625 mL of N2 was collected over water when the atmospheric
pressure was 822 mmHg. The...
625 mL of N2 was collected over water when the atmospheric
pressure was 822 mmHg. The temperature of the water was 27.0°C. How
many grams of nitrogen were collected? (Vapor pressure of water @
27°C is 26.7 mmHg)
A mole of air is sampled from the atmosphere when the
atmospheric pressure is 765 mmHg, the temperature is 25 C, an
relative humidity is 75%. The sample of air is placed inside a
closed container and heated to 135 C and then compressed to 2 atm.
What are the relative humidity, the humidity, and the mole fraction
of water in the compressed air?
50 L of a gas were collected over water when the barometer read
684.0 mmHg and the temperature was 14 oC . What volume would the
dry gas occupy at standard conditions?
HINT: Consider Dalton’s law of partial pressures.
A volume of 259 mL of hydrogen is collected over water; the
water level in the collecting vessel is the same as the outside
level. Atmospheric pressure is 756.0 Torr and the temperature is 25
°C. Calculate the molar mass of the metal.
16. If a sample of oxygen gas is collected over water at a
pressure of 0.921 atm and 23°C, whatis the partial pressure of the
oxygen gas?
17. A mixture of gases exerting a pressure of 1.11 atm consists
of 0.20 mol of O2 gas, 0.3 mol of H2 gas, and 0.7 mol of CO2 gas.
What is the partial pressure of the O2
gas, the H2 gas andthe CO2 gas?
18. 0.5 mol of O2 is added to a...
The vapor pressure of water at 45oC is 71.88 mmHg.
What is the vapor pressure of a sugar
(C12H22O11) solution made by
dissolving 54.18 g of sugar in 85.56 g of water?
A mixture of gases collected over water at 14oC has a total
pressure of 1.198 atm and occupies 72 mL. How many grams of water
escaped into the vapor phase?
1.) The total pressure (PT) os a sample of a gas
collected over water at 13.0oC is 0.588 atm. Determine
the partial pressure (Pi) of the gas.
2.) Rearrange the ideal gas equation to solve for density (g/v).
Hint: you will need to make a substitution for moles "n"
3.) Use your quation from (z) and the result from (l) to
calculate the molecular weight of a gas if 303 ml of the gas,
collected at 28oC, weighed 0.347g.
KEY PART that is TRICKY for me: (The vapor pressure of water is
23.78 mmHg at 25∘C)
A common way to make hydrogen gas in the laboratory is to place
a metal such as zinc in hydrochloric acid (see the figure). The
hydrochloric acid reacts with the metal to produce hydrogen gas,
which is then collected over water. Suppose a student carries out
this reaction and collects a total of 154.0 mL of gas at a pressure
of 742 mmHg...
Determine the concentration of H2SO4 when
10 mL of the surround water was collected near the C & H Sugar
Company. Your sample was titrated with 5 ml of 0.5 Molar NaOH
solution to neutral the pH. Determine the concentration of
H2SO4 in your water sample.
1.A
certain gas has a volume of 161 mL and a pressure of 533 mmHg. The
volume changes to 742 mL and the temperature remains constant. What
is the new pressure? Answer to a whole number .
2.A certain gas has a volume of 519 mL at 27.0C. If the
temperature changes to 70.6C at a constant temperature, what is the
new volume. Answer to a whole number