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What is the total pressure of a mixture containing two gases if the partial pressure of one gas is 70 torr and the partial pressure of the other gas is 30 torr?
P1 = 70 torr , P2 = 30 torrPTotal = P1 + P2 PTotal = 70 torr + 30 torr = 100 torr
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What is the pressure of a mixture of 525 mmHg of N<sub>2</sub>, 340 mmHg of O<sub>2</sub> and 157 mmHg of He?
P total= PN2+PO2+PHe =(525+340+157)mmHg =1022mmHg
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A nitrox to gas mixture for scuba diving contains oxygen gas at 50 ATM and nitrogen gas at 90 6:00 a.m. what is the total pressure in ATM of the scuba gas mixture
Dalton's law states; The total pressure exerted by a mixture of gases is equal to the sum of the pressures of each of the different gases making up the mixture,...
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The partial pressure of gas X is 340 mm Hg. The partial pressure of gas Y is 264 mm Hg. The partial pressure of gas Z is 100 torr. What is the total pressure exerted by the gases in this system?
According to Dalton's Law of Partial Pressure;Pt= Px +Py+ Pz = (340+264+100)mmHg (since 1torr=1mmHg) = 704mmHg
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the total pressure of gas collected over 785.0 mmhg and the temperature is 18.0 c. What is the pressure of hydrogen gas formed in mmHg
Pressure of hydrogen gas=718mmHg
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In SATP to increase 1 mole gas volume to 40L, how much temperature should increase if pressure is half decreased---
1.389.43K
2.91.43°C
3.298K
4.116.43°C
Find volume of 1 mole of a gas at SATP:P= 101325 Pan= 1 moleR= 8.314 m3Pa/(K*mole)T = 298.15PV=nRTV= nRT/V = 1*8.314*298.15/101325 = 24.5 dm3Use Combined Gas Law to determine final...
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A gas mixture contains 4.0 g of CO(g), 11.0 g of CO₂(g) and 2.0 g of CH4 (g) in a 50.0 - L vessel. Calculate the partial pressure of each gas in the mixture.
The partial pressure of each gas in a mixture is proportional to its mole fraction.n = m / MM (CO) = 28 g/molM (CO2) = 44 g/molM (CH4) = 16.04...
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A 2.0 dm³ container contains 0.15 mol of N₂ gas and 0.20 mol of O₂ gas under a total pressure of 100 kNm⁻². Calculate the partial pressure of O₂ gas in the mixture.
Solution:Calculate the mole fraction (x) of O2 gas in the mixture:x(O2) = number moles of O2 / total number moles of gasTotal number moles of gas = Moles of...
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A mixture of four gases exerts a total pressure of 860mmHg. Gas A and B each exert 220mmHg. Gas C exerts 110mmHg. What pressure is exerted by gas D?
For this task we use the Dalton’s law which says that total pressure of mixture of gases equals to the sum of partial pressures of individual gases: Ptotal=PA+PB+PC+PD Therefore PD...
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A sample of a gas occupies 1640 mL at 70◦C and 740 torr. What volume would it occupy at the same pressure and 389◦C? Answer in units of mL.
According to the ideal gas law:P1×V1/T1 = P2×V2/T2,where P1 and P2 - initial and final pressures, V1 and V2 - initial and final volumes, T1 and T2 - initial and...
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