Question

A sample of gas occupies 100ml at 25 degree celsius. What volume would the gas occupy at 32 degree celsius if the pressure remains constant

Answer 1

(V1/T1) = (V2/T2)

Answer 2

[AI-generated answer — Step-by-Step Bot]

To solve this problem, we can use the combined gas law formula:

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

Where:
P1 = initial pressure (constant)
V1 = initial volume = 100 ml
T1 = initial temperature = 25 °C (convert to Kelvin, T1 = 25 + 273.15)
T2 = final temperature = 32 °C (convert to Kelvin, T2 = 32 + 273.15)
V2 = final volume (unknown)

First, let's convert the temperatures to Kelvin:
T1 = 25 + 273.15 = 298.15 K
T2 = 32 + 273.15 = 305.15 K

Now we can substitute these values into the formula:

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

Since the pressure (P1) is constant, it cancels out:

(V1) / (T1) = (V2) / (T2)

Now plug in the known values:
(100 ml) / (298.15 K) = (V2) / (305.15 K)

To find V2, cross multiply and solve for V2:

V2 = (100 ml) * (305.15 K) / (298.15 K)
V2 ≈ 102.75 ml

Therefore, the gas would occupy approximately 102.75 ml at 32 degrees Celsius if the pressure remains constant.

Answer 3

[AI-generated answer — Explain Bot]

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 in Kelvin.

First, we need to convert the temperatures from Celsius to Kelvin.

25 degrees Celsius + 273.15 = 298.15 Kelvin
32 degrees Celsius + 273.15 = 305.15 Kelvin

Since the pressure remains constant, P1 = P2. Therefore, we can rewrite the ideal gas law equation as:

V1/T1 = V2/T2

Now, substitute the given values into the equation:

V1 = 100 ml
T1 = 298.15 K
T2 = 305.15 K

V2 = (V1 * T2) / T1

V2 = (100 ml * 305.15 K) / 298.15 K

V2 = 102.43 ml

Therefore, the gas would occupy approximately 102.43 ml at 32 degrees Celsius, assuming the pressure remains constant.