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
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.
Take a deep breath of air and assume it is one liter of air. What is the probability that the liter of air contains a molecule from Julius Caesar's last breath (also assume a liter of air)? Assume that the nitrogen that existed in the atmosphere ~ 2000 years ago is that which is currently present and that the liter of air has
1) What mass of oxgen gas will occupy 450.mL at 145mmHg and 62.5 degrees Celcius? 2) Find the volume in liters of 52.0g of CO2 at 410mmHg and 99.0 degrees Celcius.
How would you prepare 1.0 L of an aqueous solution of sodium chloride having an osmotic pressure of 25 atm at 17°C?
2C H10 + 21O2 --> 16 CO2 + 10H2O if 950 grams of O2 are used in the above reaction How many Liters od CO2 can be collected @ a Pressure of 700mmhg + Temperature of 47degrees C ?
1. The National Drinking Water standard for lead in water is no more than 0.015ppm. If a particular water supply sample has 5.0x10^-7 moles of Pb per 5.0 liters, is it suitable for drinking? 2. If a gas occupies 625mL at 0oC and 760 torr pressure, what will its volume be at 223oC and 1520 torr pressure? 3. A metal tank of
See Attachment The composition of hydrogen selenide (H2Se) can be determined by heating tin (Sn) in a measured volume of the gas. The hydrogen selenide is decomposed, producing solid tin selenide (SnSe) and hydrogen gas. If the temperature and pressure are unchanged, the gas volume when the decomposition is over is the sa
Keith wants a large helium balloon, his mom can only fit 10.0 L in her small car. The temperature outside is 17.0 The balloon has a mass of 500 g He. What pressure should she have the balloon filled with helium? a) 0.114 kPa b) 2.98 104 kPa c) 1.95 kPa d) 1.14 kPa How to set up the problem - explain in detail (high scho
A sample of gas occupies 135 mL at 22.5 C; the pressure is 165 mm Hg. What is the pressure of the gas sample when it is placed in a 252-mL flask at a temperature of 0.0 C? pressure of gas sample___________________ mmHg Ethane, C2H6, burns in air according to the equation 2C2H6(g) 7 O2(g)---->4CO2(g) + 6H2O(g) Wh
I need need help with the following. A flexible gas storage container has a volume of 3.5 x 10^2 L at a temperture of 27 degrees celcius and a pressure of 115 kPa. What is the new volume if the temperture drops to -10 degrees celcius and the pressure drops to 99 kPa?
I am given the volume (1024ml), pressure (1.2 atm) and temperature (36o C) and I need to determine the number of moles present.
The vapor pressure of water at 22 degrees C is 19.800 torr. If you put 26.662 g of water in a cubic container that is 1.1000 m on an edge, will there be any liquid water remaining in the container at 22 degrees C or will it all be vapor? R = 0.0820578 L*atm/K*mol.
A hydrogen gas thermometer is found to have a volume of 100.0 cm3 when placed in an ice-water bath at 0°C. When the same thermometer is immersed in boiling liquid chlorine, the volume of hydrogen at the same pressure is found to be 87.2 cm3. What is the temperature of the boiling point of chlorine?
The surface temperature of Venus is about 1050K and the pressure is about 75 Earth atmospheres. Assuming that these conditions represent a Venerian "STP", what is the standard molar volume (in liters) of a gas on Venus?
Ozone molecules in the stratosphere absorb much of the harmful radiation from the sun. the temp. and the pressure of ozone in the stratosphere are 250 K and 1.0*10^-3 atm. How many ozone molecules are present in 1.0 L of air under these conditions?
At STP, 0.280L of a gas weighs 0.400g. Calculate the molar mass of the gas.
Understanding how a real gas (eg. van der Waals gas) differs from an ideal gas. Interpreting the pressure-volume behaviour of gases.
In an industrial process, nitrogen has to be heated to 500K at constant volume. If it enters the system at 300 K and 100 atm, what pressure does it exert at its final working temperature? Treat it as a van der Waals gas. Assume the volume is 1 m^3 (where "^" means "to the exponent").
Understanding the properties of gases. Understanding partial pressure of a gas in a mixture, and how partial pressure relates to the mole fraction.
One mole of nitrogen and three moles of hydrogen are injected into a container of volume 10 dm^3 at 298 K. What are the partial pressures and the total pressure? (Note: "^" means "to the exponent".)
Understanding the ideal gas law. Using the ideal gas law to calculate work done as a result of a chemical reaction that generates a gas.
Calculate the work done when 50 g of iron dissolves in hydrochloric acid in (a) a closed vessel and (b) an open beaker. Hint: Use the ideal gas law and equations to determine amount of work done when a gas expands.
What is the density of N2O at STP?
Application of Charles's Law (one of the derived basic gas laws) to calculate volume at a different temperature.
A certain mass of calcium carbide, CaC2, reacts completely with water to produce 64.5 L of acetylene, C2H2, at 50 degrees C and 1 atm. If the same reactants react completely at 300 degrees C and 1 atm, what will be the volume of acetylene?
What is the pressure in a 10 L container that is at 27o C and which contains 3 mol of H2 gas and 8 mol of He gas?
Question: A metal tank of volume 75.5 L will burst if the pressure in it exceeds 50.0 atm. Will this pressure be exceeded by 82.0 moles of a gas in it at 25 degrees Celsius?