How many grams of N2 are produced when 125g of NH3 reacts by the following? 4NH3+6NO--->5N2 +6H20
I know the answer but I do not know how to do the problem. The answer in the book is 257g
But what do I do? I am not even sure where to start? Thanks
Well, my friend, let me throw some comedic clarity into this chemistry conundrum for you!
To solve this problem, we need to use stoichiometry, which is just a fancy way of saying "balancing the equation." Think of it as balancing on a unicycle while juggling fireballs – it requires some skill!
Now, let's break it down step by step:
1. Determine the molar mass of NH3 (ammonia) and N2 (nitrogen gas). NH3 has a molar mass of roughly 17 g/mol, while N2 has a molar mass of about 28 g/mol.
2. Calculate the number of moles of NH3 by dividing the given mass by its molar mass. So, 125 g NH3 / 17 g/mol = approximately 7.35 moles of NH3.
3. Use the stoichiometric coefficients in the balanced equation (4:5 ratio between NH3 and N2) to determine the number of moles of N2 produced. Since the ratio is 4:5, we'll use a little algebra and find:
7.35 moles NH3 x (5 moles N2 / 4 moles NH3) = roughly 9.18 moles N2.
4. Finally, convert moles of N2 to grams. Multiply the number of moles by the molar mass of N2, which is 28 g/mol:
9.18 moles N2 x 28 g/mol = approximately 257 grams of N2!
So, according to the mysterious book, the answer is indeed 257 grams of N2. Voila!
Keep up the good work, my friend! And remember, solving chemistry problems is a lot like juggling – sometimes you drop the ball, but laughter makes everything better!
To solve this problem, you can use stoichiometry. Stoichiometry is a method used to relate the quantities of substances involved in a chemical reaction. Here's how you can approach it step-by-step:
Step 1: Write and balance the chemical equation:
4NH3 + 6NO → 5N2 + 6H2O
Step 2: Determine the molar mass of NH3 and N2:
Molar mass of NH3 = 14.01 g/mol + 3(1.01 g/mol) = 17.03 g/mol
Molar mass of N2 = 2(14.01 g/mol) = 28.02 g/mol
Step 3: Convert the given mass of NH3 to moles:
125 g NH3 x (1 mol NH3/17.03 g NH3) = 7.34 mol NH3
Step 4: Use the balanced equation to calculate the moles of N2 produced:
From the balanced equation, we can see that 4 moles of NH3 produce 5 moles of N2.
Therefore, we can use this ratio to calculate the moles of N2:
7.34 mol NH3 x (5 mol N2/4 mol NH3) = 9.18 mol N2
Step 5: Convert the moles of N2 to grams:
9.18 mol N2 x (28.02 g N2/1 mol N2) = 257 g N2
So, the answer is indeed 257 grams of N2 produced when 125 grams of NH3 reacts.
To solve this problem, you can use stoichiometry, which is a method of relating the quantities of reactants and products in a chemical reaction.
Here's a step-by-step approach:
1. Write down the balanced chemical equation:
4NH3 + 6NO -> 5N2 + 6H2O
2. Determine the molar mass of NH3 (ammonia) and N2 (nitrogen gas).
The molar mass of NH3 is calculated as:
(1 x atomic mass of N) + (3 x atomic mass of H) = 14.01 g/mol + 3(1.01 g/mol) = 17.03 g/mol
The molar mass of N2 is calculated as:
2 x atomic mass of N = 2(14.01 g/mol) = 28.02 g/mol
3. Convert the given mass of NH3 to moles.
Use the formula:
Moles = Mass / Molar mass
Moles of NH3 = 125 g / 17.03 g/mol ≈ 7.33 mol
4. Use the stoichiometric coefficients from the balanced equation to determine the moles of N2 produced.
From the balanced equation, the ratio of NH3 to N2 is 4:5.
Therefore, 7.33 mol of NH3 would theoretically produce:
(7.33 mol NH3) x (5 mol N2 / 4 mol NH3) = 9.16 mol N2
5. Convert moles of N2 to grams.
Use the formula:
Mass = Moles x Molar mass
Mass of N2 = 9.16 mol x 28.02 g/mol ≈ 256.93 g
So, the calculated mass of N2 produced is approximately 256.93 g, which matches the answer given in the book of 257 g.
257 is right. Here is a worked example that will work all of your stoichiometry problems.
http://www.jiskha.com/science/chemistry/stoichiometry.html