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40 °c was applied to a sealed container filled with helium gas at 8 atm. after 30 minutes the volume remains constant but the pressure doubles. what's the new temperature?
New temperature=156.5K
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Find the osmotic pressure at 25°C when 60.0 mL of a solution containing 5.60 grams of glucose (MW=180 g/mol) is prepared. a. 12.7 atm b. 10 atm c. 11 atm d. 1.3 atm
Osmotic pressure =12.7atm
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50.0 and tank of helium gas placed outside a laboratory has a pressure of 5.0 atm at 25 celsius how much will the pressure increase at noon time when the temperature reaches 32 celsius
5 atm — 25Cx atm — 32Cx=32*5/25=6.4 atm
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At constant temperature, a sample of helium gas expands from 922 mL to 1.14 L against a pressure of 2.33 atm. Find w (in J) done by the gas (1J = 9.87310 expoent -3 atm L).
922×1.14×2.33/9.8731= 248.05J
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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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A sample of helium saturated with water vapour exerts a total pressure of 103.17 kPa. If the pressure of the helium is 99.39 kPa, what is the temperature?
At equillibrium temperature of water vapour is 100°cSo we have,, P1/T1=P2/T2=103170/100=99390/T2=T2=99390/1031.7=96.3 degrees.
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A helium gas cylinder of the sort used to fill balloons has a volume of 180 L and and a pressure of 2200 psi ( 150 atm) at 25° C. How many moles of helium are in the tank? How many grams?
Given n=MassMolar mass=PVRT.Mass=PVRT×molar mass,.........Agreed........?And, as is typical, we use the value of..........R=0.0821⋅L⋅atm⋅K−1⋅mol−1The which has units that chemists typically use. And so we plugs in the numbers:Mass=1.2⋅atm×2.00⋅L×4.00⋅g⋅mol−10.0821⋅L⋅atmK⋅mol×300⋅K≅400 moles
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If the total air pressure is 1.05 atm, the partial pressure of carbon dioxide is 0.08 atm, and the partial pressure of hydrogen sulfide is 0.05 atm, what is the partial pressure of the remaining air?
As we know, Total pressure is the sum of partial pressure of individual gases.PT = 1.05 -(0.08+0.05+Pair)Pair = [0.92] atm
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A sample of helium gas takes up 15 L. After being compressed down to a volume of 8 L, the sample has a pressure of 4.3 atm. What was the original pressure?
P1 = unknownV1 = 15 LP2 = 4.3 atmV2 = 8 LT1 = T2 = constSolution:Since the temperature and amount of gas remain unchanged, Boyle's law can be used. Boyle's gas law...
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Container A holds 782 mL of ideal gas at 2.80 atm. Container B holds 174 mL of ideal gas at 4.40 atm. If the gases are allowed to mix together, what is the resulting pressure?
Answer on Question #83513Container A holds 782 mL of ideal gas at 2.80 atm. Container B holds 174 mL of ideal gas at 4.40 atm. If the gases are allowed...
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