If you need to make 200 tons of NH3, how much n2 and h2 would be needed if you want H2 to be the limiting reagent?
Equation: N2+H2 =NH3
Mass of H2 needed = 32274.44 kg = 35.58 ton


3 H2 + N2 → 2 NH3 1. If you have 3.22 moles of H2, how many moles of NH3 can you make? 2. If you have 1.19 moles of H2, how many moles of NH3 can you make? 3. If you have 15.22 moles of N2, how many moles of NH3 can you make? 4. How many moles of H2 do you need to react with 5.55 moles of N2? 5. How many moles of NH3 can be made...
If you have 5 mol H2 and 2 mol N2, what is the limiting reagent in the reaction below? 3 H2(g) + N2 (g) → 2 NH3 (9) A) H2 B) N2 C) NH3 D) Both reactants are limiting.
You are running the synthesis of ammonia reaction: 3 H2(g) + N2(g) --> 2 NH3(g) You add 15 g N2 and 9.0 g H2 to your reaction flask. Which of the following statements are true? (More than one option may be correct) H2 is the limiting reactant because the limiting reactant calculation showed that less NH3 can be produced from H2 as compared to the amount of NH3 possible from the N2. N2 is the limiting reactant because the limiting...
A. Given the following equation: N2 + 3 H2 → 2 NH3 How many grams of H2 would be required to completely react with 14 g of N2? B. Given the following equation: 2Na + Cl2 → 2NaCl How much table salt could be produced from 10.0 mol of chlorine gas and excess sodium? NOTE: All numbers located immediately after elemental symbols should be considered subscripts. C. The ground state configuration of a sodium atom is 1s22s22p63s1. So, the electron...
Nitrogen gas (N2) and hydrogen gas (H2) react to make ammonia gas (NH3) N2(g)+3H2(g)-->2NH3(g) you know tat this process gives a 55% yield for ammonia. Your job is to make 610g of ammonia. what mass of nitrogen do you need?
In the reaction of N2 and H2 to produce NH3, how many moles of H2 will produce 40.3 grams NH3 if sufficient N2 is present?
3H2(g)+N2(g)→2NH3(g) Part A: How many moles of NH3 can be produced from 12.0 mol of H2 and excess N2? = 8.00 mol I need answers for Part B-D Part B: How many grams of NH3 can be produced from 3.75 mol of N2 and excess H2? Part C: How many grams of H2 are needed to produce 11.79 g of NH3? Part D: How many molecules (not moles) of NH3 are produced from 5.00×10−4 g of H2?
Given the following equation: N2 (g) + 3 H2 (g) → 2 NH3 (g) How many grams of H2 are required if 44.2 grams of NH3 is produced? Jg H2
3H2(g)+N2(g)→2NH3(g) a. How many moles of NH3 can be produced from 13.5 mol of H2 and excess N2? b. How many grams of NH3 can be produced from 4.90 mol of N2 and excess H2. c. How many grams of H2 are needed to produce 12.74 g of NH3? d. How many molecules (not moles) of NH3 are produced from 1.05×10−4 g of H2?
Given a balance chemical equation, N2(g) + 3 H2(g) LaTeX: \longrightarrow⟶ 2 NH3(g) If a reaction mixture contains 2 moles of N2(g) and 7 moles of H2(g), which reactant is the limiting reactant and what is the mass (in grams) remaining of the reactant in excess?