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Advocard [28]
3 years ago
5

How many grams of nh3 can be produced from the reaction of 28 g of n2 and 25 g of h2

Chemistry
1 answer:
vfiekz [6]3 years ago
5 0

Answer:

  • <u><em>34 g of NH₃ </em></u><em>will be produced from the reaction of   28 g of N₂ with 25 g of H₂.</em>

Explanation:

1) <u>Balanced chemical equation</u>

  • N₂ (g) + 3H₂ (g) → 2NH₃(g)

2) <u>Stoichiometric (theoretical ) mole ratios</u>

  • 1 mol N₂ (g) : 3mol H₂ (g) : 2 mol NH₃(g)

3) <u>Number of moles of each reactant</u>

  • number of moles = mass in grams / atomic mass

  • number of moles of N₂ = 28 g / 28 g/mol = 1 mol

  • number of moles of H₂: 25 g / 2 g/mol = 12.5 mol

4)<u> Limiting reactant</u>

Since the stoichiometry states that 1 mol of N₂ reacts with 3 moles of H₂, the given mass of N₂ will react completely with the given amount of H₂, and the calculations must be done with the 28 g (1 mol) of N₂ as the limiting reactant.

5) <u>Yield</u>

Set the proportion with the mole ratios:

1 mol H₂ / 2 mol NH₃ = 1  mol H₂ / x ⇒ x = 2 mol NH₃

6) <u>Convert to grams</u>

  • mass in grams = number of moles × molar mass = 2 mol × 17 g/mol = 34 g.

Answer: <em>the reaction of 28 g of N₂ with 25 g of H₂ will produce 34 g of NH₃</em>

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Explanation:

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18000 g of Nickel is deposited by = \frac{193000}{58.7}\times 18000=59182282.8C of electricity

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I = current in amperes = 31.0 A

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(1h=3600 sec)

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When 3.93 grams of lactic acid, CHoOs(s), are burned in a bomb
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The heat released in the combustion of lactic acid is absorbed by the

calorimeter and in the decomposition of the lactic acid.

ΔH°f of lactic acid is approximately <u>-716.2 kJ</u>

Reasons:

Known parameters are;

Mass of the lactic acid = 3.93 grams

Heat  capacity of the bomb calorimeter = 10.80 kJ·K⁻¹

Change in temperature of the calorimeter, ΔT = 5.34 K

ΔHrxn = ΔErxn

ΔH°f of H₂O(l) = -285.8 kJ·mol⁻¹

ΔH°f of CO₂(g) = -393.5 kJ·mol⁻¹

The chemical equation for the reaction is presented as follows;

  • C₃H₆O₃ + 2O₂ → 3CO₂ + 3H₂O

The heat of the reaction = 10.80 kJ·K⁻¹ × 5.34 K = 57.672 kJ

Molar mass of C₃H₆O₃ = 90.07 g/mol

Number of moles of C₃H₆O₃ = \dfrac{3.93 \, g}{90.07 \, g/mol} = 0.043633 moles

Number of moles of CO₂ produced = 3 × 0.043633 moles = 0.130899 moles

Heat produced = 0.130899 mole × -285.8 kJ·mol⁻¹ = -37.4109342 kJ

Moles of H₂O produced = 0.130899 moles

Heat produced = 0.130899 mole × -393.5 ≈ -51.51 kJ

Therefore, we have;

Heat absorbed by the lactic acid = ΔH°f of H₂O + ΔH°f of CO₂ + Heat absorbed by the calorimeter

Which gives;

Heat absorbed by lactic acid  = -37.4109342 kJ - 51.51 kJ + 57.672 kJ ≈ -31.249 kJ

The heat absorbed by the lactic acid ≈ -31.249 kJ

  • \Delta H^{\circ}f \ of \ C_3H_6O_3 = \dfrac{-31.249}{0.043633} \approx  -716.2

ΔH°f of C₃H₆O₃ ≈ -716.2 kJ

Heat of formation of lactic acid ≈ <u>-716.2 kJ</u>.

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brainly.com/question/13185938

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