555 mL sample of nitrous oxide at 25 degree celsius is heated to 50 degrees celsius. If the pressure remains constant, what is the final volume?

(V1/T1) = (V2/T2)

Don't forget T must be in kelvin.

Wow... noone ever answered... sorry man..

To find the final volume of the sample of nitrous oxide, we can use the combined gas law equation.

The combined gas law equation is given as:

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

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

From the information given:
Initial volume (V1) = 555 mL
Initial temperature (T1) = 25 degrees Celsius = 25 + 273 = 298 Kelvin
Final temperature (T2) = 50 degrees Celsius = 50 + 273 = 323 Kelvin
Pressure (P1) and Pressure (P2) are constant.

Substituting the given values into the combined gas law equation, we can solve for the final volume (V2):

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

(P1 * 555 mL) / 298 K = (P2 * V2) / 323 K

Since the pressure remains constant, P1 = P2. We can cancel out the pressure terms:

555 mL / 298 K = V2 / 323 K

Cross-multiplying:

(555 mL * 323 K) / 298 K = V2

Simplifying:

600.34 mL = V2

Therefore, the final volume of the sample of nitrous oxide is approximately 600.34 mL.

To determine the final volume of the nitrous oxide, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure (which remains constant)
V = volume
n = number of moles of the gas
R = ideal gas constant
T = temperature (in Kelvin)

First, let's convert the temperatures from degrees Celsius to Kelvin. The temperature in Kelvin is equal to the temperature in Celsius plus 273.15.

Initial temperature = 25°C + 273.15 = 298.15 K
Final temperature = 50°C + 273.15 = 323.15 K

Since the pressure remains constant, we can simplify the equation to:

V1/T1 = V2/T2

Where:
V1 = initial volume (555 mL)
T1 = initial temperature (298.15 K)
V2 = final volume (what we want to find)
T2 = final temperature (323.15 K)

Now we can plug in the values and solve for V2:

V1/T1 = V2/T2

555 mL / 298.15 K = V2 / 323.15 K

Cross-multiplying, we get:

(555 mL) × (323.15 K) = V2 × (298.15 K)

V2 = (555 mL × 323.15 K) / 298.15 K

Calculating this expression gives us the final volume:

V2 ≈ 602.3 mL

Therefore, the final volume of the nitrous oxide when heated to 50 degrees Celsius, assuming constant pressure, is approximately 602.3 mL.