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A gaseous product of a reaction is collected at 280K and 0.95 atm. Given R = 0.0821L atm what is the molar mass of the gas,
in grams per mole, if 5.49 g of gas occupies 4.92 L? (1 point)

24 g/mol

27 g/mol

0.04 g/mol

133 g/mol

Sagot :

Polyblockidn

Answer:

27 g/mol

Explanation:

We'll use this formula: PV = nRT

P = Pressure (0.95)

V = Volume (4.92)

n = moles (?)

R = Constant (0.0821)

T = Temperature in kelvins (280)

(0.95)(4.92) = n(0.0821)(280)

4.674 = 22.988n

Divide both sides by 22.988

4.674/22.988 = 22.988n/22.988

n = 0.20332347

Or just round it to 0.2

This means are 0.2 moles

Divide the grams by moles

5.49/0.2 = 27.45

Destinylester82idn

Gases Unit Test Honors Chemistry A

1) B. The volume increases to twice its original value.

2) A. volume and temperature directly proportional

pressure and volume inversely proportional

pressure and temperature directly proportional

3) D. Gay-Lussac’s law, by seeing how changes in temperature affect the pressure of the gas

4) B. V1P1/T1=V2P2/T2

5) A. It is a straight line with a positive slope showing that an increase in temperature results in an increase in volume.

6) D. keeping the pressure constant and increasing the temperature

7) A. When temperature is held constant and volume increases, the pressure increases.

8) D. pressure, volume, temperature, number of moles

9) A. volume

10) A. 7.10 L/mol

11) A. 0.105 mol

12) B. 27 g/mol

13) B. the temperature increasing by a factor of 2

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