Question

How many moles of O2 would be required to generate 13. 0 mol of NO₂ in the reaction below assuming the reaction has only 73. 3% yield? 2 NO (g) + O₂ (g) → 2 NO2 (g)

What mass of aspirin (C₉H₈O₄) is produced from 52. 1 g of C₇H₆O₃ assuming 95. 0% yield from the reaction below? C₇H₆O₃ (s) + C₄H₆O₃ (s) → C₉H₈O₄ (s) + HC₂H₃O₂ (aq).

In this reaction: Mg (s) + I₂ (s) → MgI₂ (s), if 10. 0 g of Mg reacts with 60. 0 g of I₂, and 62. 16 g of MgI₂ form, what is the percent yield?

The synthesis of maleic acid anhydride (C₄H₂O₃) can be accomplished by reacting benzene (C₆H₆) and oxygen gas in the following chemical reaction:

2 C₆H₆(l) + 9 O₂(g) → 2 C₄H₂O₃(s) + 4 CO₂(g) + 4 H₂O(g)



If 8. 00 moles of NH₃ of and 10. 00 moles of O₂ react in the following reaction, how many moles of which reactant will be left over?

4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g)

If 0. 275 moles of AgNO₃ react with 0. 155 moles of H₂SO₄ according to this UNBALANCED equation below, how many grams of Ag₂SO₄ could be formed?

AgNO₃(aq) + H₂SO₄ (aq) → Ag₂SO₄ (s) + HNO₃ (aq)

If 37. 3 g of NO and 26. 9 g of O₂ react together, how many grams of NO₂ can be formed via the reaction below?

2 NO (g) + O₂ (g) → 2 NO₂ (g)

You have 2. 2 mol Xe and 3. 8 mol F₂, but when you carry out the reaction you end up with only 0. 25 mol XeF₄. What is the percent yield of this experiment? Xe(g) + 2 F₂ (g) → XeF₄ (g)

Answer 1

Answer: Actual mass of C₉H₈O₄ = (Assumed yield) × (Mass of C₉H₈O₄)

= (0.

Step-by-step explanation:

Let's solve each problem step by step:

To determine the number of moles of O₂ required to generate 13.0 mol of NO₂, we need to use the stoichiometric ratio from the balanced equation:

2 NO (g) + O₂ (g) → 2 NO₂ (g)

From the equation, we can see that the mole ratio between O₂ and NO₂ is 1:2.

Given:

Number of moles of NO₂ = 13.0 mol

To find the moles of O₂, we use the equation:

Moles of O₂ = (Number of moles of NO₂) / 2

Moles of O₂ = 13.0 mol / 2

Moles of O₂ = 6.5 mol

Therefore, 6.5 moles of O₂ would be required to generate 13.0 mol of NO₂.

To calculate the mass of aspirin (C₉H₈O₄) produced from 52.1 g of C₇H₆O₃, assuming a 95.0% yield, we need to consider the stoichiometric ratio and the molar masses of the compounds involved in the reaction:

C₇H₆O₃ (s) + C₄H₆O₃ (s) → C₉H₈O₄ (s) + HC₂H₃O₂ (aq)

Given:

Mass of C₇H₆O₃ = 52.1 g

Assumed yield = 95.0%

First, we need to calculate the moles of C₇H₆O₃ using its molar mass:

Molar mass of C₇H₆O₃ = (7 × 12.01 g/mol) + (6 × 1.008 g/mol) + (3 × 16.00 g/mol)

= 106.12 g/mol

Moles of C₇H₆O₃ = (Mass of C₇H₆O₃) / (Molar mass of C₇H₆O₃)

= 52.1 g / 106.12 g/mol

≈ 0.491 mol

Since the reaction has a 1:1 stoichiometric ratio between C₇H₆O₃ and C₉H₈O₄, the moles of C₉H₈O₄ produced will be the same as the moles of C₇H₆O₃.

Moles of C₉H₈O₄ = 0.491 mol

To find the mass of C₉H₈O₄, we multiply the moles by its molar mass:

Molar mass of C₉H₈O₄ = (9 × 12.01 g/mol) + (8 × 1.008 g/mol) + (4 × 16.00 g/mol)

= 180.16 g/mol

Mass of C₉H₈O₄ = (Moles of C₉H₈O₄) × (Molar mass of C₉H₈O₄)

= 0.491 mol × 180.16 g/mol

≈ 88.52 g

However, we need to consider the 95.0% yield: