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# Gas Laws

### Total Volume of Gas Collected

Potassium chlorate, KClO3, decomposes when heated: KClO3 (s) ® KCl (s) + 3/2 O2 (g) 1.00 gram of potassium chlorate is completely decomposed and the oxygen is collected over water at 25°C and 0.99 atm. Calculate the total volume of gas collected. (The vapor pressure of water at 25°C is 23.8 torr).

### Density of 275 l h2 @ 850mmHg and 30*c

What is the density of H2 contain in a 2.75 l vessel at 850mmHg and 30.0*C?

### Calculating Volume at STP

In different containers, you have 9.0 g of water vapor(assume this is possible), 16 g of HC4, and 44.0 g of carbon dioxide, all under standard conditions of temperature and pressure. Calculate the volumes and tell which occupies the smallest volume.

### Determining the volume inside a bulb w/ a gas in it

An ideal gas at 650 mm Hg pressure occupies a bulb of unknown volume. A certain amount of the gas was withdrawn and found to occupy 1.52 mL at 1.00 atm. The pressure of the remaining gas in the bulb was found to be 600 mm Hg. Assuming that all the measurements were made at the same temperature, calculate the volume of the bul

### Calculations for decompositions of a solid using gas laws under STP. How to use molecular masses and the given equation to find out the solution.

What volume of carbon dioxide at STP is produced by the complete decomposition of 24 g of CaCO3--2.69 dm3, 4.64 dm3,5.37 dm3, 7.68 dm3 To solve the question we write down the equation of the reaction: CaCO3 -----> CO2 + CaO This equation is balanced out. The number of atoms of every element is the same on the le

### Finding excess reactant

If 23.96 kg of iron(III) oxide are combined with 11200 dm3 of carbon monoxide at STP, which substance would be the excess reactant--iron oxide, carbon monoxide, iron, carbon dioxide

### Calculation using gas law

Given 20g potassium chlorate, how many cubic decimeters of oxygen would be produced at STP 2 KCLO3----> 2 KCL(cr) + 3O2(g)

### Calculating number of molecules in a container

How many molecules of N2 are in a 500mL container at 780mm Hg and 135 degrees celsius? What formula/s do I use?

### Calculate the number of molecules present.

I want step by step instructions on how to do problem please.

### Vapor Pressure, Compressibility Factor and Combustion

When 8.21L of C4H10(g) (butane) are burned in oxygen, how many liters of O2(g) are consumed? Both gases are held at 324.5 K and 12.23 atm. Ans: 53.37 ------------------------- Pure Acetone (CH3COCH3) has a vapor pressure of 324.0 torr at room temp. What's the closest value to the molality of a solution of a nonvolatile s

### Maxwell Distribution

Plot the Maxwell distributions for CO2, N2, and He at 298K in the velocity range of 0 to 2500 m/s. Label each curve appropriately. What temp. would you have to change the CO2 to cause it to have the same mean velocity as the He at 298K? What fraction of the N2 molecules are in the velocity range 500 to 1000 m/s? What is the

### Volume and Pressure

1. What is the volume of a quantity of a gas at 172 Celcius, if its volume is 262 mL at -25 Celsius and the pressure remains constant. 2. What is the pressure, in inches of mercury, of a gas that originally had a volume of 252 mL, under a pressure of 0.834 atmosphere and a temperature of 45 Celsius if the volume is reduced to

### Pressure and Volume using Boyle's Law

A sample of nitrogen has a volume of 50 L at a pressure of 760. mmHg. What is the volume of the gas at each of the following pressures if there is no temperature change. A. 1500 mmHg (I have solves the problem for A!) B. 2.0 atm. C. .500 atm According to my text book, the answers for P3 and P4, are 25 L and 100.

### Need to know how to set up a problem with changes in pressure without knowing volume.

The problem is this.... A gas with a volume of 4.0L is contained is a closed container. Indicate the changes in pressure when the volume undergoes the following changes at a constant temperature. A. The vloume is compressed to 2 L. B. The vloume is allowed to expand to 2 L. C. The volume is copmressed to .40 L. (Thi

### General Chemistry: Gas Laws

A 36.4 liter volume of methane gas is heated from 25 °C to 88 °C at constant pressure. What is the final volume of the gas?

### Volume of an Ideal Gas

What is the volume of 0.5 moles of an ideal gas at a pressure of 1.5 atm and a temperature of 5.0 degrees C?

### What is the density of oxygen at 45 degrees Celsius?

What is the density of oxygen at 45 degrees celcius?

### Gas mixtures and movements

The following reaction takes place in a sealed 40.0-L container at a temp of 120 degrees C 4NH 3(G) + 5 O2 (g) --> 4NO (g) + 6H2O (G) a) When 34.0g of NH3 reacts with 96.0g of O2 what is the partial pressure of NO in the sealed container? b) What is the total pressure in the container?

### Ideal gas law: What volume of O2 (g) is consumed in the combustion of 125g of gaseous dimethyl ether (CH3)2) ?

What volume of O2 (g) is consumed in the combustion of 125g of gaseous dimethyl ether (CH3)2) if both gas volumes are measured at the temperature and pressure at which the density of dimethyl ether is 1.81g/l?

### What volume of oxygen gas is required to burn 0.5562 of propane gas C3H8 if both gases are measured at the same temperature?

What volume of oxygen gas is required to burn 0.5562 of propane gas C3H8 if both gases are measured at the same temperature?

### Ideal gas Law Ideal Gas Law and Hydrogen

A 2.02 gram sample of Al reacts with excess Hcl(aq) and the hydrogen produced is collected over the aqueous solution at 24 degrees Celsius. What is the total volume of hydrogen collected at barometric pressure of 760.000 Torr? (Include VP) Assume VP of the solution is the same as the VP of pure water. 2 moles Al(s) + 6 mol

### Ideal Gas Law and Aqueous Hydrogen Peroxide

A 100.0 gram sample of aqueous hydrogen peroxide decomposes over time to make 3.31 L of O2(g) at 21 degrees Celsius and 715 Torr. What must the mass percentage of H2O2 is the solution? (Ignore the VP of H2O). 2 moles of H2O2 -----> 2 moles of H2O(l) + O2(g)

### Ideal Gas Law for Liquid Hydrocarbon

A liquid hydrocarbon (contains only C and H) is found to have 16.37% H by mass. A 1.158 gram sample has a volume of 385 ml at 71 degrees Celsius and 749 Torr. What is the molecular formula of the hydrocarbon?

### Grand Canonical Partition Function

For the grand canonical ensemble we've obtained two expressions for the pressure: P = (k_B)(T)/Vln(x) or P = (k_B)(T)(dln(x))/dV_Bu,B where is the grand canonical partition function. Check that the derivative does not give the first expression exactly. Nonetheless, the pressure calculated in the two ways agree - at least

### Canonical Partition Function Q(N, V, T)

An approximate canonical partition function for a dense gas is: Q(N, V, T) = 1/N! [2(pi)(mk_nT / h^2]^3N/2 (V - Nb)^Nexp[(alphaN^2/Vk_BT)]. Where m is the mass of the particles and a and b are molecular parameters (which are independent of temperature). Calculate the energy, entropy, pressure, and chemical potential for

### Equilibrium and Reactions

Question 1 At 100oC, the equilibrium constant, KC, for the reaction COCl2(g) ?---? CO(g) + Cl2(g) has a value of 2.19 x 10-10. Is the following mixture at equilibrium? If not, indicate the direction in which the reaction must proceed to achieve equilibrium. [COCl2] = 5.00 x 10-2 M, [CO] = [Cl2] = 3.31 x 10-6 M Question 2

### Hydrogen Gas Problem Using the Ideal Gas Law

Consider a vehicle powered by hydrogen gas. a. About 3.1 kg of H2 is required for a vehicle to have a 500 km range. Assume ideal gas behavior and a storage tank of 60 L (a comparable size to conventional gasoline vehicles). What tank pressure atm might one expect at 25 degrees celsius? b. Since their discovery in 1991, tin

### Partial Pressure of Products and Reactants

A 10.0 L tank contains nitrogen gas and chlorine gas at partial pressure of 1.00 atm each, at a temperature of 300K. The mixture is allowed to react, producing nitrogen trichloride. Calculate the partial pressures of the products and reactants.

### Ideal Gas Law: Bromine and Fluorine

1) Bromine gas reacts with flourinne gas to give a low boiling liquid. A sample of this liquid is vaporized at 42.0 degrees C into a flask with a volume of 252.2mL. The atmospheric pressure is 726.3 torr. The flask is found to contain 1.632 g of the compound. a) Calculate the formula weight of the compound. b) Is the co

### Finding NaNO2 Required to Produce N2 Under Given Conditions

Show the calculation for the mass of NaNO_2 required to produce 40. mL of N_2 with a temp. of 25.6 degrees C and an atm. pressure of 739 mmHG. Please give a good simple step by step solution on how to solve the problem.