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sweet-ann [11.9K]
3 years ago
5

Describe each relationship in the box below. In each box write, direct relationship, inverse relationship, or no relationship.

Chemistry
1 answer:
avanturin [10]3 years ago
7 0

Answer:

Wave Height: the higher the height, the higher the amplitude, and vice versa

wavelength: the shorter the wavelength, the higher the frequency, and vice versa

velocity: the higher velocity, the higher the frequency (and variable amplitude)

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Na2SO3" represents sodium sulfite. What does the 4 mean in the formula 4Na2SO3? There are four atoms of sodium. There are four a
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Identify the types of intermolecular forces found for each of the liquids and relate these to the shape of the drop as seen from
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3 years ago
Ammonia (NH3) reacts with oxygen to form nitric oxide (NO) and water vapor: 4NH3 + 502 4NO + 6H2O b) When 20.0 g NH3 and 50.0 g
Solnce55 [7]

Answer: a) . Ammonia is the limiting reagent

b. Oxygen is left over and 0.1375 g of oxygen is left over.

c. The theoretical yield of NO is 35.29 g.

d. The theoretical yield of H_2O is 31.74 g.

Explanation:

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}  

For NH_3

Given mass of ammonia = 20.0 g

Molar mass of ammonia = 17.031 g/mol

Putting values in equation 1, we get:

\text{Moles of ammonia}=\frac{20.0g}{17.031g/mol}=1.17mol

For O_2

Given mass of oxygen gas = 50.0 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

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The chemical equation for the reaction is

4NH_3+5O_2\rightarrow 4NO+6H_2O

By Stoichiometry of the reaction:

4 moles of ammonia reacts with = 5 moles of oxygen

So 1.17 moles of ammonia will react with = \frac{5}{4}\times 1.17=1.4625mol of oxygen

As, given amount of oxygen is more than the required amount. So, it is considered as an excess reagent and (1.6-1.4625)= 0.1375 g of oxygen is left unreacted.

Thus ammonia is considered as a limiting reagent because it limits the formation of product.

1. By Stoichiometry of the reaction:

4 moles of ammonia produces = 4 moles of NO

1.17 moles of ammonia will produce = \frac{4}{4}\times 1.17=1.17moles of NO

Mass of NO=moles\times {\text{Molar Mass}}=1.17\times 30=35.29g

Thus Theoretical yield of NO is 35.29 grams.

2. By Stoichiometry of the reaction:

4 moles of ammonia produces = 6 moles of H_2O

1.2 moles of ammonia will produce = \frac{6}{4}\times 1.2=1.8moles of H_2O

Mass of H_2O=moles\times {\text{Molar Mass}}=1.8\times 18.015=31.74g  H_2O

Thus Theoretical yield of H_2O is 31.74 grams.

8 0
3 years ago
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