The pressure of the CO₂ = 0.995 atm
<h3>Further explanation</h3>
The complete question
<em>A student is doing experiments with CO2(g). Originally, a sample of gas is in a rigid container at 299K and 0.70 atm. The student increases the temperature of the CO2(g) in the container to 425K.</em>
<em>Calculate the pressure of the CO₂ (g) in the container at 425 K.</em>
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<em />
Gay Lussac's Law
When the volume is not changed, the gas pressure is proportional to its absolute temperature

P₁=0.7 atm
T₁=299 K
T₂=425 K

<em />
The amount of force is what this is for
Explanation:
Formula to calculate osmotic pressure is as follows.
Osmotic pressure = concentration × gas constant × temperature( in K)
Temperature =
= (25 + 273) K
= 298.15 K
Osmotic pressure = 531 mm Hg or 0.698 atm (as 1 mm Hg = 0.00131)
Putting the given values into the above formula as follows.
0.698 = 
C = 0.0285
This also means that,
= 0.0285
So, moles = 0.0285 × volume (in L)
= 0.0285 × 0.100
= 
Now, let us assume that mass of
= x grams
And, mass of
= (1.00 - x)
So, moles of
=
Now, moles of
=
=
= x = 0.346
Therefore, we can conclude that amount of
present is 0.346 g and amount of
present is (1 - 0.346) g = 0.654 g.
Answer
Sounds travel slowest in gasses so it would be air