According to the following chemical equation:

N2 + 3H2 → 2NH3

How many grams of hydrogen are needed to completely react with 28.0 grams of nitrogen?

Well, let's do some chemistry math, shall we? According to the equation, we need 3 moles of hydrogen for every 1 mole of nitrogen to react completely.

To find the number of moles of nitrogen, we divide the given mass by its molar mass. The molar mass of nitrogen (N2) is approximately 28 grams/mol, so 28 grams of nitrogen is equal to 1 mole.

Now, let's calculate the moles of hydrogen required. Since the ratio is 3:1, we multiply the moles of nitrogen by 3. Thus, we need 3 moles of hydrogen.

To find the grams of hydrogen, we multiply the number of moles by its molar mass. The molar mass of hydrogen (H2) is roughly 2 grams/mol, so 3 moles of hydrogen is equal to 6 grams.

Therefore, to completely react with 28.0 grams of nitrogen, you would need 6 grams of hydrogen.

To find out how many grams of hydrogen are needed to completely react with 28.0 grams of nitrogen, we need to use the stoichiometry of the chemical equation.

The balanced equation tells us that for every 1 mole of nitrogen (N2), 3 moles of hydrogen (H2) are needed to react.

To find the number of moles of nitrogen in 28.0 grams, we use the molar mass of nitrogen, which is 14.01 grams/mole.

28.0 grams of nitrogen / 14.01 grams/mole = 1.999 moles of nitrogen (which we'll round to 2 moles)

According to the stoichiometry, 2 moles of nitrogen react with 3 moles of hydrogen.

So, we can use the ratio of moles to find the number of moles of hydrogen needed:

2 moles of nitrogen : 3 moles of hydrogen

2 moles of nitrogen * (3 moles of hydrogen / 1 mole of nitrogen) = 6 moles of hydrogen

Now we can find the number of grams of hydrogen using the molar mass of hydrogen, which is 2.02 grams/mole:

6 moles of hydrogen * 2.02 grams/mole = 12.12 grams of hydrogen (which we'll round to 12.1 grams)

Therefore, 12.1 grams of hydrogen are needed to completely react with 28.0 grams of nitrogen.

To determine the mass of hydrogen required to react with a given mass of nitrogen, you need to use stoichiometry, which is the study of the quantitative relationships between reactants and products in a chemical reaction.

Step 1: Determine the molar mass of the substances involved.
- Nitrogen (N2) has a molar mass of 28.02 g/mol. (since nitrogen is diatomic)
- Hydrogen (H2) has a molar mass of 2.02 g/mol.

Step 2: Convert the given mass of nitrogen to moles.
- Divide the given mass of nitrogen (28.0 g) by its molar mass (28.02 g/mol).
- 28.0 g of nitrogen is equal to 1 mole of nitrogen.

Step 3: Use the balanced chemical equation to establish the mole ratio between nitrogen and hydrogen.
- The balanced equation states that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia (NH3).
- This means that for every 1 mole of nitrogen, 3 moles of hydrogen are needed.

Step 4: Convert the moles of nitrogen to moles of hydrogen using the mole ratio.
- Since 1 mole of nitrogen requires 3 moles of hydrogen, we can multiply the moles of nitrogen by the mole ratio.
- Multiply 1 mole of nitrogen by 3 moles of hydrogen/1 mole of nitrogen.
- This gives us 3 moles of hydrogen.

Step 5: Convert the moles of hydrogen to grams of hydrogen.
- Multiply the moles of hydrogen (3) by its molar mass (2.02 g/mol).
- This will give us the mass of hydrogen required.
- 3 moles of hydrogen is equal to 6.06 grams of hydrogen.

Therefore, 6.06 grams of hydrogen are needed to completely react with 28.0 grams of nitrogen.

According to the equation, 1 mol N2 reacts with 3 mols H2.

mols N2 = g/molar mass = 28/28 = 1
That will take 3 mols H2.
grams H2 = mols H2 x molar mass H2 = ?