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tangare [24]
3 years ago
15

In a study of the conversion of methane to other fuels, a chemical engineer mixes gaseous CH4 and H2O in a 0.32-L flask at 1200

K. At equilibrium the flask contains 0.028 mol of CO, 0.084 mol of H2, and 0.045 mol CH4. What is [H2O] at equilibrium if Kc at this temperature is 0.26
Chemistry
1 answer:
inessss [21]3 years ago
8 0

Answer:

[H2O] = 0.0434 M

Explanation:

Step 1: Data given

Moles CH4 = 0.045 moles

Moles CO = 0.028 moles

Moles H2 = 0.084 moles

Volume = 0.32 L

Temperature = 1200 K

Kc = 0.26

Step 2: The balanced equation

CH4(g) + H2O(g) ⇆ CO(g) + 3H2(g)

Step 3: Calculate molarity at the equilibrium

[CH4] = 0.045 moles / 0.32 L = 0.141 M

[H2O] = ?

[CO] = 0.028 moles / 0.32 L = 0.0875 M

[H2] = 0.084 moles / 0.32 L = 0.263 M

Step 4: Calculate [H2O]

Kc = 0.26 = [CO][H2]³/[CH4][H2O]

0.26 = 0.0875*0.263³ / 0.141*[H2O]

0.26 = 0.0015917516125 / 0.141*[H2O]

0.141*[H2O] = 0.0015917516125 / 0.26 = 0.006122

[H2O] = 0.0434 M

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Nikolay [14]
I assume what you're asking about is, how does the temperature changes when we increase water's mass, according the formula for heat ? 
Well the formula is : Q=m\cdot c\cdot \Delta t (where Q is heat, m is mass, c is specific heat and \Delta t is change in temperature. So according this formula, increasing mass will increase the substance's heat, but won't effect it's temperature since they are not related. Unless,  if you want to keep the substance's heat constant, in that case when you increase it's mass you will have to decrease the temperature
8 0
3 years ago
The pressure on a sample of gas is increased from 1.0 atm to 3.0 atm. If the new volume is 0.52 L, find the original volume.
swat32

Answer: 1.56 ATM

Explanation: if we assume temperature is constant, gas obeys

Boyles law pV= constant. Then p1·V1= p2·V2. And V1 = p2V2/p1

= 3.0 atm·0,52 l / 1.0 atm

3 0
3 years ago
When a skin diver is on the top of the water at 1.03 atm, her lung volume is 3.62L. How will the volume of her lungs change as s
Anon25 [30]

Answer:

–2.23 L

Explanation:

We'll begin by calculating the final volume. This can be obtained as follow:

Initial pressure (P₁) = 1.03 atm

Initial volume (V₁) = 3.62 L

Final pressure (P₂) = 2.68 atm

Final volume (V₂) =?

P₁V₁ = P₂V₂

1.03 × 3.62 = 2.68 × V₂

3.7286 = 2.68 × V₂

Divide both side by 2.68

V₂ = 3.7286 / 2.68

V₂ = 1.39 L

Finally, we shall determine the change in volume. This can be obtained as follow:

Initial volume (V₁) = 3.62 L

Final volume (V₂) = 1.39 L

Change in volume (ΔV) =?

ΔV = V₂ – V₁

ΔV = 1.39 – 3.62

ΔV = –2.23 L

Thus, the change in the volume of her lung is –2.23 L.

NOTE: The negative sign indicate that the volume of her lung reduced as she goes below the surface!

3 0
2 years ago
A gas has density 2.41 g/liter at 25°C and 770 mm Hg. Calculate it's molecular mass (R = 0.0821 L atm.mol-1K-1 ​
Evgesh-ka [11]

Answer:

Explanation:

Given : Density - 2.41 g/liter  

Temperature - 25° C  

Pressure : 770 mm Hg  

R = 0.0821 L atm mol-¹K-¹

 

Find : Molecular mass of gas

Solution : Ideal gas equation with respect to density will be : PM = dRT. In the formula, P is pressure, M is molecular mass, d is density, R is gas constant and T is temperature.

Keeping the values in equation-  

Pressure : 770 mm Hg = 1 atm  

Temperature : 273 + 25 = 298 K

 

M = dRT/P  

M = (2.41*0.0821*298)/1  

M = 58.96 gram/mol

Thus, the molecular mass of gas is 58.96 gram/mol.

8 0
3 years ago
Electrons.<br> The carbon atom has a total of
Lunna [17]

Answer:

Six electrons.

Explanation:

A carbon atom has six protons, so it must have six electrons.

6 0
3 years ago
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