1) A gas has a pressure of 3 atm when the temperature is 25C, what is the new pressure when the temperature is raised to 50C? (make sure temp is in K) - round answer to hundredths place
2) Neon at 2 atm and 273K has a volume of 10L. What is the new pressure if the volume is 20L and temperature is 400K? (round to tenths place)
3)What is the new volume of a gas originally at 273K and 20 L when the temperature is increased to 300K? (to the nearest whole number)
4)A 12 L sample of gas at 2 atm, has the pressure decreased to 1 atm, what is the new volume? *
1. Make use of pressure law,
P1/T1 = P2/T2, since volume is constant (ensure your Temperature is converted from Celsius to Kelvin)
2. Make use of the general Gas Law.
P1V1/T1 = P2V2/T2 (ensure your units are converted)
3. Charles Law is suitable for this V1/T1 = V2/T2
4. Use Boyles Law
p v = n r t ... pressure, volume, number of moles, gas constant, Kelvin temp
set up the starting equation , then change what you need to
... and see the results
1) To calculate the new pressure of a gas when the temperature is raised, we can use the combined gas law equation:
P1 * V1 / T1 = P2 * V2 / T2
Where:
P1 is the initial pressure (in atm)
V1 is the initial volume (in liters)
T1 is the initial temperature (in Kelvin)
P2 is the final pressure (unknown)
V2 is the final volume (unknown)
T2 is the final temperature (in Kelvin)
First, convert the initial temperature from Celsius to Kelvin by adding 273:
T1 = 25 + 273 = 298K
Now, plug in the given values into the equation:
3 * V1 / 298 = P2 * V1 / 323
Cross multiply and solve for P2:
3 * V1 * 323 = P2 * V1 * 298
(3 * 323) / 298 = P2
P2 ≈ 3.28 atm
Therefore, the new pressure when the temperature is raised to 50°C is approximately 3.28 atm.
2) To find the new pressure of Neon gas when the volume and temperature change, we can use the combined gas law equation:
P1 * V1 / T1 = P2 * V2 / T2
Given:
P1 = 2 atm
V1 = 10 L
T1 = 273 K
V2 = 20 L
T2 = 400 K
Plug in the values into the equation:
2 * 10 / 273 = P2 * 20 / 400
Cross multiply and solve for P2:
2 * 10 * 400 = P2 * 20 * 273
(2 * 10 * 400) / (20 * 273) = P2
P2 ≈ 2.08 atm
Therefore, the new pressure when the volume is 20L and the temperature is 400K is approximately 2.08 atm.
3) To calculate the new volume of a gas when the temperature is increased, we can use the following equation derived from the combined gas law:
(V1 * T2) / T1 = V2
Given:
T1 = 273 K
V1 = 20 L
T2 = 300 K
Plug in the values into the equation:
(20 * 300) / 273 = V2
6000 / 273 ≈ V2
V2 ≈ 22 L
Therefore, the new volume of the gas when the temperature is increased to 300K is approximately 22 L.
4) To find the new volume when the pressure changes, we can use Boyle's Law. Boyle's Law states that the pressure and volume of a gas are inversely proportional, assuming constant temperature and moles of gas.
P1 * V1 = P2 * V2
Given:
P1 = 2 atm
V1 = 12 L
P2 = 1 atm
V2 = Unknown (to be calculated)
Plug in the values into the equation and solve for V2:
2 * 12 = 1 * V2
V2 = (2 * 12) / 1
V2 = 24 L
Therefore, the new volume of the gas when the pressure decreases to 1 atm is 24 L.
1) To solve this problem, you 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.
First, convert the initial temperature from Celsius to Kelvin by adding 273 to it:
T1 = 25 + 273 = 298K
Next, plug in the values into the formula:
P1 / 298 = P2 / (50 + 273)
Now, solve for P2:
P2 = (P1 * (50 + 273)) / 298
Substituting the values, we have:
P2 = (3 * 323) / 298
P2 ≈ 3.25 atm (rounded to hundredths place)
Therefore, the new pressure when the temperature is raised to 50°C is approximately 3.25 atm.
2) The problem states that the initial pressure, volume, and temperature are 2 atm, 10 L, and 273 K respectively. Let's use the combined gas law equation again to find the new pressure:
P1 / T1 = P2 / T2
Convert the initial temperature from Celsius to Kelvin:
T1 = 273 K
Plug in the values and solve for P2:
2 / 273 = P2 / 400
P2 = (2 * 400) / 273
P2 ≈ 2.92 atm (rounded to tenths place)
Therefore, the new pressure when the volume is 20L and the temperature is 400K is approximately 2.92 atm.
3) The problem gives an initial temperature of 273K and an initial volume of 20L. Let's use the combined gas law equation once more to find the new volume:
P1 / T1 = P2 / T2
Since the pressure is not given, we can assume it remains constant. Therefore, P1 / P2 = 1.
Plug in the values and solve for the new volume:
20 / 273 = V2 / 300
V2 = (20 * 300) / 273
V2 ≈ 21.97
Rounding the volume to the nearest whole number, the new volume when the temperature is increased to 300K is 22 L.
4) To solve this problem, we can use the Boyle's Law equation:
P1 * V1 = P2 * V2
Plug in the given values:
2 atm * 12 L = 1 atm * V2
Solve for V2:
V2 = (2 atm * 12 L) / 1 atm
V2 = 24 L
Therefore, the new volume when the pressure is decreased to 1 atm is 24 L.