Asealed container contains 0.10 moles of nitrogen gas and 0.20 moles of oxygen gas. if temperature of the mixture is constant, which of the followimg is true
a molecular masses of 2 gases are the same.
b partial pressures of the two gases are same
c average kinetic energies of the two gases are same.

c. The average kinetic energies of the two gases are the same.  

Step-by-step explanation:

A major postulate of the Kinetic Molecular Theory is that the average kinetic energies of all gases are the same at the same temperature.

a. is wrong. N₂ and O₂ are different elements with different molar masses.

b. is wrong. According to Avogadro's Law, the partial pressure varies directly as the number of moles. There are twice as many molecules of O₂ as of N₂, so p(O₂)  = 2p(N₂).

yes

explanation:

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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%