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KatRina [158]
1 year ago
10

A sample of carbon dioxide occupies 200 L at 22°C and 1.0 atm. At what temperature will

Chemistry
1 answer:
xxMikexx [17]1 year ago
3 0

Answer:

1328 K or 1055 °C

Explanation:

To find the new temperature, you need to use the Combined Gas Law:

P₁V₁ / T₁ = P₂V₂ / T₂

In this equation, "P₁", "V₁", and "T₁" represent the initial pressure, volume, and temperature. "P₂", "V₂", and "T₂" represent the final pressure, volume, and temperature. After converting the temperature (T₁) from Celsius to Kelvin, you can plug the values into the equation and simplify.

P₁ = 1.0 atm                                                P₂ = 0.90 atm

V₁ = 200 L                                                  V₂ = 1000 L

T₁ = 22 °C + 273.15 = 295.15 K                 T₂ = ? K

P₁V₁ / T₁ = P₂V₂ / T₂

(1.0 atm)(200 L) / 295.15 K = (0.90 atm)(1000 L) / T₂

0.6776 = (0.90 atm)(1000 L) / T₂

(0.6776) x T₂ = (0.90 atm)(1000 L)

(0.6776) x T₂ = 900

T₂ = 1328 K

T₂ = 1055 °C

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Answer please and thank you
Alex73 [517]

Answer:

Option B. 30 KJ.

Explanation:

The following data were obtained from the question:

Temperature (T) = 5000 K

Enthalpy change (ΔH) = – 220 kJ/mol

Change in entropy (ΔS) = – 0.05 KJ/mol•K

Gibbs free energy (ΔG) =...?

The Gibbs free energy, ΔG can be obtained by using the following equation as illustrated below:

ΔG = ΔH – TΔS

ΔG = – 220 – (5000 x – 0.05)

ΔG = – 220 – (– 250)

ΔG = – 220 + 250

ΔG = 30 KJ

Therefore, the Gibbs free energy, ΔG is 30 KJ.

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3 years ago
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8 0
3 years ago
A 2.0 L container of nitrogen gas had a pressure of 3.2 atm. What volume would be necessary to decrease the pressure to 1.0 atm
beks73 [17]

Answer:

6.4 L

Explanation:

When all other variables are held constant, you can use Boyle's Law to find the missing volume:

P₁V₁ = P₂V₂

In this equation, "P₁" and "V₁" represent the initial pressure and volume. "P₂" and "V₂" represent the final pressure and volume. You can find the theoretical volume by plugging the given values into the equation and simplifying.

P₁ = 3.2 atm                      P₂ = 1.0 atm

V₁ = 2.0 L                          V₂ = ? L

P₁V₁ = P₂V₂                                                    <----- Boyle's Law

(3.2 atm)(2.0 L) = (1.0 atm)V₂                        <----- Insert values

6.4 = (1.0 atm)V₂                                           <----- Simplify left side

6.4 = V₂                                                        <----- Divide both sides by 1.0

6 0
2 years ago
A steel tank contains carbon dioxide at a pressure of 13.0 atm when the temperature is 34oC. What will be the internal gas press
morpeh [17]

Answer:

D. 15.8atm

Explanation:

Given parameters:

Initial pressure = 13atm

Initial temperature  = 34°C = 34 + 273  = 307K

Final temperature  = 100°C = 100 + 273  = 373K

Unknown:

Final pressure  = ?

Solution:

To solve this problem, we apply a derivation of the combined gas law taking the volume as a constant.

The expression is shown mathematically below;

        \frac{P_{1} }{T_{1} }   = \frac{P_{2} }{T_{2} }

P and T pressure and temperature values

1 and 2 are initial and final states

 Insert the parameters and solve for T₂;

    \frac{13}{307}   = \frac{P_{2} }{373}  

        P₂  = 15.8atm

4 0
3 years ago
A bedroom has a volume of 118 m3 What is its volume in km3?
ruslelena [56]
I believe the problem is just simply asking for us to convert the value from one unit to the other. This case from m^3 to km^3. From the SI units, we know 1 km is equal to 1000 m. We do as follows:

118 m^3 ( 1 km / 1000 m )^3 = 1.18 x 10^-7 km^3
5 0
3 years ago
Read 2 more answers
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