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3 years ago

The density of nitric oxide (NO) gas at 0.866 atm and 46.2 degrees celcius is ____ g/L

Chemistry

1 answer:

Artyom0805 [142]3 years ago

8 0

Answer:

d = 0.992 g/L

Explanation:

Data Given:

Pressure of nitric oxide (NO) = 0.866 atm

Temperature of a gas = 46.2° C

Convert the temperature to kelvin = 46.2° C + 273

temperature in kelvin = 319.2 K

density of nitric oxide (NO) = ?

Solution:

Density of a gas can be calculated by

d = PM /RT

Where

d = density

P = Pressure

M = molar mass of gas

R = ideal gas constant = 0.0821 L atm mol⁻¹ K⁻¹

T = temperature

So,

Molar mass of NO = 30 g/mol

Put values in the formula:

d = PM /RT

d = 0.866 atm × 30 g/mol / 0.0821 L atm mol⁻¹ K⁻¹ × 319.2 K

d = 25.98 atm. g/mol / 26.2 L atm mol⁻¹

d = 0.992 g/L

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2 years ago

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Answer:

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You want to study two different states, an initial state and a final state. You have a gas that is at a pressure P1 and at a temperature T1 at the beginning of the experiment. By varying the temperature to a new value T2, then the pressure will change to P2, and the following will be fulfilled:

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