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What is the temperature of 9 moles of an ideal gas in a 35 liter container at 14 atm pressure?
Use the ideal gas law, PV=nRT, in which P= pressure, V= volume, n= number of moles, R= the gas constant, and T= temperature. In this problem you know V, T, R, and n. What you are trying to figure out is the P.
P= Unknown
V= 35.0 L
n= 6.50 moles
R= .082057 L ATM/mol K
T= 305 K
PV= nRT
P35.0=6.50(.082057)305
P= 4.65 ATM
What else can I help you with?
In a 2 liter container what is the partial pressure of oxygen?
The partial pressure of oxygen in a 2 liter container depends on the concentration of oxygen present in the container. If you know the concentration of oxygen in the container, you can use the ideal gas law to calculate the partial pressure. The formula is: partial pressure = concentration of oxygen x gas constant x temperature.
Which element will uniformly fill a closed 2.0 liter container at STP?
At Standard Temperature and Pressure (STP), one mole of any ideal gas will occupy 22.4 liters. So to fill a 2.0 liter container at STP, you would need 2.0/22.4 = 0.089 moles of an ideal gas. This means any gas that is present in that amount and under those conditions can uniformly fill the container.
What will the pressure inside the container become if the piston is moved to the 1.80 L rm L mark while the temperature of the gas is kept constant?
This problem can be solved with the ideal gas law. The original pressure and volume of the container are proportional the final pressure and volume of the container. The original pressure was 1 atmosphere and the original volume was 1 liter. If the final volume is 1.8 liters, then the final pressure is 0.55 atmospheres.
How many grams of oxygen gas occupy 2.5 liter container if the pressure is 2.5 ATM and the temperature is 30 C?
To calculate the mass of oxygen gas, use the ideal gas law formula PV = nRT where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. First, convert the temperature to Kelvin (30°C + 273 = 303 K). Then, rearrange the formula to solve for the number of moles (n = PV / RT). Finally, convert moles to grams using the molar mass of oxygen gas (32 g/mol).
What is the density of hellium?
The density of helium at room temperature and pressure is approximately 0.1785 grams per liter.
In a 2 liter container what is the partial pressure of oxygen?
The partial pressure of oxygen in a 2 liter container depends on the concentration of oxygen present in the container. If you know the concentration of oxygen in the container, you can use the ideal gas law to calculate the partial pressure. The formula is: partial pressure = concentration of oxygen x gas constant x temperature.
A 4.0 liter container of gas in initially at a pressure of 16 ATM what will the pressure be if the voume is changed to 1 liters at constant temperature?
Use Boyle's Law, applicable for ideal gases at constant temperature, to solve this problem: P1*V1 = P2*V2
Which element will uniformly fill a closed 2.0 liter container at STP?
At Standard Temperature and Pressure (STP), one mole of any ideal gas will occupy 22.4 liters. So to fill a 2.0 liter container at STP, you would need 2.0/22.4 = 0.089 moles of an ideal gas. This means any gas that is present in that amount and under those conditions can uniformly fill the container.
What will the pressure inside the container become if the piston is moved to the 1.80 L rm L mark while the temperature of the gas is kept constant?
This problem can be solved with the ideal gas law. The original pressure and volume of the container are proportional the final pressure and volume of the container. The original pressure was 1 atmosphere and the original volume was 1 liter. If the final volume is 1.8 liters, then the final pressure is 0.55 atmospheres.
a container of an ideal gas is at a constant volume what occurs when the volume of the contianer is doubled from 1 liter to 2 liters?
The volume doubles
If you were to transfer a liter of air into a 2-liter container how much of the 2-liter container would be filled?
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What is the temperature of 9 moles of an ideal gas in a 35 liter container at 14 atm pressure-?
This looks suspiciously like a homework question! Temp of 8 mol of ideal gas in a 32 L container at 12 atm pressure? pV = 12 * 32 = 384 L.atm nRT = 8 * 0.082 * T = 0.656 * T L.atm T = 384/0.656 = ~516 K That should provide the template for your answer!
If you attach a manometer or pressure gauge to your two liter container what pressure would you measure?
The pressure measured in a closed two-liter container would depend on factors such as the temperature and the amount of gas or liquid inside the container. If the container is sealed and there is no chemical reaction occurring inside, the pressure would remain constant at the equilibrium pressure of the system.
If the same quantity of heat is added to both a 1-liter and a 2-liter container of water the temperature change of water in the 1-liter container will be?
The temperature change of the water in the 1-liter container will be greater than that of the 2-liter container when the same quantity of heat is added. This is because temperature change is inversely proportional to the mass of the substance when heat is added, as described by the formula (Q = mc\Delta T), where (Q) is the heat added, (m) is the mass, (c) is the specific heat capacity, and (\Delta T) is the temperature change. Since the 1-liter container has less mass, it will experience a larger temperature increase.
Can you put ten liters of oxygen into one liter volume?
No, it is not possible to compress 10 liters of oxygen into a 1-liter volume. The volume of gas is dictated by its pressure and temperature through the ideal gas law, which means you cannot reduce 10 liters of gas into 1 liter without changing these properties significantly.
What is the temperature of a 100 liter container having 1 mole of an ideal gas at a pressure of 20 kilo pascals?
To find the temperature, we can use the ideal gas law equation: PV = nRT. Rearranging the equation to solve for temperature (T), we have T = (PV) / (nR), where P is the pressure, V is the volume, n is the number of moles, and R is the ideal gas constant. Plugging in the given values (P = 20 kPa, V = 100 L, n = 1 mol, and R = 8.314 J/(mol·K)), we find that the temperature is approximately 239 K.
What is the pressure of gas in a 30 liter container at 49 degrees c?
Gas pressure depends on volume, temperature, AND the amount of gas. You didn't give an amount of gas, so there is no way to answer your question.
