A gas sample has a pressure of 2.90 atm when the temperature is - 14 deg C What is the final pressure, in atmospheres, when the temperature is 53 deg C with no change in the volume or amount of xpress your answer with the appropriate units
To solve this problem, we can use the combined gas law equation:
(P1/T1) = (P2/T2)
where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature.
Plugging in the given values:
P1 = 2.90 atm
T1 = -14°C = 259 K (converting to Kelvin)
T2 = 53°C = 326 K (converting to Kelvin)
(P1/T1) = (P2/T2)
(2.90 atm / 259 K) = (P2 / 326 K)
Solving for P2:
P2 = (2.90 atm / 259 K) * 326 K
P2 = 3.64 atm
Therefore, the final pressure when the temperature is 53°C is 3.64 atm.
To solve this problem, we can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature when pressure and the amount of gas are held constant. Since there is no change in volume or amount of gas in this problem, we can simplify the equation to:
(V₁ / T₁) = (V₂ / T₂)
where V₁ is the initial volume, T₁ is the initial temperature, V₂ is the final volume, and T₂ is the final temperature.
Given that the initial pressure (P₁) is 2.90 atm at -14°C and the final temperature (T₂) is 53°C, we can rearrange the equation to solve for the final pressure (P₂):
(P₁ / T₁) = (P₂ / T₂)
Substituting the given values:
(2.90 atm / -14°C) = (P₂ / 53°C)
Now, we can solve for P₂ by cross-multiplication:
(P₂) = (2.90 atm * 53°C) / (-14°C)
Calculating the result:
P₂ = -11.07 atm
Therefore, the final pressure, to the appropriate units, is -11.07 atm.
To solve this question, we can use the combined gas law equation, which relates the initial and final conditions of a gas sample:
(P1 * V1) / T1 = (P2 * V2) / T2
Here, P1 is the initial pressure, V1 is the initial volume, T1 is the initial temperature, P2 is the final pressure, V2 is the final volume, and T2 is the final temperature.
In this case, we are told that the volume and amount of gas remain constant (V1 = V2, and we assume the amount of gas doesn't change). Therefore, we can simplify the equation as:
P1 / T1 = P2 / T2
Now we can substitute the given values:
P1 = 2.90 atm
T1 = -14 °C + 273.15 K = 259.15 K
T2 = 53 °C + 273.15 K = 326.15 K
Plugging in these values, we can solve for P2:
2.90 atm / 259.15 K = P2 / 326.15 K
To find P2, we can rearrange the equation:
P2 = (2.90 atm * 326.15 K) / 259.15 K
P2 ≈ 3.65 atm
Therefore, the final pressure when the temperature is 53°C is approximately 3.65 atm.