States of Matter
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5.10. 34.05 mL of phosphorus vapour weighs 0.0625 g at 546°C and 1.0 bar pressure. What is the molar mass of phosphorus?
5.10. 34.05 mL of phosphorus vapour weighs 0.0625 g at 546°C and 1.0 bar pressure. What is the molar mass of phosphorus?
5.8. What will be the pressure of the gas mixture when 0.5 L of H2 at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in all vessel at 27 °C?
5.8. What will be the pressure of the gas mixture when 0.5 L of H2 at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in all vessel at 27 °C?
5.8. Calculation of partial pressure of H2 in 1L vessel:
P1= 0.8 bar, P2=? V1= 0.5 L, V2 = 1.0 L
As temperature remains constant, P1V1 = P2V2
=> (0.8 bar) (0.5 L) = P2 (1.0 L)
=>P2 = 0.40 bar, i.e., PH2 = 0.40 bar
Calculation of partial pressure of O2 in 1 L vessel
P1V1
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5.7. What will be the pressure exerted by a mixture of 3.2g of methane and 4.4g of carbon dioxide contained in a 9 dm3 flask at 27 °C?
5.7. What will be the pressure exerted by a mixture of 3.2g of methane and 4.4g of carbon dioxide contained in a 9 dm3 flask at 27 °C?
5.7. Applying PV = nRT
We get P = nRT / V
Given: nCH4 = 3.2 / 16 mol = 0.2 mol
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Upvote 5.6. The drain cleaner, Drainex contains small bits of aluminium which react with caustic soda to produce dihydrogen. What volume of dihydrogen at 20 °C and one bar will be released when 0.15g of aluminium reacts?
5.6. The drain cleaner, Drainex contains small bits of aluminium which react with caustic soda to produce dihydrogen. What volume of dihydrogen at 20 °C and one bar will be released when 0.15g of aluminium reacts?
5.6. The chemical equation for the reaction is
2 Al + 2 NaOH + H2O? 2 NaAlO2 + 3
Upvote 5.5. Pressure of l g of an ideal gas A at 27°C is found to be 2 bar. When 2 g of another ideal gas B is introduced in the same flask at same temperature, the pressure becomes 3 bar. Find the relationship between their molecular masses.
5.5. Pressure of l g of an ideal gas A at 27°C is found to be 2 bar. When 2 g of another ideal gas B is introduced in the same flask at same temperature, the pressure becomes 3 bar. Find the relationship between their molecular masses.
5.5. Suppose molecular masses of A and B are MA and MB respectively. Then their number of moles will be
nA= 1/MA
Upvote 5.3. Using the equation of state PV= nRT, show that at a given temperature, density of a gas is proportional to the gas pressure P.
5.3. Using the equation of state PV= nRT, show that at a given temperature, density of a gas is proportional to the gas pressure P.
Answer: According to ideal gas equation
PV = nRT
Or &nbs
Upvote 5.1. What will be the minimum pressure required to compress 500 dm3 of air at 1 bar to 200 dm3 at 30°C?
5.1. What will be the minimum pressure required to compress 500 dm3 of air at 1 bar to 200 dm3 at 30°C?
5.1. Initial Pressure, P1 = 1 bar Final Pressure, P2 =?
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