20 grams of ethane (c2h6) in a 15 l container has a pressure of 1.3 bar. what is the temperature, in oc

The temperature is 42.5 °C

Explanation:

We apply the Law of Ideal Gases to solve this:

P  .  V = n .  R . T

First, we convert the bar into atm, so we make a rule of three.

1.013 bar is 1 atm

1.3 bar is (1.3 . 1) /1.013 = 1.28 atm

1.28atm . 15L = n . 0.082 . T

We must convert the mass to moles ( mass / molar mass)

20 g / 30 g / mol = 0.666 moles

1.28atm . 15L = 0.666 mol . 0.082 . T

(1.28 atm . 15L) / (0.666 mol . 0.082) = T

315.5 K = T

As this is absolute temperature we must convert to °C

315.5 K - 273= 42.5 °C

The temperature is 79.52 °C

Explanation:

Step 1: Data given

Mass of ethane = 20.0  grams

Volume of the gas = 15.0 L

Pressure in the container = 1.3 bar = 1.283 atm

Molar mass of ethane = 30.07 g/mol

Step 2: Calculate moles of ethane

moles ethane = mass ethane / molar mass ethane

Moles ethane = 20.0 grams / 30.07 g/mol

Moles ethane = 0.665 moles

Step 3: Calculate temperature

p*V = n*R*T

⇒ p = the pressure in the container = 1.283 atm

⇒ V = the volume = 15.0 L

⇒ n = the moles of ethane = 0.665 moles

⇒ R = the gas constant = 0.08206 L*atm/mol*K

⇒ T = the temperature = TO BE DETERMINED

T = (p*V)/(n*R)

T = (1.283*15)/(0.665*0.08206)

T = 352.67 K

T = 79.52 °C

The temperature is 79.52 °C

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each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i