A gas has a volume of 4.25 m3 at a temperature of 95.0°C and a pressure of 1.05 atm. What temperature will the gas have at a pressure of 1.58 atm and a volume of 2.46 m3?

A. 356°C
B. 82.7°C
C. 47.5°C
D. 321°C

You know PV=kT

That means that PV/T = k is constant

So, you want T (in °C) such that

1.58*2.46/(T+273.15) = 1.05*4.25/(95.0+273.15)

T = 47.5°C

Well, well, well, looks like we've got ourselves a gas problem! But don't worry, I'll use my comedy skills to crack this one for you.

Let's call the initial temperature T1, the final temperature T2, the initial pressure P1, the final pressure P2, the initial volume V1, and the final volume V2.

According to the magical land of science, the relationship between pressure, volume, and temperature is governed by the equation P1 * V1 / T1 = P2 * V2 / T2.

Now, plug in the values we have from the question:

P1 = 1.05 atm
V1 = 4.25 m³
T1 = 95.0°C

P2 = 1.58 atm
V2 = 2.46 m³

We need to solve for T2. So let's do some mathematical acrobatics and rearrange the equation:

T2 = (P2 * V2 * T1) / (P1 * V1)

Put in the numbers and let the laughter begin!

T2 = (1.58 atm * 2.46 m³ * 95.0°C) / (1.05 atm * 4.25 m³)

After doing the math (and a few silly dance moves), we find that T2 is approximately 82.7°C.

So the answer, my friend, is B. 82.7°C. I hope my clownish antics made this gas problem a bit more entertaining for you!

To solve this problem, we can use the ideal gas law equation, which states:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature

Since we are dealing with the same gas, the number of moles and the ideal gas constant will remain constant. Therefore, we can rewrite the equation as:

P1V1/T1 = P2V2/T2

Where:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure
V2 = final volume
T2 = final temperature

Let's plug in the given values:

P1 = 1.05 atm
V1 = 4.25 m^3
T1 = 95.0°C (remember to convert to Kelvin by adding 273.15)
P2 = 1.58 atm
V2 = 2.46 m^3
T2 = ?

Now we can rearrange the equation and solve for T2:

T2 = (P2 * V2 * T1) / (P1 * V1)

Calculating the value:

T2 = (1.58 atm * 2.46 m^3 * (95.0°C + 273.15 K)) / (1.05 atm * 4.25 m^3)

T2 ≈ 356 K

Since the temperature needs to be given in Celsius, we subtract 273.15:

T2 ≈ 356 - 273.15 ≈ 82.85°C

Rounded to the nearest tenth, the answer is approximately 82.7°C.

Therefore, the correct answer is B. 82.7°C.

To solve this problem, we can use the combined gas law, which relates the pressure, volume, and temperature of a gas.

The formula for the combined gas law is:

(P1 * V1) / T1 = (P2 * V2) / T2

where P1 and P2 are the initial and final pressures of the gas, V1 and V2 are the initial and final volumes of the gas, and T1 and T2 are the initial and final temperatures of the gas.

Let's substitute the given values into the formula:

(P1 * V1) / T1 = (P2 * V2) / T2

(1.05 atm * 4.25 m^3) / (95.0°C) = (1.58 atm * 2.46 m^3) / T2

Now solve for T2:

T2 = (1.58 atm * 2.46 m^3 * 95.0°C) / (1.05 atm * 4.25 m^3)

T2 = (3.879 atm*m^3*°C) / (4.4625 atm*m^3)

T2 = 0.8682 °C

Therefore, the temperature of the gas at a pressure of 1.58 atm and a volume of 2.46 m^3 is approximately 0.8682°C.

None of the options provided match this calculated value, so there may be an error in the question or the answer choices.