What is the entropy of a solid based on

In chemical reactions, there is a conservation of(1) energy, volume and mass

Answer: option (3) energy, charge and mass.


Explanation:


1) The conservation of energy is a universal principle: energy is neither created nor destroyed. This is the first law of thermodynamic.


2) Mass conservation is another universal principle: mass is neither created nor destroyed. This principle is the base of the stochiometry: thas mass of the reactans equal the mass of the products. Another consequence, since the atoms are not transformed in the chemical reactions, is that the number of each kind of atoms in the reactants equal the number of the same kind of atoms in the products.


3) The third principle is the conservation of charge. Also, charge is neither created nor destroyed. The electrons gained/lost by one species are lost/gained by other species. So, when one atom or molecule is oxidized other is reduced.

4 0

4 years ago

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The first stage of photosynthesis produces _____ and _____.

Igoryamba

I believe its hydrogen and carbon dioxide.

5 0

3 years ago

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i like this guy but i don't think he likes me back. he also goes to school somewhere else, but we see eachother every friday. he

Firdavs [7]

You should try to strt a conversation with him or say hi introduce yourself or ask him how hes doing just talk to him i guess

3 0

4 years ago

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The energy E of the electron in a hydrogen atom can be calculated from the Bohr formula:

uysha [10]

Answer:

The wavelength of the line in the absorption line spectrum of hydrogen caused by transition is 657.1 nm.

Explanation:

Energy of the electron in a hydrogen atom in nth shell:

$E=\frac{-R_y}{n^2}$

$R_y=2.178\times 10^{-18} J$

Energy of an electron in n = 2:

$E_2=\frac{-R_y}{2^2}=-\frac{R_y}{4}$

Energy of an electron in n = 3:

$E_3=\frac{-R_y}{3^2}=-\frac{R_y}{9}$

Energy difference in between both the shells:

$\Delta E=E_3-E_2$ :

$=-\frac{R_y}{9}-(-\frac{R_y}{4})=\frac{5R_y}{36}$

$\Delta E=\frac{5R_y}{36} =\frac{5\times 2.178\times 10^{-18} J}{36}$

$=3.025\times 10^{-19} J$

$\Delta E=3.025\times 10^{-19} J=\frac{hc}{\lambda}$

$\lambda =\frac{hc\times 36}{3.025\times 10^{-19} J}$

= $\frac{6.626\times 10^{-34} J s\times 3\times 10^8 m/s}{3.025\times 10^{-19} J}$

$\lambda =6.571\times 10^{-7} m=657.1 nm$

$1 m = 10^9 nm$

The wavelength of the line in the absorption line spectrum of hydrogen caused by transition is 657.1 nm.

8 0

4 years ago

When production first began some eighty years ago, ammonia production relied upon the direct reaction between gaseous hydrogen a

kondaur [170]

Answer:

Option 2. Produce more ammonia.

Explanation:

The influence of temperature in equilibrium reactions can be predicted from the heat (enthalpy) information.

This is the chemical reaction:

3 H₂ (g) + N₂(g) ⇄ 2 NH₃(g) ∆H = −92.2 kJ

The information about the enthalpy of the reaction, ∆H = − 92.2 kJ, indicates that energy (heat) has been released to the surroundings (the products of the forward reaction have less energy than the reactants), which is defined as an exothermic reaction.

Then, you can rewrite the equaition in the form:

3 H₂ (g) + N₂(g) ⇄ 2 NH₃(g) + 92.2 kJ

This is, the heat can be seen as a product of the direct reaction (or a reactant of the reverse reaction).

Now, it is quite straight to apply Le Chatelier's principle:

a) Decreasing temperature is equivalent to extract heat or having less heat on the left side.

b) Then, the equilibrium must shift in a way that this lack of heat is compensated. Then, the reaction will shift to the right to produce more heat.

As conclusion, you can tell that in exothermic reactions, a decrase in temperature will cause the equilibrium to shift to the right.

This shift, of course, means the production of more ammonia.

The other choices are discarded following this brief reasoning:

1. increase the velocity of the gas molecules: the average velocity of the particles increases when the average kinetic energy increases, and the average kinetic energy will decrease if the temperature decreases. So, this statement is false.

3. increase the kinetic energy of the gas molecules: no, the average kinetic energy is proportional to the temperature, then reducing the temperature decreasese the average kinetic energy.

4. produce less ammonia: it was shown that reducing the temperature will produce more ammonia.

5. have no effect: no, it does have effect, as shown.

6 0

3 years ago