820 mol of hydrogen gas hydrogen gas has a volume of 2.00 l at a certain temperature and pressure. what is the volume of 0.125 mol of this gas at the same temperature and pressure

 To solve this problem, let us first assume that the hydrogen gas acts like an ideal gas. So that we can make use of the ideal gas equation:

P V = n R T

where P is the pressure, V is the volume, n is the number of moles, R is the universal gas constant and T is the absolute temperature

Since it is given that T and P is constant therefore we can write the equation as:

V / n = k

So equating the two conditions:

V1 / n1 = V2 / n2

We can now solve for the new V2 given n2 = 0.125:

2 L / 820 mol = V2 / 0.125 mol

V2 = 3.05 x 10^-4 L

The new volume is about 3.05 x 10^-4 L which is equivalent to 0.3 mL

current and voltage can both be different in different parts of a circuit so it matters where you place the ammeter and voltmete