Question

Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation: N2(g) + 3H2(g) ? 2NH3(g) 1. What is the maximum mass of ammonia that can be produced from a mixture of 870.0 g of N2 and 430.0 g of H2? 1740 g 2. Which element would be left partially unreacted? (enter nitrogen or hydrogen) nitrogen 3. What mass of the starting material would remain unreacted? 1367.14 g Look at how many grams of ammonia the N2 would produce and how many grams of ammonia the H2 would produce. Watch the mole ratios! Whichever produces the smallest amount of ammonia is the limiting reactant. HINT: After you have found which starting material was used up completely, you know that some of the other starting material is still unreacted. Subtract the reacted material (which you must calculate) from the original amount you had in the beginning, thus finding how much remains unreacted.

          Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation:
N2(g) + 3H2(g) ? 2NH3(g)
1. What is the maximum mass of ammonia that can be produced from a mixture of 870.0 g of N2 and 430.0 g of H2? 1740 g
2. Which element would be left partially unreacted? (enter nitrogen or hydrogen) nitrogen
3. What mass of the starting material would remain unreacted? 1367.14 g
Look at how many grams of ammonia the N2 would produce and how many grams of ammonia the H2 would produce.
Watch the mole ratios!
Whichever produces the smallest amount of ammonia is the limiting reactant.
HINT: After you have found which starting material was used up completely, you know that some of the other starting material is still unreacted. Subtract the reacted material (which you must calculate) from the original amount you had in the beginning, thus finding how much remains unreacted.

Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation:
N2(g) + 3H2(g) ? 2NH3(g)
1. What is the maximum mass of ammonia that can be produced from a mixture of 870.0 g of N2 and 430.0 g of H2? 1740 g
2. Which element would be left partially unreacted? (enter nitrogen or hydrogen) nitrogen
3. What mass of the starting material would remain unreacted? 1367.14 g
Look at how many grams of ammonia the N2 would produce and how many grams of ammonia the H2 would produce.
Watch the mole ratios!
Whichever produces the smallest amount of ammonia is the limiting reactant.
HINT: After you have found which starting material was used up completely, you know that some of the other starting material is still unreacted. Subtract the reacted material (which you must calculate) from the original amount you had in the beginning, thus finding how much remains unreacted.

Added by Blanca T.

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