Question

What product or ratio of properties remains constant (PxT, TxV, P/V, V/T, etx)?When you have decided, label the "constant?" column with proper term and fill in the values.

Answer 1

The product of pressure and volume (P x V) remains constant at constant amount and temperature. This is known as Boyle's Law and can be used to calculate the change in pressure or volume when the other property changes, as long as the amount and temperature remain constant.

Step-by-step explanation:

The product of pressure (P) and volume (V), represented as P x V, remains constant at constant amount (n) and temperature (T).

This means that if either the volume or pressure changes while the amount and temperature stay the same, the other property must change in order to maintain the constant product. For example, if the original conditions are labeled P₁ and V₁ and the new conditions are labeled P₂ and V₂, we have P₁V₁ = P₂V₂ at constant n and T.

This relationship is also known as Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume at constant temperature and amount of gas. As the volume of a gas decreases, the pressure increases, and vice versa, as long as the amount and temperature are kept constant.

Therefore, we can label the 'constant' column in the ratio of properties as 'P x V' and fill in the values accordingly.

Answer 2

In this phenomenon we talk about ideal gases, that is why in these equations the constant is the number of moles and the constant R, which has a value of 0.082

Step-by-step explanation:

The complete equation would have to be P x ​​V = n x R x T

where n is the number of moles, and if it is not clarified it is because they remain constant, as the question was worded.

On the other hand, the symbol R refers to the ideal gas constant, which declares that a gas behaves like an ideal gas during the reaction, and its value will always be the same, which is why it is called a constant. The value of R = 0.082.

The ideal gas model assumes that the volume of the molecule is zero and the particles do not interact with each other. Most real gases approach this constant within two significant figures, under pressure and temperature conditions sufficiently far from the liquefaction or sublimation point. The real gas equations of state are, in many cases, corrections to the previous one.

The universal constant of ideal gases is not a fundamental constant (therefore, choosing the temperature scale appropriately and using the number of particles, we can have R = 1, although this system of units is not very practical)