Answer:
250,000 ML is equal to 250 Liters.
Explanation:
The term 'Mili' multiplies the term 'Liter' by 1,000. Per every liter is 1000 milliliters.
Equilibrium is a state of balance or a stable situation where the opposing forces cancel each other out and where no changes are occurring.
<h3>How to explain the equilibrium?</h3>
Your information is incomplete. Therefore, an overview will be given. In a chemical reaction, chemical equilibrium is a state where the reactants and products are present in concentrations that have no further tendency to change with time.
In terms of volume changes within a system at equilibrium, the following applies:
- When there is a decrease in volume, then the equilibrium will shift to favor the direction that produces fewer moles of gas.
- When there is an increase in volume, then the equilibrium will shift to favor the direction that produces more moles of gas.
In conclusion, if you increase the pressure of a system at equilibrium, the stress will be reduced by reaction that favors the side with the fewest moles of gas.
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Answer:
A- Small ice pellets that may fall to the ground in a mixture of rain and snow in the form of a solid
Explanation:
Small ice pellets that may fall to the ground in a mixture of rain and snow in the form of a solid best describes hail.
1.Find the number of mole of N2H4
2.Number of mole of N2H4 X Avogadro constant
TLDR: It’s D.
This is a principle of quantum chemistry, where a subset of n, l, m, and s numbers identify a specific type of atom. The Pauli Exclusion Principle states that two elements that are not the same can not have the same four quantum numbers.
N represents the principal quantum number, L represents the azimuthal quantum number, M represents the magnetic quantum number, and S represents the atomic spin.
The rules are as follows:
L < N
M= -L to + L
S = +,- 1/2 (although this one doesn’t matter since it isn’t asked)
Therefore, D doesn’t work as the azimuthal quantum value exists outside of the principal boundary that L must be less than N (3 /< 2).
