Answer:
Step 1: Explanation
According to Dalton's Law of Partial Pressures the partial pressure of a component of a gaseous mixture depends on the mole ratio of each component and the total pressure of the gaseous mixture
Partial pressure of component = mole fraction of that component x total pressure
Step 2: Calculation of mole fraction
mole fraction of methane = 90 % / 100 % = 0.9
mole fraction of ethane = 8.90 % / 100 % = 0.089
mole fraction of propane = 1.10 % / 100 % = 0.011
Step 3: Calculation of partial pressure of propane
We know
Partial pressure of component = mole fraction of that component x total pressure
we got,
total pressure = 307.2 kPa
mole fraction of propane = 0.011
Partial pressure of Propane = mole fraction × Total pressure = 0.011 × 307.2 kPa = 3.38 kPa
hence, the partial pressure of propane = 3.38 kPa [ note: exact value of partial presure = 3.3792 kPa]
a sample of gas isolated from unrefined petroleum contains 90.0% methane, 8.90% ethane, and 1.10% propane...
Perm calculations with Dalton's Low Question A sample of gas isolated from unrefined petroleum contains 9.00 mol CH 0.890 mol CH. and 0.110 mol CH, at a total pressure of 307.2 kPa What is the partial pressure of CH,? Select the correct answer below: 276 LP. O 27.3 kPa 3.37 kP O 307 kPa - here to search 11:40 PM AD6 44 2/2000
Be sure to answer all parts.A sample of natural gas contains 6.327 moles of methane (CH4), 0.803 moles of ethane (C2H6), and 0.216 moles of propane (C3H8). If the total pressure of the gases is 2.99 atm, what are the partial pressures of the gases?
A) Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount of propane, C3H8) were added to the same 10.0-L container. At 23.0 ∘C, the total pressure in the container is 3.90 atm . Calculate the partial pressure of each gas in the container. Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane. B) A gaseous mixture of O2O2 and N2N2 contains...
PART A: Three gases (8.00 g of methane, C H 4 , 18.0 g of ethane, C 2 H 6 , and an unknown amount of propane, C 3 H 8 ) were added to the same 10.0- L container. At 23.0 ∘ C , the total pressure in the container is 3.80 atm . Calculate the partial pressure of each gas in the container. Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of...
Part A Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H, and an unknown amount of propane, C3Hs) were added the same 10.0-L container. At 23.0c C, the total the container is 3.50 atm . Calculate the partial pressure each gas in the container. pressure Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane. View Available Hint(s) ΠνΠ ΑΣ Φ atm Previous Answers Submit X...
A sample of methane gas has a volume of 10. L at a pressure of 1.5 atm and a temperature of 20.0 °C. What is the temperature of the gas in °C if it is expands into 18 L with a pressure of 0.90 atm? Please respond with the correct number of significant figures in scientific notation.
6. Problem 5.25 525. An ideal gas mixture contains 35% helium, 20% methane, and 45% nitrogen by volume at 200 atm absolute and 90°C. Calculate (a) the partial pressure of each component. (b) the mass fraction of methane, (c) the average molecular weight of the gas, and (d) the density of the gas in kgim 7. Problem 5.30 5.30. A fuel gas containing 86% methane, 8% ethane, and 6% propane by volume t ows to a furnace at a rate...
For many purposes we can treat propane (CH) as an ideal gas at temperatures above its boiling point of - 42. "C. Suppose the temperature of a sample of propane gas is lowered from 25.0°C to - 22.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.58 kPa and the volume decreased by 40.0%, what is the final pressure? Round your answer to the correct number of significant digits. kPa
a) A natural gas fuel contains 80 v/o methane, 10 v/o ethane, and 10 v/o propane. Determine the heat released by combustion of 1m3 of the gas. Assume that products of combustion are CO2 and liquid H2O. b) How would the answer to part (a) change if the water produced were vaporized?
A 1.00 L flask is filled with 1.10 g of argon at 25 °C. A sample of ethane vapor is added to the same flask until the total pressure is 1.400 atm Part A What is the partial pressure of argon, PAr, in the flask? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) HA PAr0.727 atm Previous Answers Submit Incorrect; Try Again Part B What is the partial pressure of ethane, Pethane, in...