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vodka [1.7K]
2 years ago
13

A 642 mL sample of oxygen gas at 23.5°C and 795 mm Hg, is heated to 31.7°C and the volume of the gas expands to 957 mL. What is

the new pressure in atm?
Chemistry
1 answer:
malfutka [58]2 years ago
4 0
Let's assume that O₂ is an ideal gas.

We can use combined gas law,
 PV/T = k (constant)

Where, P is the pressure of the gas, V is volume of the gas and T is the temperature of the gas in Kelvin.

For two situations, we can use that as,
P₁V₁/T₁= P₂V₂/T₂

P₁ = <span>795 mm Hg
</span>V₁ = <span> 642 mL
</span>T₁ = (273 + 23.5) K = 296.5 K
P₂ = ?
V₂ = <span>957 mL
</span>T₂ = (273 + 31.7) K = 304.7 K

By applying the formula,

795 mm Hg x 642 mL / 296.5 K = P₂ x 957 mL / 304.7 K
                                              P₂ = 548.07 mm Hg
                                              P₂ = 548 mm Hg
760 mmHg = 1 atm
548 mm Hg = 1 atm x (548 mmHg / 760 mmHg) = 0.721 atm

Pressure of gas = 
548 mm Hg = 0.721 atm
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The addition of NaOH to water would result in which of the following?
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Give the number of lone pairs around the central atom and the molecular geometry of XeF4.A)0 lone pairs, tetrahedralB)1 lone pai
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3 years ago
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Explanation:

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So,     P = \frac{40 torr}{760 torr} \times 1 atm

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Putting the given values into the above equation to calculate the value of n as follows.

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It is known that molar mass of ethanol is 46 g/mol. Hence, calculate its mass as follows.

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                 6.85 \times 10^{-3} = \frac{mass}{46 g/mol}  

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Thus, we can conclude that the mass of liquid ethanol is 0.315 g.

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