### Application of ideal gas equation, mole and mass calculation.

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Any number of green plants can photosynthesize glucose (C6H12O6) in the presence of carbon dioxide and water, and producing oxygen as the remaining product. 250 ml of oxygen was produced. The oxygen was collected over water at 27C and at a pressure of 755 Torr. The vapor pressure of water at 27C is approximately 26mm Hg. What

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Ideal gas equation, mole, temperature conversion, pressure conversion, % weight.

Production of ethyne, ideal gas equation's application, Temperature conversion: Celcius to Kelvin, Pressure conversion: mm Hg to Pascal, mole and volume calculation.

The density of benzene vapor at 100 C* and 650 mmHg is 2.18g/L. Calculate the molecular mass. (Hint D=n(mol. Weight)/vol.=P(mol. Weight)/RT)

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).

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

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.

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 A certain amount of the gas was withdrawn and found to occupy 1.52 mL at 1.00 atm.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

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

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

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

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

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

This is a review for old material that am unfamiliar with ... thanks for your help! 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

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 th

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

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.

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

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?

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 celcius?

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?

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

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

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)

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

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