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dem82 [27]
3 years ago
5

An air-filled balloon has a volume of 225 L at 0.940 atm and 25 °C. Soon after, the pressure changes to 0.990 atm and the temper

ature changes to 0 °C. What is the new volume of the balloon?
Chemistry
1 answer:
lorasvet [3.4K]3 years ago
7 0

Answer:

The right choice is  V₂ = 195.7 L

Explanation:

  • We can use the general law of ideal gas: PV = nRT.

where, P is the pressure of the gas in atm.

V: is the volume of the gas in L.

n: is the no. of moles of the gas in mol.

R:  is the general gas constant,

T: is the temperature of the gas in K.

If n is constant, and have different values of P, V and T:

(P₁*V₁) / T₁ = (P₂ * V₂) / T₂

Knowing that:  

V₁  =  225 L  ,         P₁ = 0.940 atm

T₁ = 25  °C + 273  =  298 K

V₂  =  ??? L,           P₂ = 0.990 atm  

T₂ = 0 °C + 273  =  273 K

applying in the above equation

(P ₁* V₁) / T₁ = (P₂ * V₂) / T₂

(0.940 atm * 225 L) / 298 K= (0.990 atm  * V₂) / 273 K

V₂ = (0.940 atm * 225 L * 273 K) / (298 K * 0.990 atm)

V₂ = 195.7 L

So, the right choice is:

V₂ = 195.7 L

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Explanation:

In the elements of the periodic table, the atomic mass = molar mass. <u>Ex:</u> Atomic mass of Carbon is 12.01 amu which means molar mass of Carbon is also 12.01g/mol.

In order to find the # of moles in a 12 g sample of NiC-12, we will need to multiply the number of each atom by its molar mass and then add the masses of both Nickel and C-12 found in the periodic table:

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Since there's just one atom of both Carbon and Nickel, we just add up the masses to find the molar mass of the whole compound of NiC-12.

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3 years ago
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