Gaseous and liquid states Questions and Answers

Methane gas and oxygen gas react to form water vapor and carbon dioxide gas. What volume of carbon dioxide would be produced by this reaction if 2.32 L of oxygen were consumed? Also, be sure your answer has a unit symbol, and is rounded to 3 significant digits.

A reaction between liquid reactants takes place at 6.0 °C in a sealed, evacuated vessel with a measured volume of 5.0 L. Measurements show that the reaction produced 25. g of sulfur tetrafluoride gas. Calculate the pressure of sulfur tetrafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits.

Suppose this container is filled with 27.6 L of oxygen gas (O₂) at STP. Approximately how many moles of oxygen would there be in the container?

How many molecules are there in 0.758 moles of Hydrochloric Acid?

An aerosol can is empty, except for the propellant gas which exerts a pressure of 1.20 atm at 24 °C. If the can is thrown into a fire and heated to a temperature of 595 °C, what will be the pressure inside the hot can?

If a gas is at STP (standard temperature and pressure), the temperature is 0.00°C and the pressure is 1.00 atmosphere. Calculate the volume of exactly 1 mole of gas in liters, giving your answer to three significant figures. The gas constant is 0.08206 L.atm/K.mol. PV = nRT

At 25°C, the vapor pressure in equilibrium with a solution containing CS₂ and CH3CN (solvent) has a total pressure of 263 mmHg. The mole fraction of CS₂ in vapor is 0.855. What is the mole fraction of CS₂ in the solution? At 25°C, the vapor pressure of CS₂ is 375 mmHg.

A 15 mL sample of nitrogen at 38 °C and 2.2 atm is heated to 42 °C and the pressure changed to 1.4 atm. What volume (in mL) does the gas occupy at this final temp and pressure?

A 395 mL balloon of hydrogen is cooled from 75 °C to -65 °C. Calculate the new volume in mL at constant pressure. Make sure you convert each temperature in kelvins (K).

"Determine the initial volume, in m³, of a gas with a starting temperature of 0°C. The final temperature of the gas is 200°C, with a final volume of 145 m³." The student says that their calculator gave them an "Undefined" error. They tried again, and got the same error. What is the student forgetting to do?

A sample of oxygen has a volume of 850 mL at 31 °C and 266 torr. What is the pressure of the gas in atmospheres at 69 °C if the new volume is 450 mL? Using the named gas laws and Table 11.2 as your guide, answer the following:. Based upon the volume change (V1 to V2), how do you expect the pressure to change (P1 to P2)? Based upon the temperature change (T1 to T2), how do you expect the pressure to change (P1 to P2)? When you rearrange the equation to solve for P2, what is the equation? Each blank should contain a letter number combination (format like P2).

A 2.75 L sample of methane gas exerts a pressure of 1550 mm Hg. Calculate the new pressure (in atm) if the volume changes to 4.75 L at constant temperature. Look at what variables you have and what variables are not changed (or not mentioned in problem). You have volume and pressure information so this means the other factors are held constant.

For the following equation Fe(s) + 2 HCl (aq) ---> H₂ (g) + FeCl₂ (aq) If 20 grams of Fe reacts with 4000 mL of a 0.1 M solution of HCl, what will the volume of the H₂ gas be if it has a pressure of 0.5 atm and a temperature of 250 K?

A flexible sealed plastic container is holding an ideal gas that has the initial conditions where pressure is 755 mmHg, temperature is 87.9 °C with a volume of 0.123 L. If the container is placed in the freezer and the temperature of the gas drops to 45.6°C with a new volume of 0.089 L, what would the new pressure (atm) of the gas be?

Using Figure 9.13 from section 9.2 the OpenStax Textbook entitled Chemistry 2E by Flowers, Leopold et al., what is the value of K in Boyle's Law relationship of PV=K? Enter an integer or decimal number

The partial pressure of O₂ and N₂ gases are 0.252 atm and 0.125 atm. These gases are held in a 15.3 L vessel at 88.3 °C. If the temperature and volume remain constant when 0.444 moles of argon are added, what will be the total pressure (atm)?

An unknown non-metal element has a mass of 0.120g. If the gas experiences the following conditions with a pressure of 0.765 atm, volume of 35.55 mL and a temperature of 88.3 °C, identify the element?

A sample of ideal gas ha a volume of 3.20 mL. At constant pressure and moles, the gas is heated to 279 K and the volume reaches 0.0340L. What is the initial temperature of the gas in Kelvin.

A balloon contains 1.21 x 105 L of ideal gas at 265K. The gas is then cooled to 201 K. What is the volume (L) assuming no gas enters or exits the balloon?

For the following chemical equation 2 Al (s) + 6 HCl (aq) ---> 2 AlCl3 (aq) + 3H₂ (g) How many grams of Al should be mixed with hydrochloric acid to obtain the hydrogen gas conditions of 2.06 L, 301 K and 2.25 atm?

It's 32°F (0°C) outside under normal atmospheric conditions (1 atm) at a stunt performer's birthday party. There is a huge blue balloon filled with flammable hydrogen (H₂, molar mass = 2.02 g/mol) gas that she plans to safely ignite, causing a massive explosion. Inside the balloon is 243 g of H₂(g). What is the volume of the balloon, in liters? Round to the nearest whole number.

The melting point for acetanilide is 113- 115°C. The following answer choices represent the melting point of acetanilide for various students. Which student has the most pure recovered acetanilide? A. Student A: 111-114°C B. Student B: 105-110°C C. Student C: 107-111°C D. Student D: 112-114°C

A gas stored in a container at 19.9°C has a pressure of 281 kPa is placed next to the fireplace. The temperature increased to 620 What is the pressure of the gas inside the container? (Answer in integer)

An automobile tire is filled with air at a pressure of 35.0 psi at 25°C. A cold front moves through and the temperature drops to 5°C. Assuming no change in volume, what is the new tire pressure?

The combustion reaction of ethane gas, C₂H6(g) (molar mass=30.068 g/mol) produces CO₂(g) and H₂O(g) according to the chemical equation: 2 C₂H6(g) +7O₂(g) 4 CO₂(g) + 6 H₂O(g) If 35 5 g of C₂Hg(g) is burned in excess of oxygen, how many liters (in L) of CO₂(g) is released into the atmosphere at 25°C and 1 &m. Given R = 0.08206 L atm/mol K

A gas in a cylinder with a piston occupied a volume of 963 mL at 233°C. The cylinder is cooled down to a temperature of 22.9°C. What is the volume (in mL) of gas in the cylinder?

What volume of 1.25 M HCl in liters is needed to react completely (with nothing left over) with 0.750 L of 0.100 M Na₂CO3? Express your answer numerically in liters.

To cough, you inhale about 2.5 L of air at ambient temperature and pressure. The epiglottis and vocal cords shut, trapping the air in the lungs where it warms to body temperature and compressed to about 1/3 the volume. Suddenly opening the epiglottis and vocal cords releases the air explosively. Estimate the gas pressure in the lungs prior to its release. it varies a bit from cough to cough, but we can estimate ~2.5 atm ~ 4.3 atm ~0.31 atm ~ 3.1 atm ~1.3 atm

Which statement CORRECTLY describes a phase change concerning water? a) when liquid water gains enough heat, it will change to a solid. b) Cooling liquid water will cause a phase change to a solid. c) when water vapor gets hot enough, it will turn into liquid water. d) Cooling water vapor can never cause a phase change.

A sample containing 45.0 moles of propane gas at a temperature of 25.0 °C is stored in a 15.0-liter cylinder. What is the pressure of the gas inside the cylinder? a) 6.16 atm b) 3.69 atm c) 73.4 atm d) 44.0 atm

Hydrogen bonding is a particularly strong intermolecular force. Click on the 2 main reasons why this is so. A) N-H, O-H, and F-H bonds are highly polar resulting in strong dipole-dipole forces. B) Highly negatively charged H atoms make strong intermolecular bonds. C) London forces for H atoms are unusually strong due to the small size of a hydrogen atom. D) The non-bonding electrons on the N, O, and F atoms participate in the hydrogen bond adding to the strength of the hydrogen bond.

Which of the following sets of varables when graphed will give a linear relationship with a positive slope when all other variables are held constant? (Choose all that are correct.) Number of moles of gas versus Volume Pressure versus 1/Temperature Volume versus 1/Pressure. Pressure versus volume Pressure versus Temperature Pressure versus 1/Volume Volume versus Temperature

At 1.16 atm and 16.48 °C, a 2.63 g sample of gas occupies a volume of 2320 mL. Calculate the molar mass of the gas.

A reaction in aqueous solution is run in a calorimeter and it is found that the the solution gains 53 kJ of heat and the calorimeter gains 3 kJ of heat. What is the heat gained or lost by the reaction (qrxn) in kJ? (If it is negative, include the negative sign. If it is positive, include nothing)

A sample of 1 mole of nitrogen gas in a fixed volume container has a pressure of 10 atm and a temperature of 300 K. If the temperature is increased to 500 k, what is the resulting pressure due to the temperature increase?

The combined gas law states that for a fixed amount of gas, the quantity PV/T' is constant. This is often expressed by the equation P₁V₁/T₁ = P₂V₂/T₂ where P is the pressure, V is the volume, and T is the temperature, and the subscripts 1 and 2 denote two different conditions. Rearrange the combined gas law to solve for T₂. A gas with an initial pressure of 2.05 atm, an initial temperature of 215 K, and an initial volume of 15.6 L is heated. The final pressure of the gas is 5.52 atm and the final volume of the gas is 12.8 L. What is the final temperature (T₂) of the gas?

A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15 °C. What is the volume of the bubble when it reaches the surface where the pressure is 1.0 atm and the temperature is 27 °C, if the amount of gas does not change? A) 630 mL B) 110 mL C) 1100 mL D) 580 mL

A pycnometer is a glass apparatus used for accurately determining the density of a liquid. When dry and empty, a certain pycnometer had a mass of 27.059 g. When filled with distilled water at 25.0°C, it weighed 36.634 g. When filled with chloroform (a liquid once used as an anesthetic before its toxic properties were known), the apparatus weighed 41.243 g. At 25.0°C, the density of water is 0.99704 g/mL. a) What is the volume of the pycnometer? (b) What is the density of chloroform?

One mole of triatomic vapours of an unknown substance effuses 1/2 times of 1 mole of O₂ under identical conditions. If the density of unknown vapours at pressure P and temperature T is d, which of the following statement(s) is/are correct for the unknown substance? (A) Density at NTP = 5.71 g/L (B) z(compressibility factor) = 15P/4dRT (C) Vapour density = 64 (D) Vapour density = 16

Which law states that the volume of a gas is proportional to the moles of the gas when pressure and temperature are kept constant? A. Boyle's law B. Dalton's law C. Charles's law D. Avogadro's law

A weather reporter on TV reports the barometer pressure as 27.8 inches of mercury. Calculate this pressure in the following units: a. Pressure = ___ atm b. Pressure = ___ torr c. Pressure = ___ psi d. Pressure = ___ bars

Calculate to three significant digits the density of sulfur tetrafluoride gas at exactly 5 °C and exactly 1 atm. You can assume sulfur tetrafluoride gas behaves asan ideal gas under these conditions.

Chlorine pentafluoride gas is collected at 23.0 °C in an evacuated flask with a measured volume of 45.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.440 atm. Calculate the mass and number of moles of chlorine pentafluoride gas that were collected.

The pressure of a sample of nitrogen gas, N2, is 3.40atm at 314K. What will be the new temperature, in Kelvin, If the pressure is changed to 912mmHg? If needed: R = 0.0821 L atm/K mole and 1.000atm = 760.0mmHg

If the absolute temperature of a gas is quadrupled, what happens to the root-mean-square speed of the molecules? A. Nothing happens to the rms speed. B. The new rms speed is 16 times the original rms speed. C. The new rms speed is 4 times the original rms speed. D. The new rms speed is 2 times the original rms speed. E. The new rms speed is 1/4 the original rms speed.

A gas can is found to have a volume of 10400 milliliters. Set up the problem below and calculate the volume of the gas can in cubic centimeters, cm³. 10400 mL X __ / ___ = ___ cm3