At 273K and 1 ATM, most gases typically exist in the gaseous state. However, the specific gas present will depend on the composition of the system.
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.
This is equivalent to 0.2 atm. (152 mmHg)*(1 atm)/(760 mmHg)=0.2atm
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.
0.045 mol L 0.5. Mol.
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.
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.
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.
At 0C and 1 atm, the gas that is best described by the ideal gas law is helium.
Krypton is a colorless, odorless gas at room 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.
water changes from a gas to a solid to a liquid
Simply convert atm to mm Hg using 1 atm = 760 mm Hg. Thus, 3.1 atm = 3.1x760 = 2356 mm Hg
1.0
1 atm of pressure equals 760 mm Hg, so 2 atm = 1520 mm Hg.
1.54 atm
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.
The lowest possible temperature is -273.15 C which equated to '0'K. Therefore, temperature -273K cannot exist. No -ve K temperatures exist.