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ELEN [110]
3 years ago
6

A student uses 0. 0821 LĂ˘â‚¬Ë atm/mol Ă˘â‚¬Ë K as the value of the gas constant. What is most likely true about the variables i

n the ideal gas law? P has the units of liters Ă˘â‚¬Ë atmospheres, and T has the units of kelvin. P has the units of liters Ă˘â‚¬Ë atmospheres, and T has the units of degrees Celsius. V has the units of liters, and T has the units of kelvin. V has the units of liters, and T has the units of degrees Celsius.
Chemistry
1 answer:
xz_007 [3.2K]3 years ago
6 0

The variables in the ideal gas constant has V as the unit of liters and T has the unit of Kelvin. Thus, option C is correct.

The gas constant in an ideal gas equation has been the value of the energy absorbed by 1 mole of an ideal gas at standard temperature and pressure.

The value of R has been dependent on the units of volume, temperature and pressure of the ideal gas.

The given value of R has been 0.0821 L.atm/mol.K

The unit in gas constant has been L (Liter) for volume (V).

The unit of pressure (P) has been atm.

The unit of temperature (T) has been Kelvin  (K).

Thus the gas law constant used by student has V has the unit of liters and T has the unit of Kelvin. Thus, option C is correct.

For more information about the gas constant, refer to the link:

brainly.com/question/24814070

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Nitrogen dioxide (NO2) cannot be obtained in a pure form in the gas phase because it exists as a mixture of NO2 and N2O4. At 16°
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Answer:

PNO₂ = 0.49 atm

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Explanation:

Let's begin with the equation of ideal gas, and derivate from it an equation that  involves the density (ρ = m/V).

PV = nRT

n = m/M (m is the mass, and M the molar mass)

PV = \frac{m}{M}RT

PxM = \frac{m}{V}RT

PxM = ρRT

ρ = PxM/RT

With the density of the gas mixture, we can calculate the average of molar mass (Mavg), with the constant of the gases R = 0.082 atm.L/mol.K, and T = 16 + 273 = 289 K

2.7 = \frac{0.94xMavg}{0.082x289}

0.94Mavg = 63.9846

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Mavg = M_{NO2}y_{NO2} + M_{N2O4}y_{N2O4}

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68.0687 - 92 = 46y_{NO2} - 92y_{NO2}

46y_{NO2} = 23.9313

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The partial pressure is the molar fraction multiplied by the total pressure so:

PNO₂ = 0.52x0.94 = 0.49 atm

PN₂O₄ = 0.48x0.94 = 0.45 atm

8 0
3 years ago
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