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Eddi Din [679]
3 years ago
12

Scientific predictions based on laws are formulated using:

Chemistry
2 answers:
abruzzese [7]3 years ago
7 0

Answer:

A. deductive reasoning

Artist 52 [7]3 years ago
3 0
The answer is definitely A
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On a distance-time graph, at 2 hours the graph is at a height of 20 meters, and at 3 hours it is at a height of 100 meters. What
Gnoma [55]

Answer:

80 m/hr

Explanation:

Changes from 20 to 100 meters in ONE Hour

    changes  80 meters in one hour    = 80 m/hr

8 0
1 year ago
Suppose you see a crescent Moon. How do you know if it is waxing or waning?
nasty-shy [4]

Answer:

waxing is in the evening and waning is in the morning if you cant see the moon in the evening it is waning if you can see it in the evening it is waxing

5 0
2 years ago
Determine the mass of 9.2 x 10^18 molecules of dinitrogen tetroxide.
steposvetlana [31]

Answer: 1.4x10-3 g N2O4

Explanation: First convert molecules of N2O4 to moles using Avogadro's Number. Then convert moles to mass using the molar mass of N2O4.

9.2x10^18 molecules N2O4 x 1 mole N2O4 / 6.022x10²³ molecules N2O4

= 1.53x10-5 moles N2O4

1.53x10-5 moles N2O4 x 92 g N2O4/ 1 mole N2O4

= 1.4x10-3 g N2O4

4 0
3 years ago
Suppose the flask is already at equilibrium but then the volume of the reaction flask is then reduced what will happen
sveta [45]

1) Answer is: c) The reaction will proceed right.

Balanced chemical reaction: N₂(g) + 3H₂(g) ⇄ 2NH₃(g) ΔH = +92 kJ.

Reducing the volume of the system increase the partial pressures of the products and reactants.

With a pressure increase due to a decrease in volume, the side of the equilibrium with fewer moles is more favorable, there are 4 moles at the left side (three moles of hydrogen and one mole of nitrogen) and 2 moles (ammonia) at the right side of the reaction.

2) Answer is: d) The partial pressure of ammonia will increase.

This reaction is endothermic (enthalpy is higher than zero), which means that heat is added.

According to Le Chatelier's principle when the reaction is endothermic heat is included as a reactant and when the temperature increased, the heat of the system increase, so the system consume some of that heat by shifting the equilibrium to the right,  producing more ammonia.

8 0
3 years ago
Identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid and the conjugate base for each of the following r
Vlad1618 [11]

Answer:

Acids → H₂CO₃ from equilibrium 1 and water, from equilibrium 2.

Bases → Water from equilibrium 1 and ammonia from equilibrium 2.

In 1st equilibrium, H₃O⁺ is the conjugate acid and HCO₃⁻ the conjugate base.

In 2nd equilibrium, NH₄⁺ is the conjugate acid, and OH⁻, the conjugate base.

Explanation:

By the Bronsted-Lowry you know that acids are the one that release protons and base are the ones that catch them.

For the first equilibrium:

H₂CO₃(aq) + H₂O(l) ⇄ H₃O⁺(aq) + HCO₃⁻(aq)

Carbonic acid is the acid → It donates the proton to water, so the water becomes the base. As H₂CO₃ is the acid,  the bicarbonate is the conjugate base (it can accept the proton from water to become carbonic acid, again) and the hydronium is the conjugate acid (it would release the proton to become water).

For the second equilibrium:

NH₃(aq) + H₂O(l) ⇄  NH₄⁺ (aq) + OH⁻(aq)

This is the opposite situation → Water relase the proton to ammonia, that's why water is the acid and NH₃, the base (it accepted to become ammonium). The NH₄⁺ is the conjugate acid (it can release the H⁺ to become ammonia) and the OH⁻ is the conjugate base (It can accept the proton to become water, again).  

5 0
3 years ago
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