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Please help ill give brainliest
Calculate the volume of ammonia produced at STP from the complete reaction of 10.00g of nitrogen with excess hydrogen. Put one digit per box.

Please help ill give brainliest Calculate the volume of ammonia produced at STP from the complete reaction of 1000g of nitrogen with excess hydrogen Put one dig class=

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Intriguing456

Answer:

16.00 L

Explanation:

We are given the chemical reaction:

[tex]\rm N_2 + 3 \: H_2 \to 2\: NH_3[/tex]

and the amount of nitrogen gas reacted:

[tex]m_{\text{N2}} = 10.00\text{ g}[/tex]

We are being asked to calculate the volume of ammonia (the product) that will be formed from the given amount of nitrogen.

First, we can convert the mass of nitrogen to moles, then use the reaction's stoichiometric ratios to solve for how many moles of ammonia will be produced.

[tex]n = \dfrac{10.00\text{ g N}_2}{1}\times\dfrac{1 \text{ mole N}_2}{2(14.01)\text{ g N}_2} \times \dfrac{2\text{ mole NH}_3}{1\text{ mole N}_2}[/tex]

[tex]n \approx 0.71378 \text{ mole NH}_3[/tex]

Then, we can plug this amount of ammonia gas into the ideal gas law to solve for the amount of volume it will occupy at standard temperature and pressure (STP):

[tex]PV = nRT[/tex]

where:

  • [tex]P[/tex] = pressure
  • [tex]V[/tex] = volume
  • [tex]n[/tex] = moles of gas
  • [tex]R[/tex] = universal gas constant
  • [tex]T[/tex] = temperature in Kelvin

According to the College Board, STP is defined as:

[tex]P = 1\text{ atm}[/tex],   [tex]T = 273.15\text{ K}[/tex]

and the gas constant is:

[tex]R = 0.08206\ \dfrac{\text{ L}\cdot\text{atm}}{\text{mole} \cdot \text{K}}[/tex]

Solving the ideal gas law for volume gives us:

[tex]V = \dfrac{nRT}{P}[/tex]

Now, we can plug in the known values to solve for [tex]V[/tex]:

[tex]V = \dfrac{(0.71378\text{ mole})\,(0.08206 \text{ L}\cdot\text{atm} \, / \, [\text{mole} \cdot \text{K}])\,(273.15\text{ K})}{1\text{ atm}}[/tex]

[tex]\boxed{V = 16.00 \text{ L}}[/tex]

So, the volume of ammonia produced by the given reaction is 16.00 Liters.

wongjianyit

Answer: 44.8liters

To calculate the volume of ammonia produced at STP (Standard Temperature and Pressure) from the complete reaction of nitrogen with excess hydrogen, we first need to determine the moles of nitrogen and then use the stoichiometry of the reaction to find the moles of ammonia. Finally, we can apply the ideal gas law to find the volume.

The balanced chemical equation for the reaction between nitrogen (N₂) and hydrogen (H₂) to form ammonia (NH₃) is:

N2 +3H2→2NH 3

Find moles of nitrogen (N₂):

Moles=Mass / Molar Mass

The molar mass of nitrogen (N₂) is approximately

28.02g/mol

Moles of N=10.00 g

28.02 g/mol

Moles of N₂=

28.02g/mol

10.00g

Use stoichiometry to find moles of ammonia (NH₃):

From the balanced equation, 1 mole of nitrogen reacts to produce 2 moles of ammonia.

Moles of NH₃=2×Moles of N₂

Apply the ideal gas law to find volume at STP:

At STP, 1 mole of any gas occupies approximately

22.4liters.

Volume of NH₃=2×22.4liters=44.8 liters

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