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lora16 [44]
3 years ago
6

Answer this i will mark brainliest and don't steal points im gonna report you ​

Chemistry
2 answers:
jeka943 years ago
8 0

Answer:

The answer is c

Explanation:

Nuetrik [128]3 years ago
3 0
The answer is for this is A
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In a particular reaction 6.80g of dinitrogen trioxide gas (N203) was actually produced by
xenn [34]

Answer:

<em />

<em>a) Balanced chemical equation:</em>

<em />

<em>       </em>2N_2(g)+3O_2(g)\longrightarrow 2N_2O_3(g)<em />

<em />

<em>b) Theoretical yield:</em>

  • 27.4 g of N₂O₃

c) % yield:

  • 24.5%

Explanation:

The complete question is:

<em>In a particular reaction 6.80g of dinitrogen trioxide gas (N₂0₃) was actually produced by reacting 8.75g of oxygen gas (O₂) with excess nitrogen gas (N₂)</em>

<em>a) Write a balanced chemical equation for the reaction. Be sure to include physical states in the equation.</em>

<em>b) Calculate the theoretical yield (in grams) of dinitrogen trioxide: Use dimensional analysis</em>

<em>c) Calculate the % yield of the product</em>

<em />

<h2>Solution</h2>

<em />

<em>a) Write a balanced chemical equation for the reaction. Be sure to include physical states in the equation.</em>

<em />

<em>       </em>2N_2(g)+3O_2(g)\longrightarrow 2N_2O_3(g)<em />

<em />

Check the balance:

<em />

Atom     Left-handside    Right-hand side

  N              2×2=4                  2×2=4

  O              3×2=6                  2×3=6

  • Mole ratio: it is the ratio of the coefficients of the balanced equation

        \dfrac{2molN_2O_3}{3molO_2}

<em>b) Calculate the theoretical yield (in grams) of dinitrogen trioxide: Use dimensional analysis</em>

<em />

<u>1. Convert 8.75 g of O₂(g) to number of moles</u>

  • number of moles = mass in grams / molar mass
  • molar mass of O₂ = 15.999g/mol
  • number of moles = 8.75g / 15.999 g/mol = 0.5469 mol O₂

<u />

<u>2. Use dimensional analysis to calculate the maximum number of moles of N₂O₃(g) that can be produced</u>

      \dfrac{2molN_2O_3}{3molO_2} \times 0.5469molO_2=0.3646molN_2O_3

<u>3. Convert to mass in grams</u>

  • mass = number of moles × molar mass
  • molar mass of N₂O3 = 76.01g/mol
  • mass = 0.3646mol × 76.01g/mol = 27.7g N₂O3

<em>c) Calculate the % yield of the product</em>

<em />

Formula:

<em />

  • %yield = (actual yield/theoretical yield)×100

Substitute and compute:

  • % yield = (6.80g/27.7g)×100 = 24.5%

<em />

6 0
3 years ago
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