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What is the pressure of 7.85g of CO2 at 27.0c in a volume of 19.6L?
You can use the Ideal Gas Law or the Combined Gas Law. PV/T = PV/T ---- left are usually labeled (1) and right (2) to show different conditions left P = unknown, V = 19.6L, T = (273+27)K right P= 760 torr or 1 amt, V = 22.4 L, T = 273K --- all are standard P(19.6L)/300K = 1atm(22.4L)/273K --- solve for P P = (1 atm)(22.4L)(300K)/ [(273K)(19.6L)] do the math --- get the answer.
The pressure of a gas in a container is 152 mm Hg. what is itequivalent to?
This is equivalent to 0.2 atm. (152 mmHg)*(1 atm)/(760 mmHg)=0.2atm
Suppose two gases in a container have a total pressure of 1.20 ATM. What is the pressure of gas b if the partial of gas a is 0.75 ATM?
To find the pressure of gas B, you can use Dalton's Law of Partial Pressures, which states that the total pressure is the sum of the partial pressures of individual gases. Given that the total pressure is 1.20 ATM and the partial pressure of gas A is 0.75 ATM, you can calculate the pressure of gas B as follows: Pressure of gas B = Total pressure - Pressure of gas A = 1.20 ATM - 0.75 ATM = 0.45 ATM. Thus, the pressure of gas B is 0.45 ATM.
The active mass of 22.2 lit of carbondioxied gas at 273k is?
0.045 mol L 0.5. Mol.
A gas occupies a volume of 2.4 L at 1 ATM what volume will the gas occupy at 6 ATM?
Using Boyle's Law (P1V1 = P2V2), we can rearrange the formula to find the new volume: V2 = (P1 * V1) / P2 V2 = (1 ATM * 2.4 L) / 6 ATM V2 = 0.4 L Therefore, the gas will occupy a volume of 0.4 L at 6 ATM.
What change in pressure would result in the volume of gas increasing A 2 ATM to 3 ATM B 3 ATM to 4 ATM C 4 ATM to 1 ATM D 1 ATM to 3 ATM?
A. An increase in pressure from 2 ATM to 3 ATM will result in a decrease in volume of gas. B. An increase in pressure from 3 ATM to 4 ATM will result in a decrease in volume of gas. C. A decrease in pressure from 4 ATM to 1 ATM will result in an increase in volume of gas. D. An increase in pressure from 1 ATM to 3 ATM will result in a decrease in volume of gas.
What is the pressure of 7.85g of CO2 at 27.0c in a volume of 19.6L?
You can use the Ideal Gas Law or the Combined Gas Law. PV/T = PV/T ---- left are usually labeled (1) and right (2) to show different conditions left P = unknown, V = 19.6L, T = (273+27)K right P= 760 torr or 1 amt, V = 22.4 L, T = 273K --- all are standard P(19.6L)/300K = 1atm(22.4L)/273K --- solve for P P = (1 atm)(22.4L)(300K)/ [(273K)(19.6L)] do the math --- get the answer.
Which gas at 0C and 1 atm is best described by the ideal gas law?
At 0C and 1 atm, the gas that is best described by the ideal gas law is helium.
What is krypton state of matter at room temperature?
Krypton is a colorless, odorless gas at room temperature.
What will the total pressure be and partial pressure be if two gases with pressures of 2 ATM and 3 ATM are mixed at a constant temperature?
The total pressure of the mixed gases will be 5 ATM. The partial pressure of each gas will remain the same as their individual pressures before mixing, so the partial pressure for the gas originally at 2 ATM will remain at 2 ATM, and the gas originally at 3 ATM will remain at 3 ATM.
According to the phase diagram for H2O what happens to the phases of water at 0 degC as the pressure is increased from 0 ATM to 10 ATM?
water changes from a gas to a solid to a liquid
How many millimeters of mercury does a gas exert at 3.1 atm?
Simply convert atm to mm Hg using 1 atm = 760 mm Hg. Thus, 3.1 atm = 3.1x760 = 2356 mm Hg
What is the compressibility factor of chlorine gas at 1 ATM and 250C?
1.0
What is the pressure in mm Hg of a gas at 2atm?
1 atm of pressure equals 760 mm Hg, so 2 atm = 1520 mm Hg.
What is the total pressure of a gas mixture containing partial pressures of 0.23 ATM ATM and 0.89 ATM?
1.54 atm
Does N2 behave more ideally at 1 ATM or at 500 ATM please explain?
Nitrogen (N2) behaves more ideally at 1 ATM rather than at 500 ATM. At higher pressures, deviations from ideal gas behavior become more significant due to the increased intermolecular interactions and molecular volume effects, causing the gas to behave less ideally.
Can a gas exist at -273K?
The lowest possible temperature is -273.15 C which equated to '0'K. Therefore, temperature -273K cannot exist. No -ve K temperatures exist.
