At a pressure of 1.00 × 10⁻¹⁰ mmHg and a temperature of 273.15 K, the volume occupied by the 1.00 × 10⁶ moles of gas is 1.70 × 10²³ millilitres. This is derived from the universal gas equation PV = nRT, where V is the volume, n is the number of moles (1.00 × 10⁶), R is the universal gas constant (62.363 mmHg·L/(mol·K)), T is the temperature (273.15 K), and P is the pressure (1.00 × 10⁻¹⁰ mmHg). By substituting these values into the equation, we find the volume in millilitres equals 1.703 × 10²⁰ L converted to millilitres equals 1.703 × 10²³ millilitres.
d is your answer; I hope this assists you.
The reply is: He did not mention any of these topics.
Explanation: Dalton outlined certain postulates for his atomic theory, which are:
1) Matter consists of indivisible atoms.
2) Atoms from different elements combine in fixed proportions to form compounds.
3) The atomic characteristics of a specific element are uniform, including mass. This means all atoms of a given element share the same mass, whereas atoms from different elements exhibit different masses.
4) During a chemical reaction, atoms are not created or destroyed.
5) Atoms of an element are uniform in mass, size, and all other chemical and physical properties.
From these postulates, it is evident that he focused solely on atoms, neglecting subatomic particles or isotopes.
