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"206.46 J/g" energy required to heat the solid iron.
Energy due to change in temperature:
The movements or the activity of microscopic particles known as atoms, molecules, or ions in solids, solvents, as well as gases.
Thermal energy may go from one item towards the another one.
Given:
Temperature, °C
°C
Change,
We know the relation,
→
By putting the values,
J/g
Thus the answer above is right.
Find out more information about energy here:
Answer:
Explanation:
Hello,
In this case, since the energy due to the change of temperature is computed via:
Thus, since the specific heat of iron is 0.444 J/(g°C), the heat per unit of mass turns out:
Best regards.
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Answer: 0.9851mol.
Explanation:
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Answer:
MnO- Manganese Oxide
Explanation:
Empirical formula: This is the formula that shows the ratio of elements
present in a
compound.
How to determine Empirical formula
1. First arrange the symbols of the elements present in the compound
alphabetically to determine the real empirical formula. Although, there
are exceptions to this rule, E.g H2So4
2. Divide the percentage composition by the mass number.
3. Then divide through by the smallest number.
4. The resulting answer is the ratio attached to the elements present in
a compound.
Mn O
% composition 72.1 27.9
Divide by mass number 54.94 16
1.31 1.74
Divide by the smallest number 1.31 1.31
1 1.3
The resulting ratio is 1:1
Hence the Empirical formula is MnO, Manganese oxide
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Answer:
49.4 mol Oxygen
Explanation:
Mg(NO3)2 ----- 6 O
1 mol 6 mol
8.24 mol x mol
x = 8.24*6/1 = 49.44 mol ≈ 49.4 mol Oxygen
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Complete question is;
What is the frequency of light emitted when the electron in a hydrogen atom undergoes a transition from energy level n=6 to level n=3?
Answer:
Frequency = 2.742 × 10^(14) s^(-1)
Explanation:
First of all, the energy of hydrogen electron from online values is;
E_n = -2.18 × 10^(-18) × (1/n²) J
n is the principal quantum number
We are told that hydrogen atom undergoes a transition from energy levels n = 3 to n = 6.
Thus, it means we have to find the difference between the electrons energy in the energy levels n = 3 to n = 6.
Thus;
E_n = E_6 - E_3
Thus;
E_n = [-2.18 × 10^(-18) × (1/6²)] - [-2.18 × 10^(-18) × (1/3²)]
E_n = (2.18 × 10^(-18)) × [-1/36 + 1/9]
E_n = 0.1817 × 10^(-18) J
From Planck expression, we can find the frequency. Thus;
E = hf
Where h is Planck's constant = 6.626 × 10^(-34) m²kg/s
Thus;
0.1817 × 10^(-18) = 6.626 × 10^(-34) × f
f = (0.1817 × 10^(-18))/(6.626 × 10^(-34))
f = 2.742 × 10^(14) s^(-1)
Final answer:
The frequency of light emitted during an electron transition in a hydrogen atom is determined by calculating the energy difference between the two energy levels and then using this to calculate the frequency using the equation for energy of a photon.
Explanation:
The frequency of light emitted during a transition of an electron in a hydrogen atom can be calculated using the formula for the energy difference (∆E) between two energy levels n1 and n2 in the hydrogen energy level diagram.
The formula to calculate energy difference is: ∆E = E(n2) - E(n1) where E(n) represents the energy of an energy level n. The energy difference ∆E is negative when an electron goes down an energy level (i.e., emits a photon), as the energy level n1 is greater than n2.
The frequency of the emitted photon (∆E) is then given by the formula ∆E = hf where h is Planck's constant (6.63 x 10^-34 Joule seconds) and f is the frequency. Therefore, you can rearrange the equation to find the frequency: f = ∆E / h.
Learn more about Electron Transitions here:
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Answer:
Zeros located at the end of significant figures are significant.
Explanation:
Hope it will help :)