Ammonia chemically reacts with oxygen gas to produce nitric oxide and water .
What mass of ammonia is consumed by the reaction of 4.5g of oxygen gas?
Round your answer to significant digits.
Why did the oxygen gas go on a date with the ammonia? Because it wanted to make some NOx-ious jokes!
Now, to find the mass of ammonia consumed, we need to set up a balanced chemical equation and find the mole ratio.
The balanced equation is: 4 NH3 + 5 O2 → 4 NO + 6 H2O
The molar mass of O2 is approximately 32 g/mol.
Now, we can use the molar ratio to find the amount of ammonia consumed. According to the balanced equation, for every 5 moles of O2, 4 moles of NH3 are consumed.
So, let's set up the calculation:
(4.5 g O2) × (1 mol O2 / 32 g O2) × (4 mol NH3 / 5 mol O2) × (17 g NH3 / 1 mol NH3) = 12.09 g NH3
Therefore, approximately 12.09 grams of ammonia are consumed by the reaction.
Hope that helped, and remember to always keep your chemistry jokes well-balanced!
To determine the mass of ammonia consumed, we need to use the balanced chemical equation for the reaction:
4 NH3 + 5 O2 -> 4 NO + 6 H2O
Based on the equation, we can see that 4 moles of ammonia react with 5 moles of oxygen gas to produce 4 moles of nitric oxide and 6 moles of water.
To find the mass of ammonia consumed, we need to use the molar mass of ammonia and the given mass of oxygen gas.
The molar mass of ammonia (NH3) is:
1 nitrogen (N) * 14.01 g/mol + 3 hydrogen (H) * 1.01 g/mol = 17.04 g/mol
To find the moles of oxygen gas, we can use its molar mass:
O2 has a molar mass of 2 oxygen (O) * 16.00 g/mol = 32.00 g/mol
Now, let's set up the proportion:
5 moles of O2 = 32.00 g
4.5 g of O2 = x moles
Using the proportion:
x = (4.5 g * 5 moles) / 32.00 g
x = 0.7031 moles
Since 4 moles of NH3 react with 5 moles of O2, we can set up another proportion:
4 moles of NH3 = 0.7031 moles
1 mole of NH3 = y moles
Using the proportion:
y = (0.7031 moles * 1 mole) / 4 moles
y = 0.1758 moles
Finally, we can calculate the mass of ammonia consumed:
Mass of ammonia consumed = moles of ammonia * molar mass of ammonia
Mass of ammonia consumed = 0.1758 moles * 17.04 g/mol
Mass of ammonia consumed = 2.992 g
Therefore, the mass of ammonia consumed by the reaction of 4.5 g of oxygen gas is approximately 3.0 g (rounded to significant digits).
To find the mass of ammonia consumed by the reaction of 4.5g of oxygen gas, we need to determine the balanced chemical equation for the reaction. The balanced chemical equation for the reaction between ammonia (NH3) and oxygen gas (O2) to produce nitric oxide (NO) and water (H2O) is:
4 NH3 + 5 O2 -> 4 NO + 6 H2O
From the balanced chemical equation, we can see that the ratio of ammonia to oxygen gas is 4:5. This means that for every 4 moles of ammonia consumed, we need 5 moles of oxygen gas.
Now we need to convert the mass of oxygen gas (4.5g) into moles. To do this, we'll use the molar mass of oxygen, which is approximately 32g/mol.
Number of moles of oxygen gas = mass / molar mass
Number of moles of oxygen gas = 4.5g / 32g/mol
Number of moles of oxygen gas = 0.14 mol (rounded to two decimal places)
Using the ratio from the balanced equation, we can determine the moles of ammonia consumed by the reaction:
Number of moles of ammonia = (number of moles of oxygen gas) x (4 moles of ammonia / 5 moles of oxygen gas)
Number of moles of ammonia = 0.14 mol x (4 mol / 5 mol)
Number of moles of ammonia = 0.112 mol (rounded to three decimal places)
Finally, to find the mass of ammonia consumed, we'll use the molar mass of ammonia, which is approximately 17g/mol.
Mass of ammonia consumed = number of moles of ammonia x molar mass of ammonia
Mass of ammonia consumed = 0.112 mol x 17g/mol
Mass of ammonia consumed = 1.90g (rounded to two decimal places)
Therefore, the mass of ammonia consumed by the reaction of 4.5g of oxygen gas is approximately 1.90g.
4NH3+5O2-->4NO+6H2O
4.5g*(1 mol/32g)*(4 mol/5 mol)*(16.03g/1 mol)
1.8g Ammonia