To calculate the number of moles in an experiment, you need to know the mass of the substance and its molecular weight. The number of moles is then found by dividing the mass by the molecular weight. This applies to any substance, including bromobenzene, magnesium, and benzophenone.
To calculate the number of moles of bromobenzene, magnesium, and benzophenone you will use in the experiment, we first need the molecular weights of each substance. The molecular weights determined from experimental data are crucial to this calculation. The number of moles of a compound is equal to the mass of the compound divided by its molecular mass. For example, if we consider a substance like benzene, the molecular formula is C6H6 which is derived from its empirical formula CH, and the ratio of the elements within it. Let's say you have 'm' grams of bromobenzene, 'n' grams of magnesium, and 'p' grams of benzophenone. Also, let the molecular weights of bromobenzene, magnesium, and benzophenone be 'M', 'N', and 'P' respectively. Then the number of moles of bromobenzene would be m/M, of magnesium would be n/N, and of benzophenone would be p/P. To get the exact values, you would need the specific weights of these substances in your experiment. Remember to ensure that the weights are in grams (for mass) and g/mol (for molecular weight) since the number of moles is a dimensionless quantity.
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Answer:
Explanation:
1. q=mcat
q = (20)(4.184)( 30-20)
q = 836.8
Answer:
A. Metal
Explanation:
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Answer:
Metal
Explanation:
they deleted my answer so I am putting it back sorry
The safest method for diluting concentrated sulfuric acid with water is to add acid to water. This way, when spill occurs, the acid is already diluted and less harmful than adding water to acid.
Explanation:
The electron configuration you provided is for the element with 3 electrons. The 2p² electron configuration would involve adding two more electrons to the 2p subshell. Let's determine the four quantum numbers (n, l, ml, and ms) for one of these 2p² electrons:
1. Principal Quantum Number (n): In this case, n is the same as the principal quantum number for the 2p subshell, which is 2.
2. Azimuthal Quantum Number (l): The azimuthal quantum number (l) represents the subshell within the principal energy level. For the 2p subshell, l = 1.
3. Magnetic Quantum Number (ml): The magnetic quantum number (ml) specifies the orientation or orbital within a subshell. For the 2p subshell, ml can take on three values: -1, 0, and 1. Since we're describing one of the two 2p² electrons, you can choose either -1 or 1 for ml.
4. Spin Quantum Number (ms): The spin quantum number (ms) represents the spin of the electron. It can have two values: +1/2 (spin up) or -1/2 (spin down). You can choose either +1/2 or -1/2 for ms.
So, one possible set of quantum numbers for one of the 2p² electrons could be:
n = 2
l = 1
ml = 1 (or -1)
ms = +1/2 (or -1/2)
You can choose either ml = 1 and ms = +1/2 or ml = -1 and ms = -1/2 for one of the 2p² electrons, as long as the other electron in the same orbital has the opposite spin.
The quantum numbers of an electron in the 2p orbital with the electron configuration 1s² 2s² 2p¹ are principal quantum number (2), azimuthal quantum number (1), magnetic quantum number (-1, 0 or 1) and spin quantum number (+1/2 or -1/2). These numbers represent the energy level, orbital shape, orbital orientation and electron's spin respectively.
The electron configuration expressed as 1s² 2s² 2p¹ represents how electrons are distributed in an atom's atomic orbitals. Examining this, it indicates that there are two electrons in the 1s orbital, two electrons in the 2s orbital, and one electron in the 2p orbital. The four quantum numbers of the electron in the 2p orbital are principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (m_l), and spin quantum number (m_s).
The principal quantum number (n), denotes the energy level the electron is in, in this case, 2.
The azimuthal quantum number (l), also, known as the orbital quantum number indicates the shape of the orbital, for a 'p' orbital, l = 1.
The magnetic quantum number (m_l), describes the orientation of the orbital - this can have any value from -l to +l. For a 'p' orbital, m_l could be -1, 0, or 1, representing the three 'p' orbitals, 2px, 2py, and 2pz respectively.
Finally, the spin quantum number (ms) will be either +1/2 or -1/2, representing the two possible spin states of an electron.
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