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A fixed mass of gas at 35 0C exhibits a pressure of 12 atm and occupies a volume of
65 cm3.
(a) Use Boyle’s law to calculate the volume the gas will occupy at 35 0C if the pressure is
increased to 45 atm.
(b) Use Charles’s law to calculate the volume the gas will occupy if the temperature is
increased to 135 0C while the pressure is held constant
What is the concentration of a solution with a volume 3.3 mL that contains 12 grams of ammonium sulfite?
You are a NASA engineer. You are the chief engineer for the Apollo 13 mission to the moon. The astronauts are running out of oxygen and need to get rid of the excess carbon dioxide. You know that sodium hydroxide (NaOH) has been suggested as a means of removing carbon dioxide from the spacecraft cabin. The filter which they had been using is fully saturated and no longer works. You remember that the astronauts have a 5000. g container of sodium hydroxide on the ship. You also know that sodium hydroxide can be used to remove carbon dioxide.
Use the following reaction: NaOH + CO2 → Na2CO3 + H2O
The astronauts have 2 days left before they land on Earth. You know that there are three astronauts, and each astronaut emits roughly 500. g Of carbon dioxide each day. Is there enough sodium hydroxide in the cabin to cleanse the cabin air of the carbon dioxide, or are the astronauts doomed?
a flask of 7l contains a mixture of 6g of o2 and 15g of n2 at 30°c.what is the partial pressure of the oxygen gas?
Bailey bought some of blue balloons for his birthday, the balloons inflated at the initial pressure of 1.70 atm, at that pressure the gas inside of it takes up 4.25L of volume, if Bailey increases the pressure to 2.40 atm, what will be the new volume?
14.7 grams of sodium sulfate (Na2SO4) was dissolved in 3.15 L of water. Determine the Ion Concentration of the following elements inside the solution.
1.) Sodium (Na2)?
2.) Sulfur (S)?
3.) Oxygen (O4)?
Camphor (C10H16O2) freezes at 175 °C, and it has a particularly large freezingpoint-depression constant, Kf = 40.0 °C/m. When 0.086 g of an organic substance of unknown molar mass is dissolved in 22.01 g of liquid camphor, the freezing point of the mixture is found to be 1.7 °C below of pure camphor. What is the molar mass of the solute?
You add 0.25 g of an unknown solute to 11.1 g of benzene. The boiling point of the benzene rises from 80.10 °C to 80.46 °C. What is the molar mass of the compound? Kb=2.53 °C /m
A solution of an unknown non-dissociating solute was prepared by dissolving 0.300 g of the substance in 40.0 g of CCl4. The boiling point of the solution was 0.357 °C higher than that of the pure solvent. Calculate the molar mass of the solute. Kb=5.02 °C/m
Three liters of hydrogen at -20°C is allowed to warm to 27°C. What is the volume at this temperature if the pressure remains constant?
Three liters of hydrogen at -20°C is allowed to warm to 27°C.What is the volume at this temperature if the pressure remains constant.
A battery with a terminal voltage of 12V is connected to a circuit consisting of four 10 ohms and one 5 ohms resistor all in series. Assume the battery has negligible internal resistance. Calculate the current through each resistor.
