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The pressure of a sample of helium in a 1.50-L container is 0.88 atm. What is the new pressure if the sample is placed in a 2.00 L container?
P1V1 = P2V20.88 atm × 1.50L = 2.00L × X1.32 = 2.00XX = 1.32/2.00= 0.66 atm
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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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A gas exerts a pressure of 2.0 atm, at 30°C, in a 10 L container. In what size container would the same amount of gas exert a pressure of 4.0 atm at 20° C?
Using the gas law: pV = nRT, and keeping the same number of moles of gas (n),we find the final volume V2:V2 = (T2/p2)*(p1*V1/T1) = (293 K/ 4.0 atm)*(2.0 atm...
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Calculate the volume of ammonia gas formed by the reaction between 7 grams of nitrogen gas and excess nitrogen gas at r.t.p.
7g of nitrogen and excess of nitrogen will form excess of ammonia
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When a real gas is placed into a container at high pressure, why might the pressure of the gas be higher than what was predicted by the ideal gas law?
The weight and size of the molecules that are negotiated in the ideal gas law increase the volume of the gas mixture. However, as the container has a constant volume,...
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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 40.8 mol sample of methane gas CH4(g) is placed in a 1020 L container at 298 K. What is the pressure, in atm of the methane gas?
ollowing the Ideal gas law: pV=nRT where R is gas constant and equal to 0.0821 L·atm·K-1·mol-1 For this case, pressure in atm have been equal to: p=nRTV=40.8 (mol)∙0.0821 (L∙atm∙K-1∙mol-1)∙298 (K)/...
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A sample of nitrogen gas is collected in a 100 mL container at a pressure of 688 mmHg and a temp. of 565 degree C. How many grams of nitrogen are present in this sample?
To answer this question we should use ideal gas law : PV=nRT. V= 100mL=0.1 L = 0.1 dm3= 0.110-3m3; P= 688 mmHg or P =688133.322 Pa =91725.54 Pa; T =565C...
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In one mole of nitrogen gas (N2) there are two atoms of nitrogen (N).
How many atoms are there in three moles of nitrogen gas?
In one mole of nitrogen gas (N2) there are two atoms of nitrogen (N). There are six atoms of nitrogen(N) in three moles of nitrogen gas (N_2)
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