At 10.°c, 20.g of oxygen gas exerts a pressure of 2.1atm in a rigid, 7.0l cylinder. assuming ideal behavior, if the temperature of the gas was raised to 40.°c, which statement indicates the new pressure and explains why?

The new pressure of the gas if the ideal gas situation is assumed is; P2 = 2.323atm.

The statement which explains why is the Gay lussac's law; otherwise known as the Amonton's law.

qqThe general ideal gas equation is;

The ideal gas las is however modified in the Amonton's law which states that;

Therefore;

Ultimately, P1/P2 = T1/T2

where:

P2 = (2.1 × 313)/283

P2 = 2.323 atm.

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Ideal gas is a hypothetical gas in which all the collision between the particles are perfectly elastic and have no intermolecular attractive forces. The ideal gas new pressure in the given situation is P = 2.323 atm.

Ideal gas equation is used for the approximation behaviour of the general gases. The ideal gas is defined as:

Given that,

Now, from the ideal gas equation, :

PV=nRT

At constant volume, the pressure of given mass of gas is directly proportional to the temperature, such that:

where,

Now, substituting the values in the above equation:

Therefore, the pressure after raising the temperature of the gas will be 2.323 atm.

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1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

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