Harvey kept a balloon with a volume of 348 milliliters at 25.0˚C inside a freezer for a night. When he took it out, its new volume was 322 milliliters, but its pressure was the same. If the final temperature of the balloon is the same as the freezer’s, what is the temperature of the freezer?
To solve this problem, we would need to use the concept of the General Gas Law that states the product of the initial pressure, volume, and temperature of a gas is equal to the product of its final pressure, volume, and temperature. This is mathematically represented as: P1*V1/T1 = P2*V2/T2, where:
- P1 and P2 are the initial and final pressures,
- V1 and V2 are the initial and final volumes, and
- T1 and T2 are the initial and final temperatures.
In this problem, the balloon's pressure remained constant, so we can simplify the gas law equation by removing P1 and P2. This gives us the equation: V1/T1 = V2/T2.
The temperatures in this simplified equation need to be in Kelvins (K), not degrees Celsius (˚C). To convert from ˚C to K, we would add 273.15. So, the initial temperature T1 of the balloon is 25.0˚C + 273.15 = 298.15 K.
Substitute the known values into the simplified gas law to find the final temperature T2 (which would be the freezer's temperature). We now have: 348 mL / 298.15 K = 322 mL / T2.
To solve for T2, we would cross-multiply and divide: T2 = 322 mL * 298.15 K / 348 mL. When you do this calculation, you get T2 ≈ 275.36 K. Therefore, the freezer's temperature is approximately 275.36 K.
Based on Charles law, which states that the volume of a given mass of a ideal gas is directly proportional to the temperature provided that the pressure is constant. It can be applied using the below formula
Answer: b. Fiona is correct because the diagram shows two individual simple machines.
Explanation:
A mechanical device using which we can change the direction or magnitude of force applied is known as simple machine.
For example, in the given diagram there are two individual simple machines.
The machine helps in changing the direction or magnitude of force applied by the man. As a result, it becomes easy for him to carry different things easily from one place to another.
Thus, we can conclude that the statement Fiona is correct because the diagram shows two individual simple machines, is correct.
A positive reaction for Molisch's test is given by almost all carbohydrates (exceptions include tetroses & trioses). It can be noted that even some glycoproteins and nucleic acids give positive results for this test (since they tend to undergo hydrolysis when exposed to strong mineral acids and form monosaccharides).
Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N2 gas at 328K and 0.884 atm is 26.07 L.
An ideal gas is a theoretical gas that is considered to be composed of point particles that move randomly and do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.
The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:
P×V = n×R×T
where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas. The universal constant of ideal gases R has the same value for all gaseous substances.
Explanation:
In this case, you know:
P= 0.884 atm
V= ?
n= 0.857 moles (where 28 g/mole is the molar mass of N₂, that is, the amount of mass that the substance contains in one mole.)
R=0.082
T= 328 K
Replacing in the ideal gas law:
0.884 atm×V= 0.857 moles× 0.082 ×328 K
Solving:
V= 26.07 L
The volume of a container that contains 24.0 grams of N2 gas at 328K and 0.884 atm is 26.07 L.
Answer: 25 g
Explanation: Given:
Original amount (N₀) = 100 g
Number of half-lives (n) = 11460/5730 = 2
Amount remaining (N) = ?
N = 1/2ⁿ × N₀
N = 1/2^2 × 100
N = 0.25 × 100
N = 25 g
Answer: 7.8125 g
Explanation: Given:
Original amount (N₀) = 500 g
Number of half-lives (n) = 9612/1602 = 6
Amount remaining (N) = ?
N = 1/2ⁿ × N₀
N = 1/2^6 × 500
N = 0.015625 × 500
N = 7.8125 g
2
17 823
rating
= 348 mL
= 
= 322 mL
0.857 moles (where 28 g/mole is the molar mass of N₂, that is, the amount of mass that the substance contains in one mole.)
×328 K
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