol = 18.77 g (approx.)
Therefore, the correct answer is approximately 18.77 grams of water produced.