How many moles of NH₃ can be produced from 4.81 moles of nitrogen in the following reaction:

Chemistry

1 answer:

makkiz [27]4 years ago

8 0

Answer:

9.62moles of NH₃

Explanation:

Given parameters:

Number of moles of nitrogen = 4.81moles

Unknown:

Number of moles of NH₃ = ?

Solution:

To solve this problem, we need to establish a balanced reaction equation:

N₂ + 3H₂ → 2NH₃

Now, we can solve the problem by working from the known to the unknown.

1 mole of N₂ produced 2 moles of NH₃

4.81moles of N₂ will produce 2 x 4.81 = 9.62moles of NH₃

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How many molecules in each sample? 64.7 g N2 83 g CCl4 19 g C6H12O6

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Answer:

1.39x10²⁴ molecules N₂

.25x10²³ molecules CCl₄

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Explanation:

First we convert the given masses into moles, using the compounds' respective molar mass:

64.7 g N₂ ÷ 28 g/mol = 2.31 mol N₂

83 g CCl₄ ÷ 153.82 g/mol = 0.540 mol CCl₄

19 g C₆H₁₂O₆ ÷ 180 g/mol = 0.106 mol C₆H₁₂O₆

Then we multiply each amount by Avogadro's number, to calculate the number of molecules:

2.31 mol N₂ * 6.023x10²³ molecules/mol = 1.39x10²⁴ molecules

0.540 mol CCl₄ * 6.023x10²³ molecules/mol = 3.25x10²³ molecules

0.106 mol C₆H₁₂O₆ * 6.023x10²³ molecules/mol = 6.38x10²² molecules

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What is the specific latent heat of fusion for a substance that takes 550 KJ to melt 14 KG at 262 K?

Arte-miy333 [17]

Answer:- The right choice is A. $3.9*10^4\frac{J}{kg}$ .

Solution:- Latent heat of fusion means the heat required to melt the solid at constant temperature means there is no change in temperature only the solid changes to liquid. So, it is a solid to liquid phase change.

$q=m*\Delta H_f_u_s$

where q is the heat required to convert solid to liquid, m is the mass and $\Delta H_f_u_s$ is the latent heat of fusion.

From given info, 550 kJ that is 550000 J of heat is required to melt 14 kg of solid at 262K temperature. Let's rearrange the equation for latent heat of fusion and plug in the values in it.

$\Delta H_f_u_s=\frac{q}{m}$