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mel-nik [20]
3 years ago
8

Ammonia forms when hydrogen gas reacts with nitrogen gas according to the equation below. If equal moles of nitrogen and hydroge

n are combined, the maximum number of moles of ammonia that could be formed will be equal to:two thirds the number of moles of hydrogenthe number of moles of hydrogenthe number of moles of nitrogentwice the number of moles of nitrogen
Chemistry
2 answers:
Aleksandr-060686 [28]3 years ago
6 0

Answer:

Two thirds the number of moles of hydrogen

Explanation:

The balanced reaction is

3H₂ + N₂ → 2NH₃

So 1 mol of nitrogen gas reacts completely with 3 moles of hydrogen gas, to produce 2 moles of ammonia.

If equal moles of nitrogen and hydrogen are combined, <em>then hydrogen would be the limiting reactant</em>. Let's say we have 3 moles of each reactant, one mol of N₂ reacts with the 3 moles of H₂ and produces 2 moles of NH₃, and 2 moles of N₂ would remain. So the answer is<em> two thirds the number of moles of hydrogen.</em>

Kamila [148]3 years ago
3 0

Answer:

The number of moles NH3 produced is two thirds of moles of hydrogen.

Explanation:

Step 1: Data given

Number of moles H2 = Number of moles N2

Step 2: The balanced equation

3H2 + N2 → 2NH3

Step 3: Calculate mol NH3 produced

For 1 mol N2 consumed, we need 3 moles of H2, to produce 2 mol of NH3

H2 is the limiting reactant. This will be completely consumed.

N2 is in excess. There will be consumed 1/3 of moles of H2

The mole ratio H2:NH3 = 3:2

The number of moles NH3 produced is two thirds of moles hydrogen.

The number of moles N2 is one third of moles hydrogen.

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Consider a pot of water at 100 C. If it took 1,048,815 J of energy to vaporize the water and heat it to 135 C, how many grams of
jeka57 [31]

Answer:

There was 450.068g of water in the pot.

Explanation:

Latent heat of vaporisation = 2260 kJ/kg = 2260 J/g = L

Specific Heat of Steam = 2.010 kJ/kg C = 2.010 J/g = s

Let m = x g be the weight of water in the pot.

Energy required to vaporise water = mL = 2260x

Energy required to raise the temperature of water from 100 C to 135 C = msΔT = 70.35x

Total energy required = 2260x+x\times2.010\times(135-100)=2260x+70.35x=2330.35x

2330.35x=1048815\\x=450.068g

Hence, there was 450.068g of water in the pot.

8 0
3 years ago
How many grams are in 2.45E24 formula units of Fp3BZ2? The molar mass of Fp3Bz2. is 97.05<br> g/mol.
dlinn [17]

Answer:

394.99g

Explanation:

The number of moles of a substance can be calculated by dividing the number of atoms of such substance by Avagadro's number (6.02 × 10^23)

n = nA ÷ 6.02 × 10^23

The number of atoms of Fp3BZ2 in this question is 2.45E24 formula units i.e. 2.45 × 10^24

n = 2.45 × 10^24 ÷ 6.02 × 10^23

n = 2.45/6.02 × 10^(24-23)

n = 0.407 × 10¹

n = 4.07moles

Using mole = mass/molar mass

Where; molar mass of Fp3Bz2. is 97.05

g/mol.

mass = molar mass × mole

mass = 97.05 × 4.07

mass = 394.99g

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Answer: 14 :12 water molecules,  

Explanation: 17: 6 molecules

8 0
3 years ago
How many moles of NH3 can be produced by the reaction of 2.00 g of N2 with 3.00 g H2?
yulyashka [42]
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8 0
2 years ago
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