Chemistry, 24.06.2019 07:20 Lilyy1k

When 10.0 g of nh3 reacts, the actual yield of n2 is 8.50 g. what is the percent yield? 4 nh3 (g) + 6 no(g) --> 5 n2 (g) + 6 h2o(l)

Answers: 1

Show answers

Answers

Answer from: khuak877

The percent yield of N₂ is 41.34%

From the question,

We are to determine the percent yield of N₂

The given balanced chemical equation for the reaction is

4NH₃(g) + 6NO(g) → 5N₂(g) + 6H₂O(l)

This means 4 moles of NH₃ reacts with 6 moles of NO to produce 5 moles of N₂ and 6 moles of H₂O

First, we will determine the number of moles of NH₃ that reacted

From the question,

Mass of NH₃ that reacted = 10.0 g

From the formula

$Number\ of\ moles = \frac{Mass}{Molar\ mass}$

Molar mass of NH₃ = 17.031 g/mol

∴ Number of moles of NH₃ that reacted = $\frac{10.0}{17.031 }$

Number of moles of NH₃ that reacted = 0.58716 mole

Now, we will determine the theoretical number of moles of N₂ produced

From the balanced chemical equation

Since

4 moles of NH₃ reacts to produce 5 moles of N₂

Then,

0.58716 mole of NH₃ will react to produce $\frac{0.58716 \times 5}{4}$ moles of N₂

$\frac{0.58716 \times 5}{4} = 0.73395$

∴ The theoretical number of moles of N₂ that would be produced is 0.73395 mole

Now, we will determine the theoretical yield in grams

Using the formula

Mass = Number of moles × Molar mass

Molar mass of N₂ = 28.0134 g/mol

∴ Mass of N₂ that would be produced = 0.73395 × 28.0134

Mass of N₂ that would be produced = 20.56 g

∴ The theoretical yield of N₂ is 20.56 g

Now, for the percent yield

$Percent\ yield = \frac{Actual\ yield}{Theoretical\ yield}\times 100\%$

From the question,

Actual yield of N₂ = 8.50 g

∴ Percent yield of N₂ = $\frac{8.50}{20.56}\times 100\%$

Percent yield of N₂ = 41.34 %

Hence, the percent yield of N₂ is 41.34%

Learn more here: link

Answer from: XynonAdat

%Yield = 41.3% (w/w)

Explanation:

4NH₃ + 6NO => 5N₂ + 6H₂O

10g NH₃ = (10/17)mole NH₃ = 0.588 mole NH₃ => 5/4(0.588)mole N₂ = 0.735 mole N₂ x 28g N₂/mole N₂ = 20.58g N₂ (Theoretical Yield)

Given Actual Yield = 8.5g N₂

%Yield = (Actual Yield/Theoretical Yield)100% = (8.5g N₂/20.58g N₂)100% =41.3% Yield (w/w)

Answer from: Quest

answer: the primary difference between a hypothesis and a theory is that b hypothesis is falsifiable, but a theory has been proven to be correct. theory is an explanation of something that is happening but hypothesis is a guess of something that can happen

explanation:

Answer from: Quest

It could possibly be beneficial if the experiment is successful.

Another question on Chemistry

Chemistry, 22.06.2019 02:30

What does the cell nucleus do or, how does it function?

Answers: 1

Answer

Chemistry, 22.06.2019 10:00

Why is carbon ideal for making different compounds?

Answers: 2

Answer

Chemistry, 22.06.2019 18:00

How many moles of oxygen gas are produced from the decomposition of six moles of potassium

Answers: 1

Answer

Chemistry, 23.06.2019 00:50

Which of the following warnings would an agricultural chemist tell a farmer who wants to recycle his or her own ammonia? recycling ammonia is a difficult process that sometimes takes weeks. recycling ammonia requires a degree in biochemistry or a related field. recycling ammonia can be harmful because it is highly flammable and toxic. recycling ammonia costs too much money considering the price of the necessary chemicals.

Answers: 1

Answer

You know the right answer?

When 10.0 g of nh3 reacts, the actual yield of n2 is 8.50 g. what is the percent yield? 4 nh3 (g) +...

Questions