<span>1 mole of any substance contain Avogadro's number of molecules so we can calculate the number of moles by dividing the provided number of atoms over Avogadro's number to obtain the number of moles
Answer : 19.9 moles of phosphorus
Solution : Atoms / Avogadro's number (6.022 x 10</span>²³<span> atoms/mol)
1.20 x 10</span>²⁵<span> atoms / 6.022 x 10</span>²³<span> = 19.927</span>
A answer.
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Answer:
At temperatures greater than 756 °C this reaction is spontaneous under standard conditions.
Explanation:
Let's consider the following reaction.
C(s) + H₂O(g) ⇄ CO(g) + H₂(g)
The reaction is spontaneous when the standard Gibbs free energy ΔG° < 0. ΔG° is related to the standard enthalpy of the reaction (ΔH°) and the standard entropy of the reaction (ΔS°) through the following expression.
ΔG° = ΔH° - T.ΔS°
If ΔG° < 0
ΔH° - T.ΔS° < 0
ΔH° < T.ΔS°
T > ΔH°/ΔS° = (131.3 × 10³ J/mol)/(127.6 J/K.mol) = 1029 K
The temperature in Celsius is:
°C = K - 273.15 = 1029 - 273.15 = 756 °C
Answer:
1.64x10⁻¹⁸ J
Explanation:
By the Bohr model, the electrons surround the nucleus of the atom in shells or levels of energy. Each one has it's energy, and the electron doesn't fall to the nucleus because it can reach another level of energy, and then return to its level.
When the electrons go to another level, it absorbs energy, and then, when return, this energy is released, as a photon (generally as luminous energy). The value of the energy can be calculated by:
E = hc/λ
Where h is the Planck constant (6.626x10⁻³⁴ J.s), c is the light speed (3.00x10⁸ m/s), and λ is the wavelength of the photon.
The wavelength can be calculated by:
1/λ = R*(1/nf² - 1/ni²)
Where R is the Rydberg constant (1.097x10⁷ m⁻¹), nf is the final orbit, and ni the initial orbit. So:
1/λ = 1.097x10⁷ *(1/1² - 1/2²)
1/λ = 8.227x10⁶
λ = 1.215x10⁻⁷ m
So, the energy is:
E = (6.626x10⁻³⁴ * 3.00x10⁸)/(1.215x10⁻⁷)
E = 1.64x10⁻¹⁸ J
the balanced equation for the combustion of ethane is as follows
2C₂H₆ + 7O₂ --> 4CO₂ + 6H₂O
molar ratio of C₂H₆ to H₂O is 2:6
this means that when 2 mol of C₂H₆ react 6 mol of H₂O are produced
for every 1 mol of C₂H₆ that reacts thrice the number of moles of H₂O are produced
therefore when 1.4 mol of C₂H₆ reacts - 3 x 1.4 = 4.2 mol of H₂O are produced
the answer is 4.2 mol