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1. Ammonia is produced by the reaction of hydrogen and nitrogen.
N2(g)+3H2(g)→2NH3(g)ammonia

How many moles of N2 reacted if 0.65mole NH3 is produced?

How many moles of NH3 are produced when 1.2moles H2 reacts?

2.In the acetylene torch, acetylene gas (C2H2) burns in oxygen to produce carbon dioxide and water.
2C2H2(g)+5O2(g)→4CO2(g)+2H2O(g)

How many moles of O2 are needed to react with 2.10moles C2H2?

How many moles of CO2 are produced when 4.0moles C2H2 reacts?

How many moles of C2H2 are required to produce 0.50mole H2O?

How many moles of CO2 are produced from 0.100mole O2?

I thought I did #1 last night. All of the others are off shoots of that. Remember that any component in an equation (in mols) can be converted to any other component in the reaction by using the coefficients in the balanced equation.

yes

1. To find the number of moles of N2 reacted if 0.65 mole NH3 is produced, we can use the mole ratio from the balanced chemical equation:

From the equation: N2(g) + 3H2(g) → 2NH3(g)
The mole ratio between N2 and NH3 is 1:2.

So, if 2 moles of NH3 are produced, then 1 mole of N2 reacted. Therefore, if 0.65 moles of NH3 are produced:

0.65 moles NH3 * (1 mole N2 / 2 moles NH3) = 0.325 moles N2

Therefore, 0.325 moles of N2 reacted if 0.65 moles of NH3 are produced.

2. To find the number of moles of NH3 produced when 1.2 moles of H2 reacts, we can again use the mole ratio from the balanced chemical equation:

From the equation: N2(g) + 3H2(g) → 2NH3(g)
The mole ratio between H2 and NH3 is 3:2.

So, if 3 moles of H2 react, then 2 moles of NH3 are produced. Therefore, if 1.2 moles of H2 react:

1.2 moles H2 * (2 moles NH3 / 3 moles H2) = 0.8 moles NH3

Therefore, 0.8 moles of NH3 are produced when 1.2 moles of H2 reacts.

3. To find the number of moles of O2 needed to react with 2.10 moles of C2H2, we can use the mole ratio from the balanced chemical equation:

From the equation: 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g)
The mole ratio between C2H2 and O2 is 2:5.

So, if 2 moles of C2H2 react, then 5 moles of O2 are needed. Therefore, if 2.10 moles of C2H2 react:

2.10 moles C2H2 * (5 moles O2 / 2 moles C2H2) = 5.25 moles O2

Therefore, 5.25 moles of O2 are needed to react with 2.10 moles of C2H2.

4. To find the number of moles of CO2 produced when 4.0 moles of C2H2 reacts, we can use the mole ratio from the balanced chemical equation:

From the equation: 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g)
The mole ratio between C2H2 and CO2 is 2:4.

So, if 2 moles of C2H2 react, then 4 moles of CO2 are produced. Therefore, if 4.0 moles of C2H2 react:

4.0 moles C2H2 * (4 moles CO2 / 2 moles C2H2) = 8.0 moles CO2

Therefore, 8.0 moles of CO2 are produced when 4.0 moles of C2H2 reacts.

5. To find the number of moles of C2H2 required to produce 0.50 mole of H2O, we can again use the mole ratio from the balanced chemical equation:

From the equation: 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g)
The mole ratio between C2H2 and H2O is 2:2.

So, if 2 moles of C2H2 react, then 2 moles of H2O are produced. Therefore, if 0.50 mole of H2O is produced:

0.50 moles H2O * (2 moles C2H2 / 2 moles H2O) = 0.50 moles C2H2

Therefore, 0.50 moles of C2H2 are required to produce 0.50 mole of H2O.

6. To find the number of moles of CO2 produced from 0.100 mole of O2, we can use the mole ratio from the balanced chemical equation:

From the equation: 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g)
The mole ratio between O2 and CO2 is 5:4.

So, if 5 moles of O2 react, then 4 moles of CO2 are produced.
Therefore, if 0.100 mole of O2 reacts:

0.100 moles O2 * (4 moles CO2 / 5 moles O2) = 0.080 mole CO2

Therefore, 0.080 mole of CO2 is produced from 0.100 mole of O2.

To find the number of moles of a reactant or product in a chemical equation, you need to use the coefficients of the balanced equation. The coefficients represent the mole ratios between the reactants and products.

For the given questions, let's use the balanced equations provided to determine the number of moles involved in each reaction.

1. Ammonia Production:
The balanced equation is: N2(g) + 3H2(g) → 2NH3(g)

a) How many moles of N2 reacted if 0.65 mole NH3 is produced?
From the balanced equation, the mole ratio between N2 and NH3 is 1:2.
Therefore, if 2 moles of NH3 are produced, it means 1 mole of N2 reacted.
So, to find the moles of N2, you can use the following equation:

(0.65 mole NH3) * (1 mole N2 / 2 moles NH3) = 0.325 moles N2

Therefore, 0.325 moles of N2 reacted.

b) How many moles of NH3 are produced when 1.2 moles H2 react?
From the balanced equation, the mole ratio between H2 and NH3 is 3:2.
So, using the equation:

(1.2 moles H2) * (2 moles NH3 / 3 moles H2) = 0.8 moles NH3

Therefore, 0.8 moles of NH3 are produced.

2. Acetylene Torch Reaction:
The balanced equation is: 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g)

a) How many moles of O2 are needed to react with 2.10 moles C2H2?
From the balanced equation, the mole ratio between C2H2 and O2 is 2:5.
So, using the equation:

(2.10 moles C2H2) * (5 moles O2 / 2 moles C2H2) = 5.25 moles O2

Therefore, 5.25 moles of O2 are needed.

b) How many moles of CO2 are produced when 4.0 moles C2H2 react?
From the balanced equation, the mole ratio between C2H2 and CO2 is 2:4 (or simplified, 1:2).
So, using the equation:

(4.0 moles C2H2) * (4 moles CO2 / 2 moles C2H2) = 8.0 moles CO2

Therefore, 8.0 moles of CO2 are produced.

c) How many moles of C2H2 are required to produce 0.50 mole H2O?
From the balanced equation, the mole ratio between C2H2 and H2O is 2:1.
So, using the equation:

(0.50 mole H2O) * (2 moles C2H2 / 1 mole H2O) = 1.0 mole C2H2

Therefore, 1.0 mole of C2H2 is required.

d) How many moles of CO2 are produced from 0.100 mole O2?
From the balanced equation, the mole ratio between O2 and CO2 is 5:4.
So, using the equation:

(0.100 mole O2) * (4 moles CO2 / 5 moles O2) = 0.080 mole CO2

Therefore, 0.080 mole of CO2 is produced.

Remember, to find the number of moles, you need to use the balanced equation and the mole ratios between the reactants and products.