What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0316 grams of magnesium generates 31.53 mL of hydrogen at 22.6 °C with a hydrogen partial pressure of 762.6 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure.     23.1 g/mol

Solid potassium chlorate, KCIO3, decomposes upon heating to form potassium chloride and oxygen gas. Write a balanced chemical equation for the reaction. The volume of oxygen that would form at standard temperature and pressure if 0.456 g KCIO3 decomposes is mL. Answer must be verified.

An empty flask weighs 130.084 g. After vaporization of a sample of volatile liquid at a temperature of 100.0 °C, the flask was sealed, cooled to room temperature, and found to have a mass of 130.316 g. The atmospheric pressure was 759.7 mm Hg. The flask was rinsed and completely filled with water at 18.0 °C. The mass of the water-filled flask was determined to be 379.551 g. What is the pressure of the gas that fills the flask in atmospheres? (Enter your answer as a number without units.)

Given the following data from the experiment, calculate the molar volume of hydrogen gas at STP. Be sure to show all of your calculations. Note: You can assume the solution level was the same inside and outside of the tube at the end of the experiment.  Mass of metal used : 0.0862 g Temperature of the gas collected : 24.0 °C Vapor pressure of water at 24 °C : 22.4 torr Volume of gas collected : 89.4 mL Room atmospheric pressure : 757 torr Gas constant : 0.0821 L • atm / K • mol

HCl(g) can be made by the direct reaction of H2 and Cl2 in the presence of light. 6.00 g of H2 and 1.50 x 102 g Cl2 are mixed in a 5.00 L flask at 28.0 °C. What are the partial pressures of gases after the reaction has completed. Given Information:             > Temperature and volume remains constant at 28.0 °C             > Wavelength of light needed for the reaction is 340 nm.

What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0204 grams of magnesium generates 20.54 mL of hydrogen at 24.6 °C with a hydrogen partial pressure of 761.7 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure. O25.9 g/mol O26.0 g/mol O 24.2 g/mol 23.8 g/mol O 20.9 g/mol

a sample of KClO3 (Mw = 122.55 g/mol) allowed to decompose in presence of MnO2. The resulting oxygen gas that is produced displaces 68.9 mL of water. The temperature of the water is 22.7oC and the barometric pressure is 745.9 mmHg. The vapor pressure of water at 22.7oC is 22.6 mmHg. Calculate the mass of KClO3 that decomposed. 2 KClO3(s) => 2 KCl(s) + 3 O2(g)

Calculate the volume occupied by 25.8 g of methane gas (CH4) at 28°C and 1.0 atm (R = 0.0821 L·atm·K-1·mol-1). 0.039 L 8.7 L 39.8 L 99.2 L 59.7 L

A particular balloon can be stretched to a maximum surface area of 1257 cm². The balloon is filled with 3.2 L of helium gas at a pressure of 759 torr and a temperature of 310 K. The balloon is then allowed to rise in the atmosphere. Assume an atmospheric temperature of 273 K and determine at what pressure the balloon will burst. (Assume the balloon to be in the shape of a sphere.) Express your answer using two significant figures. 15] ΑΣΦ P = 0.22 Submit Previous Answers Request Answer ? X Incorrect; Try Again; 5 attempts remaining atm

When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete - the lime absorbs CO₂ from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 550. L and heated to 520.0 °C. When the amount of CaCO3 has stopped changing, it is found that 8.46 kg have disappeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 520.0 °C. Round your answer to 2 significant digits. P Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. 0 X