What is the mass of neon that exerts a pressure of 720 mmHg with a temperature of -15.0°C, when the volume of the container is 760 mL?

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What is the mass of neon that exerts a pressure of 720 mmHg with a temperature of -15.0°C, when the volume of the container is 760 mL?

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Answer 1 · 2018-05-13T18:03:05

$Mass of neon \equiv 1.36 \cdot g$ $"Mass of neon"-=1.36*g$

Explanation:

We use the old Ideal Gas equation...

$n = \frac{P V}{R T} = \frac{\frac{720 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t m^{- 1}} \times 760 \cdot m L \times 10^{- 3} \cdot L \cdot m L^{- 1}}{0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 258.15 \cdot K}$ $n=(PV)/(RT)=((720*mm*Hg)/(760*mm*Hg*atm^-1)xx760*mLxx10^-3*L*mL^-1)/(0.0821*(L*atm)/(K*mol)xx258.15*K)$

$= 0.0340 \cdot m o l$ $=0.0340*mol$ ...a mass of .......

$0.034 \cdot m o l \times 40.0 \cdot g \cdot m o l^{- 1} = 1.36 \cdot g$ $0.034*molxx40.0*g*mol^-1=1.36*g$

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What is the mass of neon that exerts a pressure of 720 mmHg with a temperature of -15.0°C, when the volume of the container is 760 mL?

1 Answer

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