2NH3 ---------------> N2 + 3H2
1.Explain what this equation is telling you.
2.Identify which compounds are the reactants and which are the products.
3. Is the equation balanced as written? How many nitrogen atoms and how many hydrogen atoms are represented on each side of the equation?
2NH3 ---------------> N2 + 3H2 1.Explain what this equation is telling you. 2.Identify which compounds are...
Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N2(g) + 3H2(g) → 2NH3(g) Calculate the mass of ammonia produced when 32.0 g of nitrogen react with 13.5 g of hydrogen. ___________NH3 Which is the excess reactant and how much of it will be left over when the reaction is complete? hydrogen or nitrogen ________ g
2. Fill in the table concerning the following redox reaction: N2 + 3H2 → 2NH3 What is the oxidation state of nitrogen in NZ ? What is the oxidation state of hydrogen in H2 ? What is the oxidation state of nitrogen in NH3? What is the oxidation state of hydrogen in NH3? What is being oxidized? What is being reduced? How do you know? What is the oxidizing agent? Reducing agent?
Nitrogen and hydrogen can react to form ammonia. N2(g)+3H2(g)→2NH3(g) 1. Choose ratios showing the relationships between moles of each of the reactants and products in the reaction. Multiple choice, which one? A. 2 mol N2 : 2 mol H2 : 3 mol NH3 B.1 mol N2 : 1/3 mol H2 : 1/2 mol NH3 C. 1 mol N2 : 1 mol H2 : 1 mol NH3 D. 1 mol N2 : 3 mol H2 : 2 mol NH3 2. How...
N2 + 3H2 --> 2NH3 Given the balanced equation above, how many grams of NH3 (theoretical yield) can be produced from the reaction of 28.8 g of N2 and 25 g of H2?
Consider the following balanced reaction between hydrogen and nitrogen to form ammonia: 3H2(g) + N2(g)→2NH3(g) How many moles of NH3 can be produced from 18.0 mol of H2 and excess N2? Express the number of moles to three significant figures
QUESTION 17 How would you read the following chemical equation? N2(g) + 3H2(g) + 2NH3(g) Note: Some chemist might say diatomic nitrogen and diatomic hydrogen gas, to make that really clear. That would be a second correct way fo asking these questions 2 moles of nitrogen gas and 2 moles of hydrogen gas react to form 2 moles of nitrogen trihydride gas. . 1 mole of nitrogen gas and 3 moles of hydrogen gas react to form 2 moles of...
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?
9 please. Nitrogen gas reacts with hydrogen gas to produce ammonia. N2(g) + 3H2(g) — 2NH3(g) a. If you have 3.64 g of H, how many grams of NH3 can be produced? b. How many grams of H, are needed to react with 2.80 g of N? c. How many grams of NH; can be produced from 12.0 g of H? DO
What happens when you remove a catalyst from Haber process? N2 (g)+ 3H2 (g) 2NH3(g) if the process has deltaG rxn= -4000 kJ/mol Kp= 8200 A) How would the values of deltaG and Kp change when you remove a catalyst? (decrease, increase, stay the same) B) If catalyst is removed, is reaction going to favour reactants or products?
1. For the reaction N2(g) + 3H2(g) → 2NH3(g), if 2.25 L H2 reacts, what volume of NH3 forms if both are at the same temperature and pressure? 2.Given the balanced reaction below: 2 C6H6(g) + 15 O2(g) ⟶ 12 CO2(g) + 6 H2O(g) If 2.45 liters of benzene are consumed in this reaction, how many liters of water can be formed? Benzene is C6H6