A 2.9 L sample of gas has a pressure of 5 atm and a temperature of 50 °C. What will be the new temperature in Kelvin if the volume is decreased to 2.4 L and the pressure decreased to 3 atm? Round to the nearest whole number. Don't forget the units.

P1V1/T1 = P2V2/T2

P1 = 5 atm, V1 = 2.9L, T1 = 273+50 = 323K

P2 = 3 atm, V2 = 2.4L, T2 = ?

5*2.9/323 = 3*2.4/T2

T2 = 3*2.4*323/5*2.9

= 160.4K

It’s right just the steps are not clear

Well, well, well, it seems we have a temperature conversion problem here! Let's clown around and solve it, shall we?

To convert Celsius to Kelvin, all we have to do is add 273.15 to our temperature. So, first things first, let's convert that initial temperature of 50 °C into Kelvin.

50 °C + 273.15 = 323.15 K

Now that we have the initial temperature in Kelvin, let's move on to the next act – calculating the final temperature.

According to the Gay-Lussac's Law, when the volume and pressure of a gas decrease or increase, the temperature changes in the same way. So, we can use the formula:

(initial pressure x initial volume) / initial temperature = (final pressure x final volume) / final temperature

Plugging in our values:

(5 atm x 2.9 L) / 323.15 K = (3 atm x 2.4 L) / final temperature

Simplifying:

14.5 / 323.15 = 7.2 / final temperature

Now, let's solve this little equation for the unknown final temperature:

14.5 x final temperature = 7.2 x 323.15

final temperature = (7.2 x 323.15) / 14.5

final temperature ≈ 160.32 K

Ta-da! The new temperature, when the volume is decreased to 2.4 L and the pressure is decreased to 3 atm, will be approximately 160 K.

Hope that brought a little smile to your face!

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

(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, T1 is the initial temperature, and T2 is the final temperature.

Let's plug in the given values into the formula and solve for T2:

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

(5 atm * 2.9 L) / (50 °C + 273.15) = (3 atm * 2.4 L) / T2

(14.5 L atm) / (323.15 K) = (7.2 L atm) / T2

Cross-multiply to get:

14.5 L atm * T2 = 7.2 L atm * (323.15 K)

Divide both sides by 14.5 L atm:

T2 = (7.2 L atm * 323.15 K) / 14.5 L atm

T2 = 160.68 K

Rounding to the nearest whole number, the new temperature in Kelvin is approximately 161 K.

So, the answer is 161 K.

(P1V1/T1) = (P2V2/T2)

Wrong