Question

If 0.3 moles of N2 were reacted with 0.6 moles of H2, what mass of NH3...

If 0.3 moles of N2 were reacted with 0.6 moles of H2, what mass of NH3 could form? N2 +3H2 -------> 2 NH3

a) 0.6 g b) 1.2 g c) 6.8 g d) 10.2 g

I know how to do the math portion, I'm just confused on how to determine the limiting and excess reagent. a) 0.6 g b) 1.2 g c) 6.8 g d) 10.2 g

Homework Answers

Answer #1

Balanced equation is

N2 +3H2 -------> 2 NH3

Fromm the balanced equation we can say that

1 mole of N2 requires 3 mole of H2 so

0.3 mole of N2 will require

= 0.3 mole of N2 *( 3 mole of H2 / 1 mole of N2)

= 0.9 mole of H2 will be required

But we have 0.6 mole of H2 which is in short so H2 is limiting reactant

From the balanced equation we can say that

3 mole of H2 produces 2 mole of NH3 so

0.6 mole of H2 will produce = 0.4 mole of NH3 is formed

mass of 1mole of NH3 = 17.0 g

Therefore, the mass of 0.4 mole of NH3 = 6.8 g

Therefore, option C is correct

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
hydrogen gas, H2, reacts with nitrogen gas,N2, to form ammonia gas , NH3 according to the...
hydrogen gas, H2, reacts with nitrogen gas,N2, to form ammonia gas , NH3 according to the equation... 3H2+N2 --->2NH3 1.how many grams of NH3 can be produced from 3.42 mol of N2 and excess H2 2. how many grams of H2 are needed to produce 14.93 g of NH3 ? 3. How many molecules (not moles) of NH3 are produced from 6.04*10^-4 g of H2 ?
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the...
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation 3H2(g)+N2(g)→2NH3(g) 1. How many molecules (not moles) of NH3 are produced from 5.25×10−4 g of H2 ?
N2(g) + 3H2(g) → 2NH3(g) 5.00 g N2 is reacted with 5.00 g H2 How many...
N2(g) + 3H2(g) → 2NH3(g) 5.00 g N2 is reacted with 5.00 g H2 How many mol NH3 can be produced in this reaction?
How many moles of NH3 are produced when 1.7 moles H2 reacts? How many moles of...
How many moles of NH3 are produced when 1.7 moles H2 reacts? How many moles of N2 reacted if 0.65 mole NH3 is produced? How many moles of SO3 are in 17.51 g of SO3? How many moles of Ca(NO3)2 are in 4.502 g of Ca(NO3)2? How many moles of C are in each of the following quantities? 88.1 g Sn(C2O4)2
Consider the following balanced reaction between hydrogen and nitrogen to form ammonia: 3H2(g) + N2(g)→2NH3(g) How...
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 24.0 mol of H2 and excess N2? Express the number of moles to three significant figures.
Ammonia is produced using the Haber process: 3 H2 + N2 → 2 NH3 What mass...
Ammonia is produced using the Haber process: 3 H2 + N2 → 2 NH3 What mass of NH3 could be produced if 12.5 g H2 reacts with excess nitrogen? 4.13g, 105g, 142g, 70.4g
Ammonia, NH3(g), can be prepared by the following reaction: 2NO(g) + 5 H2(g)----> NH3(g) + 2...
Ammonia, NH3(g), can be prepared by the following reaction: 2NO(g) + 5 H2(g)----> NH3(g) + 2 H2O(g) What is the limiting reagent of the reaction and the theoretical yield of NH3(g) in grams if 26.5 g NO(g) and 1.77 g of H2(g) were added to a flask? A, NO(g) and 7.51 g NH2(g) B. NO(g) and 15.0 g NH3(g) C. H2(g) and 15.0 g NH3(g) D. H2(g) and 5.96 g NH3(g) *Please explain how you got your answer. Much appreciated...
N2 + 3H2 ??2NH3 complete the problems below if the reaction above has starting of 28.0...
N2 + 3H2 ??2NH3 complete the problems below if the reaction above has starting of 28.0 g of N2 and 25.0 g of H2? (a) which is the limiting reactant? (b) how many grams of ammonia can be produced from these starting amounts? (C) in the laboratory exercise a students products measures 28.0 g of ammonia- what is the % yield of the lab exercise? (d) how many grams of the excess reactant are left over? please step by step...
So I did a titration lab where were reacted various amounts of Mg with 10mL of...
So I did a titration lab where were reacted various amounts of Mg with 10mL of HCL and then neutralized the raction with NaOH. I have my table of values for Mass of Mg (g), Initial Volume NaOH (mL), Final Volume NaOH (mL), End Point Volume (mL), Limiting Reagent (Mg or HCL). There is a Titration table I need to fill in that asks for Moles of Mg (mol), Moles of NaOH (mol) and Moles of H+ reacting with Mg...
Consider the reaction for the Haber Process: 3H2 (g) + N2 (g) <--> 2NH3(g) A mixture...
Consider the reaction for the Haber Process: 3H2 (g) + N2 (g) <--> 2NH3(g) A mixture of 1.0 mol each of N2, H2, and NH3 are placed into a 1.0 L flask and allowed to come to equilibrium at 500.0 C. Kp at this temperature is 1.45 x 10-5 atm-2. A.) What is the value of Kc at this temperature? irst find the relationship between Kc and Kp in terms of RT. Then substitute T = 773K and R =...