55 WHAT units?
(V1/T1) = (V2/T2)
Remember T is in kelvin.
(V1/T1) = (V2/T2)
Remember T is in kelvin.
The formula for the combined gas law is:
(P1 * V1) / T1 = (P2 * V2) / T2
Given:
P1 = P2 (constant pressure)
V1 = 295 ml
T1 = 36 °C (convert to Kelvin by adding 273.15)
T2 = 55 °C (convert to Kelvin by adding 273.15)
V2 = ? (volume at 55 °C)
Let's substitute the values into the equation and solve for V2:
(P1 * V1) / T1 = (P2 * V2) / T2
(P1 * V1 * T2) / (T1 * P2) = V2
Since the pressure is constant, P1 / P2 = 1. Therefore, we can simplify the equation to:
(V1 * T2) / T1 = V2
Now, let's calculate the volume at 55 °C:
V2 = (V1 * T2) / T1
V2 = (295 ml * (55 °C + 273.15 K)) / (36 °C + 273.15 K)
V2 = (295 ml * 328.15 K) / 309.15 K
Using the formula, we can calculate V2:
V2 = 313.28 ml
Therefore, the volume of the argon gas at 55 °C, assuming constant pressure, is 313.28 ml.
The formula for the combined gas law is as follows:
(P₁ * V₁) / (T₁) = (P₂ * V₂) / (T₂)
Where:
P₁ and P₂ are the initial and final pressures, respectively (assuming constant pressure in this case).
V₁ and V₂ are the initial and final volumes, respectively.
T₁ and T₂ are the initial and final temperatures, respectively.
Given that the pressure is constant (so the ratio of P₁ to P₂ is 1), we can simplify the formula to:
(V₁ / T₁) = (V₂ / T₂)
Now let's plug in the values from the problem into the formula:
V₁ = 295 mL
T₁ = 36 °C + 273.15 (convert to Kelvin) = 309.15 K
T₂ = 55 °C + 273.15 (convert to Kelvin) = 328.15 K
Now, we can rearrange the formula to solve for V₂:
V₂ = (V₁ / T₁) * T₂
Substituting the given values into the equation:
V₂ = (295 mL / 309.15 K) * 328.15 K
Calculating this expression will yield the volume (V₂) the gas will occupy at 55 °C assuming constant pressure.