hahaha ur soo dum u dont know lol go to dumbppl.com dumbo
If 5.0 moles of NH3 are produced 2.5 moles of N2 are used.
You can make a simple balance. There are (12.36 * 3) moles of H You have 2*H to form H2. So take the total from ammonia and divide by two to find the moles of H2 required.
0,044 moles of NH3 can be produced.
The formula reaction for NH3 when using N2 and H2 is: (N2)+3(H2) ---> 2(NH3) Now, first step is to find the moles of the H2 reactant. This is found via (grams of reactant)/(molar mass of reactant). There are 10 grams, and the molar mass of H2 is approximately 2.016. Therefore, the equation should look like: 10/2.016. This yields a value of ~4.9606 moles of H2. Now, you use the molar ratio from the reactant to the product to determine how many moles of product were yielded. According to the reaction, three moles of H2 are required to produces 2 moles of NH3. So, the mole ratio is 2/3. Multiply the number of moles of H2 with the molar ratio to determine the moles of NH3. 4.0606 * 2/3 = 3.3071 moles of NH3. Multiply the number of moles with the molar mass of NH3 (17.0306), and voila! 3.3071 * 17.0306 = 56.3216 grams. Now, if your teacher is feeling like a stickler about significant figures, than that value should be rounded to 56 grams of NH3.
How many moles of NH3 are produced when 1.2 mol of nitrogen reacts with hydrogen?
N2 + 3H2 -> 2NH3 If you have moles produced you can do it this way. 22.5 moles NH3 (3 moles H2/2 moles NH3) = 33.8 moles H2 needed -----------------------------------
This is based on calculations too. It contains 18 hydrogen moles.
If 5.0 moles of NH3 are produced 2.5 moles of N2 are used.
N2 + 3H2 -> 2NH3 The stoichiometric equation (or balanced equation) for the formation of ammonia from this we can read off the mole ratio between hydrogen and ammonia; 3M H2 needed to produce 2M NH3 times each by 9 (so the ratio remains the same and 18M NH3 is formed) 27M H2 needed to produce 18M NH3
170 kg = 170,000g NH3 = 170,000g / 17.0g/molNH3 = [10,000 molNH3] * 3moleH2 / 2moleNH3= 15,000 mole H2 needed to produce 170 kg NH3
You can make a simple balance. There are (12.36 * 3) moles of H You have 2*H to form H2. So take the total from ammonia and divide by two to find the moles of H2 required.
0,044 moles of NH3 can be produced.
The formula reaction for NH3 when using N2 and H2 is: (N2)+3(H2) ---> 2(NH3) Now, first step is to find the moles of the H2 reactant. This is found via (grams of reactant)/(molar mass of reactant). There are 10 grams, and the molar mass of H2 is approximately 2.016. Therefore, the equation should look like: 10/2.016. This yields a value of ~4.9606 moles of H2. Now, you use the molar ratio from the reactant to the product to determine how many moles of product were yielded. According to the reaction, three moles of H2 are required to produces 2 moles of NH3. So, the mole ratio is 2/3. Multiply the number of moles of H2 with the molar ratio to determine the moles of NH3. 4.0606 * 2/3 = 3.3071 moles of NH3. Multiply the number of moles with the molar mass of NH3 (17.0306), and voila! 3.3071 * 17.0306 = 56.3216 grams. Now, if your teacher is feeling like a stickler about significant figures, than that value should be rounded to 56 grams of NH3.
Balanced equation. N2 + 3H2 --> 2NH3 1.4 moles H2 (2 moles NH3/3 moles H2) = 0.93 moles NH3 produced =======================
How many moles of NH3 are produced when 1.2 mol of nitrogen reacts with hydrogen?
Using the molar mass of nh3, we find that we have 2.5 moles of nh3. Since 3 moles of h2o are produced per 2 moles of nh3, we see that we will produce 3.75 moles of h2o. This is equivalent to around 3.79 g.
How many moles of NH3 are produced when 1.2 mol of nitrogen reacts with hydrogen?