Explanation:
The atoms of one element differs from the atoms of other elements in terms of the number of protons they contain. This is often taken as the atomic number of such an atom.
- The number of proton is the best indicator of the atom one is dealing with.
- Based on this number, elements are categorized into distinct columns and rows on the periodic table.
- The atomic number is the number of protons or positively charge particles in the atom.
II.
It is possible to change the identity of an atom. This is only possible by altering the atomic number of the atom.
Only nuclear reactions have this capability.
When an atom undergoes nuclear reaction that involves change in number of protons, transmutation occurs and a new atom forms.
Chlorine is a halogen and all halogens and oxygen, nitrogen and hydrogen are diatomics
Answer:
Al(NO₃)₃ > KI > HF > CH₃OH
Explanation:
The electrical conductivities of the solutions will depend on the concentration of ions in solution.
Al(NO₃)₃ solution contains 0.1 M of Al³⁺ ions and 0.3 M of NO₃⁻ ions
KI solution contains 0.1 M of K⁺ ions and 0.1 M of I⁻ ions
HF solution contains less than 0.1 M of H⁺ ions and less then 0.1 M of F⁻ ions, because the HF acid will not dissociate completely
CH₃OH practically it does not dissociate, so in the solution will not be electrical conductive (comparative with the other solutions)
The solutions in order of decreasing intensity of the bulb are ranked as following:
Al(NO₃)₃ > KI > HF > CH₃OH
Molar mass is the given substance divided by the amount of that substance, measured in g/mol.
Example: titanium atomic mass is 47.88 amu or 47.88 g/mol. In 47.88 grams of titanium there is 1 mole, or 6.022 x 10^23 titanium atoms.
Answer:- partial pressure of Kr = 0.306 atm, partial pressure of oxygen = 0.264 atm and partial pressure of carbon dioxide = 0.396 atm
Total pressure is 0.966 atm
Solution:- moles of Kr = 21.7 g x (1mol/83.8g) = 0.259 mol
moles of oxygen = 7.18 g x (1mol/32g) = 0.224 mol
moles of carbon dioxide = 14.8 g x (1mol/44g) = 0.336 mol
Volume of container = 23.1 L and the temperature is 59 + 273 = 332 K
From ideal gas law equation, P = nRT/V
partial pressure of Kr = (0.259 x 0.0821 x 332).23.1 = 0.306 atm
partial pressure of oxygen = (0.224 x 0.0821 x 332)/23.1 = 0.264 atm
partial pressure of carbon dioxide = (0.336 x 0.0821 x 332)/23.1 = 0.396 atm
Total pressure of the gas mixture = 0.306 atm + 0.264 atm + 0.396 atm = 0.966 atm
