I am not quite sure how to do this problem, it doesn't seem to fit into any of my given equations:

A gas has a volume of 35.5L and a pressure of 765mmHg at standard temperature. If the same sample is placed in a 56.0L container and the pressure is measured at 0.92atm, calculate the temperature of the sample in this new container.

I have already converted the .92atm to 699.2mmHg but i don't know where else to go from here. PLEASE HELP!!!

P1V1/T1 = P2V2/T2

(765mmHg)(35.5L)/273K = (699.2mmHg)(56.0L)/T2

Solve for T2 to get the final temperature in degrees Kelvin. If you need degrees Celsius, use:
C = K - 273

How did you find that value for K?

Standard T is 273 Kelvin (0 degrees C).

Standard pressure is 1 atmosphere or 760 mm Hg.

To solve this problem, you can use the ideal gas law, which relates the pressure, volume, and temperature of a gas. The ideal gas law is expressed as:

PV = nRT

Where:
P is the pressure of the gas (in atmospheres or mmHg)
V is the volume of the gas (in liters)
n is the number of moles of gas
R is the ideal gas constant (0.0821 L·atm/(mol·K) or 62.36 L·mmHg/(mol·K))
T is the temperature in Kelvin (K)

In this problem, you are given the initial pressure (765 mmHg), the initial volume (35.5 L), and the final volume (56.0 L). You need to find the final temperature.

To solve for the final temperature, you can use the equation:

P1V1/T1 = P2V2/T2

Now let's plug in the given values:

P1 = 765 mmHg
V1 = 35.5 L
T1 = ?

P2 = 699.2 mmHg
V2 = 56.0 L
T2 = ?

First, let's convert the initial pressure to atm:

P1 = 765 mmHg / 760 mmHg/atm ≈ 1.00789 atm

Next, let's convert the final pressure to atm:

P2 = 699.2 mmHg / 760 mmHg/atm ≈ 0.91958 atm

Now we can set up the equation:

P1V1/T1 = P2V2/T2

(1.00789 atm)(35.5 L)/T1 = (0.91958 atm)(56.0 L)/T2

Now, we solve for T2:

T2 = [(0.91958 atm)(56.0 L)T1] / [(1.00789 atm)(35.5 L)]

There are a few variables left, but we can simplify the equation further.

Notice that V1 and V2 appear in the equation only as a ratio (V1/V2). So, let's substitute this ratio with a variable, x:

V1/V2 = 35.5 L / 56.0 L = x

Now, we can rewrite the equation using x:

T2 = [(0.91958 atm)(56.0 L)T1] / [(1.00789 atm)(35.5 L)x]

Now, we have a linear equation with only two variables, T1 and x. We can further rearrange it to solve for T2:

T2 = (56.0/35.5) * (T1/x) * (0.91958/1.00789)

T2 = 1.57746 * (T1/x) * 0.91354

T2 = (1.57746 * 0.91354) * (T1/x)

T2 = 1.43898 * (T1/x)

Now, you can substitute the given value of x (= V1/V2 = 35.5 L / 56.0 L) into the equation:

T2 = 1.43898 * (T1 / (35.5 L / 56.0 L))

T2 = 1.43898 * (T1 * (56.0 L / 35.5 L))

T2 = 1.43898 * (1.57746 * T1)

T2 = 2.26818 * T1

Finally, you can solve for T2 by rearranging the equation:

T2 = (0.91958 atm)(56.0 L)(299.2 K) / [(1.00789 atm)(35.5 L)]

T2 ≈ 462.47 K

Therefore, the temperature of the gas in the new container is approximately 462.47 Kelvin (K).