A magnesium with a mass of 0.06581 grams was reacted with excess HCl. The reaction produced 51.12 mL of Hydrogen gas at 22°C. The barometric pressure was recorded as 818.1 mm of Hg while water vapor pressure was 21.09 mm Hg. Atomic mass of magnesium metal = 24 grams/mol. Calculate the number of moles of Hydrogen gas. *

What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0327 grams of magnesium generates 34.85 mL of hydrogen at 24.1 °C with a hydrogen partial pressure of 715.2 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure.   A 19.5 g/mol   B 26.2 g/mol   C 22.4 g/mol   D 24.3 g/mol   E 26.0 g/mol

What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0157 grams of magnesium generates 15.92 mL of hydrogen at 23.6 °C with a hydrogen partial pressure of 747.1 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure. 20.4 g/mol 24.4 g/mol 25.1 g/mol 22.1 g/mol 25.2 g/mol

How many grams of water will be lost when 8.000 g of YBr3 .9H2O is heated?

Air entering the lungs ends up in tiny sacs called alveoli. It is from the alveoli that oxygen diffuses into the blood. The average radius of the alveoli is 0.0041 cm, and the air inside contains 14 percent oxygen. Assuming that the pressure in the alveoli is 1.0 atm and the temperature is 37 °C, calculate the number of oxygen molecules in one alveolus. For calculation purposes, assume that the average alveolus is a perfect sphere. Be sure your answer has the correct number of significant digits. Note: Reference the Fundamental Constants table for additional information. 8.486 x 10 10° | molecules x10

Given the following balanced equation, what volume of hydrogen gas (in liters) would be produced under conditions of STP from the reaction of 0.082 grams of magnesium solid reacting with excess hydrochloric acid solution?  Please report your answer WITH the correct number of significant figures, and WITHOUT units. Mg  +  2 HCl  →  MgCl2  +  H2

The atmospheric pressure on a particular day is 726 mmHg. Given that the mole fraction of N2 in air is 0.781, determine the partial pressure of nitrogen (in mmHg).

Calculate the final Kelvin temperature when 5.00 L of fluorine gas at 50 degrees Celsius is cooled to give a volume of 3.75 L.

Ancient Romans built often out of bricks and mortar. A key ingredient in their mortar was quicklime (calcium oxide), which they produced by roasting limestone (calcium carbonate). 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid calcium carbonate (CACO) into solid calcium oxide and gaseous carbon dioxide. 2. Suppose 43.0 L of carbon dioxide gas are produced by this reaction, at a temperature of 250.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Round your answer to 3 significant digits. Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Access MacBook Air 4 F7 II F8 A F10 O F3 9 FR . F6 F5 4.

Three bulbs are connected by tubing, and the tubing is evacuated. The volume of the tubing is 49.0 mL The first bulb has a volume of 58.0 ml and contains 6.07 atm of argon, the second bulb has a volume of 250 ml. and contains 1.62 atm of neon, and the third bulb has a volume of 27.0 ml. and contains 7.72 atm of hydrogen. If the stopcocks (valves) that isolate all three bulbs are opened, what is the final pressure of the whole system in atm? Answer: