Answer:
4.4 × 10^-7
3 × 10^5
Explanation:
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Answer: No, a<span>t high pressures, volume of a real gas does not compare with the volume of an ideal gas under the same conditions.
Reason:
For an ideal gas, there should not be any intermolecular forces of interaction. However, for real gases there are intermolecular forces of interaction like dipole-dipole and dipole-induced dipole. Further, at high pressures, molecules are close by. Hence, extend of these intermolecular forces is expected to be high. This results in decreases in volume of real gas. Thus, </span>volume of a real gas does not compare with the volume of an ideal gas under the same conditions.
Answer:
e−(Ea/RT): the fraction of the molecules present in a gas which have energies equal to or in excess of activation energy at a particular temperature
Rutherford's model shows that an atom is mostly empty space, with electrons orbiting a fixed, positively charged nucleus in set, predictable paths. ... It was after this that Rutherford began developing his model of the atom.
When heating lithium carbonate (Li2CO3), it will dissociate to Li2O and Co2. So the balanced chemical equation of this reaction is Li2CO3 = Li2O + CO2.
