The pressure of a fixed quantity of an ideal gas was held constant. The initial volume was 8.00 cubic meters and the final volume was 2.50 cubic meters. What was the final temperature in kelvins if the initial temerature was 188 degrees fahrenheit...

Please walk me through your steps instead of just suggesting a formula..

Thank you

188F=359.82= 360 K

V1/T1 =V2/T2

T2 =T1•V2/V1 =360•2.5/8 = 112.5 K

thank you

To solve this problem, we can use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

First, let's convert the initial temperature from Fahrenheit to Kelvin. To do this, we'll use the formula: T(°C) = (T(°F) - 32) * 5/9 and T(K) = T(°C) + 273.15.

Converting 188 degrees Fahrenheit to Celsius:
T(°C) = (188 - 32) * 5/9 = 100°C

Now converting 100 degrees Celsius to Kelvin:
T(K) = 100°C + 273.15 = 373.15 K

Next, we'll use the given information that the pressure was constant and the initial and final volumes were 8.00 cubic meters and 2.50 cubic meters, respectively.

Since the pressure is constant, we can rewrite the ideal gas law as follows:

(V1 / T1) = (V2 / T2)

Substituting the known values:
(8.00 m³ / 373.15 K) = (2.50 m³ / T2)

We can solve for T2 by cross-multiplying:
8.00 m³ * T2 = 2.50 m³ * 373.15 K

Now divide both sides by 2.50 m³ to isolate T2:
T2 = (2.50 m³ * 373.15 K) / 8.00 m³

Simplifying, we get:
T2 = 116.97 K

Therefore, the final temperature is approximately 116.97 Kelvin.