What is the partial pressure of oxygen gas produced if 8.42 g of hydrogen peroxide decomposes at 22 degrees C into a container with a fixed volume of 3.78 L (assuming no oxygen is initially present)? 2H2O2 --> 2 H2O +O2
1. Chlorine gas occupies a volume of 1.20 liters at 725 torr pressure. What volume will it occupy at 1 atm pressure? 2. Fluorine gas exerts a pressure of 975 torr. When the pressure is changed to 1.50 atm, its volume is 250 mL. What was the original volume? 3. Helium occupies a volume of 3.80 Liters at -45 C. Wh
Mole and Mass relationship in chemical equation: 1. What mass of ammonia, in grams, can be made from 440g of H2? N2+3H2-2NH3 The combined Gas Law: 1.If the gas present in 4.65L at STP is changed to a temperature of 15C and pressure of 756mmHg, what will be new volume? The Ideal Gas Law: 1. Calculate the
1. A diver at a depth of 100 ft (pressure approximately 3 atm) exhales a small bubble of air with a volume equal to 100 mL. What will be the volume of the bubble (assume the same amount of air) at the surface? 2. What would the volume of gas contained in an expandable 1.0 L cylinder at 15 MPa (1MPa = 10^6 Pa) be at 1 atm (assum
One mole of argon gas inside a cylinder fitted with a piston is made to expand very slowly in good thermal contact with its surroundings. During this expansion the volume was doubled and the temperature was constant. The same expansion is performed very rapidly with the cylinder being thermal isolated. The conditions were contro
A sample of ammonia gas with a volume of 7.0 mL at a pressure of 1.68 atm is compressed to a final volume of 2.7 mL at constant temperature. Use the ideal gas law to calculate the final pressure. a. 100 atm b. 2.2 atm c. 1 atm d. 4.4 atm
It is found that 250 ml of gas at STP has a mass of 1.00 gram. What is the molar mass? a. 89.6 gram/mol b. 28.0 gram/mol c. 14.0 gram/mol d. 22.4 gram/mol
Please show all work. 1.)(Ideal Gas Law) How many moles of chlorine atoms are there in a container that holds 1.529 kg of XCl5 gas (where X = unknown element) at 600.5°C at a pressure of 1213 torr? The density of the gas is 4.63 g/L. 2.) (Ideal Gas Law) A chemist carries out a reaction and isolates a gaseous product.
We wish to double the volume of a gas held at constant pressure. To what temperature must we heat it if its original temperature was (a) 0^oC, (b) 100^oC, and (c) 1000^oC? I believe the answer is a) 546 K, b) 746 K and c) 2546 K. I need to see each step and formula to solve this question.
A nitrogen container has 100.0 liters of gas at a pressure of 3200 psi ruptures in a room at 28° C and 0.92 atm pressure. What volume will the nitrogen gas occupy in the room after the bottle empties? Please show all steps. 2 A typical vacuum system can obtain a pressure of 1.0 x 10-8 (-8 power) torr. Calculate the numbe
1.86 moles of a gas occupies 245L at 281 degrees C with a pressure of 0.63 ATM. The pressure is increased to 886 ATM with the same temp. What is the volume?
In most general chemistry courses, students calculate the molar mass (MM) of a volatile liquid using the ideal gas law (PV = nRT) in the following form: MM = (mass of vapor*R*boiling point in Kelvins)/(pressure in atmospheres*flask volume). If R = 0.0821 liter-atmospheres/mole-degree K, the flask volume is 550 ml, the pressure i
See the attachment.
See the attachment. 6. In the reaction of copper with concentrated nitric acid, the products are copper (II) nitrate, water and nitrogen monoxide, sometimes called nitric oxide. If 150 ml of nitric oxide were collected over mercury at 42C and under a pressure of 74.5 cm of mercury, how many grams of copper had reacted?
3. The solubility of laughing gas, dinitrogen monoxide, in water is 7.50 mg per cent by mass at 760 Torr and 25C. If the density of the resulting solution is 1.01 grams per milliliter, what is the morality of the resulting solution? What is the % of the volume?
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
1. How many grams of oxygen are required to fill a 4.5 x 103 liter hyperbaric chamber at a pressure of 225 cm Hg and 62 F?
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
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
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.
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