The partial pressure of CO2 inside a bottle of soft drink is 4.0 atm at 25°C. The solubility of CO2 is 0.12 mol/L. When the bott
1 answer:
We can solve this problem by using Henry's law.
Henry's law states that the amount of dissolved gas is proportional to its partial pressure.
C is <span>the solubility of a gas.
</span><span>k is Henry's law constant.
</span><span>P is the partial pressure of the gas.
</span>We can calculate the constant from the first piece of information and then use Henry's law to calculate solubility in open drink.
0.12=4k
k=0.03
Now we can calculate the solubility in open drink.
Now we need to convert it to g/L. One mol of CO2 is 44.01<span>g.
</span>The final answer is:
Henry's law states that the amount of dissolved gas is proportional to its partial pressure.
C is <span>the solubility of a gas.
</span><span>k is Henry's law constant.
</span><span>P is the partial pressure of the gas.
</span>We can calculate the constant from the first piece of information and then use Henry's law to calculate solubility in open drink.
0.12=4k
k=0.03
Now we can calculate the solubility in open drink.
Now we need to convert it to g/L. One mol of CO2 is 44.01<span>g.
</span>The final answer is:
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Answer : The molar volume of the gas will be, 44.82 L
Solution :
Using ideal gas equation,
where,
n = number of moles of gas = 1 mole
P = pressure of the gas = 0.5 atm
T = temperature of the gas = 273 K
R = gas constant = 0.0821 Latm/moleK
V = volume of the gas.
Now put all the given values in the above equation, we get the molar volume of the gas.
Therefore, the molar volume of the gas will be, 44.82 L