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3 years ago

If nitrogen and hydrogen combine in a synthesis reaction, what would the product of the reaction be? n2 + 3h2 → 3

Chemistry

2 answers:

mario62 [17]3 years ago

5 0

Answer: Ammonia ( $NH_3$ )

Explanation: A synthesis reaction is one in which two or more than two elements combine together to forma single product.

The atoms present in the reactants are found on the product side. According to the law of conservation of mass, the number of atoms on both sides of the arrow must be same as the total mass must be conserved.

Thus the balanced chemical equation is:

$N_2+3H_2\rightarrow 2NH_3$

Fed [463]3 years ago

4 0

N2 + 3H2 ---> 2NH3
nitrogen + hydrogen ---> ammonia

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Two liquids, a and b are immiscible. liquid a has a density of 0.89 g/ml. liquid b has a density of 0.72 g/ml. what would you ex

Burka [1]

In the given above, we have two densities which are 0.89 g/mL and 0.72 g/mL. We are also given that the liquids are immiscible. After the settlement of the liquids, they will form two layers.

The heavier substance, the one which has a higher density will be at the bottom and the lighter substance, the one which has a lower density will be at the top layer.

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3 years ago

Determine whether or not the equation below is balanced. If it isn’t balanced, write the balanced form. Also, identify the react

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Answer:

Explanation:

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3 years ago

Read 2 more answers

Which of the following best describes a single replacement reaction?

Lady_Fox [76]

Answer:

One element takes the place of another in a compound

Explanation:

I just took a test for it and got it right. :)

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3 years ago

Calculate the energy that is required to change 50.0 g ice at -30.0°C to a liquid at 73.0°C. The heat of fusion = 333 J/g, the h

OverLord2011 [107]

Answer:

There is 3.5*10^4 J of energy needed.

Explanation:

Step 1: Data given

Mass of ice at -30.0 °C = 50.0 grams

Final temperature = 73.0 °C

The heat of fusion = 333 J/g

the heat of vaporization = 2256 J/g

the specific heat capacity of ice = 2.06 J/gK

the specific heat capacity of liquid water = 4.184 J/gK

Step 2: Calculate the heat absorbed by ice

q = m*c*(T2-T1)

⇒ m = the mass of ice = 50.0 grams

⇒ c = the heat capacity of ice = 2.06 J/gK = 2.06 J/g°C

⇒ T2 = the fina ltemperature of ice = 0°C

⇒ T1 = the initial temperature of ice = -30.0°C

q = 50.0 * 2.06 J/g°C * 30 °C

q = 3090 J

Step 3: Calculate heat required to melt the ice at 0°C:

q = m*(heat of fusion)

q = 50.0* 333J/g

q = 16650 J

Step 4: Calculate the heat required to raise the temperature of water from 0°C to 73.0°C

q = m*c*(T2-T1)

⇒ mass = 50.0 grams

⇒ c = the specific heat of water = 4.184 J/g°C

⇒ ΔT = T2-T1 = 73.0 - 0 = 73 °C

q = 50.0 * 4.184 * 73.0 = 15271.6 J

Step 5: Calculate the total energy

qtotal = 3090 + 16650 + 15271.6 = 35011.6 J = 3.5 * 10^4 J

There is 3.5*10^4 J of energy needed.

8 0

3 years ago

7. Compare and contrast a dilute solution of a strong acid

Cloud [144]

Explanation:

An acid is a substance that ionizes to produce excess hydrogen ion in solutions.

A concentrated acid contains a high amount of hydrogen ions in solution compared to other ions.
Such solutions usually ionizes completely.
A dilute solution contains a high proportion of water and with low amount of hydrogen ions.
They do not ionize easily and as fast as strong acids.

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3 years ago