Carbonated drinks in cans have a small amount of space above the liquid level inside the can known as the “headspace.” What woul
2 answers:
Answer: The temperature remains constant.
Explanation: Carbonated drinks have carbon dioxide mixed in water at high pressures as the solubility increases with high pressure. So, when we open the can at atmospheric pressure, the pressure will decrease and the solubility also decreases which will result in the increase in volume.
This phenomena is explained by Boyle's Law:
This law states that pressure is inversely proportional to the volume of the gas at constant temperature and number of moles.
Increase in pressure will result in decrease of volume and vice versa.
So, when we open the can of a carbonated drink, the pressure and volume changes but the temperature remains constant.
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<u>Answer:</u> The mass of methane burned is 12.4 grams.
<u>Explanation:</u>
The chemical equation for the combustion of methane follows:
The equation for the enthalpy change of the above reaction is:
We are given:
Putting values in above equation, we get:
The heat calculated above is the heat released for 1 mole of methane.
The process involved in this problem are:
Now, we calculate the amount of heat released or absorbed in all the processes.
- <u>For process 1:</u>
where,
= amount of heat absorbed = ?
m = mass of water = 242.0 g
= specific heat of water = 4.18 J/g°C
= final temperature =
= initial temperature =
Putting all the values in above equation, we get:
- <u>For process 2:</u>
where,
= amount of heat absorbed = ?
m = mass of water or steam = 242 g
= latent heat of vaporization = 2257 J/g
Putting all the values in above equation, we get:
- <u>For process 3:</u>
where,
= amount of heat absorbed = ?
m = mass of steam = 242.0 g
= specific heat of steam = 2.08 J/g°C
= final temperature =
= initial temperature =
Putting all the values in above equation, we get:
Total heat required =
- To calculate the number of moles of methane, we apply unitary method:
When 802.34 kJ of heat is needed, the amount of methane combusted is 1 mole
So, when 621.552 kJ of heat is needed, the amount of methane combusted will be =
To calculate the number of moles, we use the equation:
Molar mass of methane = 16 g/mol
Moles of methane = 0.775 moles
Putting values in above equation, we get:
Hence, the mass of methane burned is 12.4 grams.