a gas has a volumn of 36.0 L and a pressure of 750 torr when the temperature is 10 degrees celsius. what is the pressure if the volume changes to 78 degrees celsius if the amount of gas stays the same?
You need to read your post and note it doesn't make any sense. "Volume changing to 78 degrees celsius"?
Use (P1V1/T1) = (P2V2/T2)
a gas has a volumn of 36.0 L and a pressure of 750 torr when the temperature is 10 degrees celsius. what is the pressure if the volume changes to 78 degrees celsius if the amount of gas stays the same?
To find the new pressure of the gas when the volume changes from 36.0 L to 78.0 L, and the temperature changes from 10 degrees Celsius to 78 degrees Celsius, we can use the combined gas law equation:
P₁V₁/T₁ = P₂V₂/T₂
Where:
P₁ = Initial pressure
V₁ = Initial volume
T₁ = Initial temperature (in Kelvin)
P₂ = Final pressure (what we need to find)
V₂ = Final volume
T₂ = Final temperature (in Kelvin)
Let's begin by converting the initial and final temperatures from Celsius to Kelvin:
T₁ = 10 + 273.15 = 283.15 K
T₂ = 78 + 273.15 = 351.15 K
Now, we can plug in the given values into the combined gas law equation:
(P₁ * V₁) / T₁ = (P₂ * V₂) / T₂
Let's substitute the values and solve for P₂:
(750 torr * 36.0 L) / 283.15 K = (P₂ * 78.0 L) / 351.15 K
To find P₂, isolate it by cross-multiplying and solving for P₂:
(750 torr * 36.0 L * 351.15 K) = (283.15 K * P₂ * 78.0 L)
P₂ = (750 torr * 36.0 L * 351.15 K) / (283.15 K * 78.0 L)
Calculating this expression should give us the new pressure (P₂).
To solve this problem, we can use the Combined Gas Law, which relates the initial and final conditions of pressure, volume, and temperature of a gas.
The formula for the Combined Gas Law is:
(P1 * V1) / T1 = (P2 * V2) / T2
Where:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure (what we need to find)
V2 = final volume
T2 = final temperature
Given:
P1 = 750 torr
V1 = 36.0 L
T1 = 10 degrees Celsius
V2 = unknown
T2 = 78 degrees Celsius
First, we need to adjust the temperatures to Kelvin since the gas law requires temperatures in Kelvin. The formula to convert Celsius to Kelvin is:
T(Kelvin) = T(Celsius) + 273.15
So, for T1:
T1(Kelvin) = 10 + 273.15 = 283.15 K
And for T2:
T2(Kelvin) = 78 + 273.15 = 351.15 K
Now we can substitute the values into the Combined Gas Law:
(P1 * V1) / T1 = (P2 * V2) / T2
Plugging in the known values:
(750*36) / 283.15 = (P2*V2) / 351.15
Next, we solve for P2 by rearranging the equation:
P2 = (750 * 36 * 351.15) / (283.15 * V2)
Finally, we can substitute the given value of V2 (78.0 L) into the equation and solve for P2:
P2 = (750 * 36 * 351.15) / (283.15 * 78.0)
Calculating this will give you the value for P2.