50 > A 0.775 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H,SO,(aq) → MSO,(aq) + H,(g) A volume of 301 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. Calculate the molar mass of the metal. g/mol 63.29 molar mass: Question Source: MRG-General Chemistry | Publisher: Univer help contact us terms of use wbout os privacy policy careers MacBook Pro

50 > A 0.775 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H,SO,(aq) → MSO,(aq) + H,(g) A volume of 301 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. Calculate the molar mass of the metal. g/mol 63.29 molar mass: Question Source: MRG-General Chemistry | Publisher: Univer help contact us terms of use wbout os privacy policy careers MacBook Pro

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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pressure remains constant.
What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0278 grams of magnesium generates 28.92 mL of hydrogen at 22.2 °C with a hydrogen partial pressure of 727.5 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure. In the lab, you used 2.0 mM FD&C Red Dye No. 40 solution. How much solid dye, molar mass 496.42 g/mol, should be dissolved to make 8.20 liters of 8.61 mM FD&C Red Dye No. 40 solution? Hint, 2.0 mM is 0.0020 M.
The "air bags" that are currently installed in automobiles to prevent injuries in the event of a crash are equipped with sodium azide, NaN3, which decomposes when activated by an electronic igniter to produce nitrogen gas that fills the bag. How many liters of nitrogen, measured at 25 °C and 1.00 atm, will be produced by 100.0 g of NaN3? Equation: 2NaN3(s) → 2Na(s) + 3N2(s)
1.) This reaction occurs in large test tube at 32.0oC: 2 Al (s) + 3 H2SO4(aq) ---> 6 H2 (g) + Al2(SO4)3 (aq) A tube going through the stopper of the test tube feeds into a graduated cylinder that has been inverted in a tub of water. At the end of the reaction, the total pressure of gas in the inverted cylinder is 435. torr, and the volume of gas collected is 455. mL. What mass of aluminum must have reacted? P.s- please show how you got it. I get confused with it
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 910.0 °C. When the amount of CaCO3 has stopped changing, it is found that 567. g have disappeared. P Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 910.0 °C. Round your answer to 2 significant digits. 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. K-0 P
If 8g of ammonium hydroxide is completely decomposed by the reaction below in a closed container with a total volume of 5.00L and at 25°C, what will be the partial pressure of the ammonia gas liberated, in atmospheres? Assume the volume of the liquid is negligible. NH4OH(aq) --> H2O(l)+NH3(g)
Gases are different from solids and liquids. In a sample of gas, the molecules are far apart. The gas molecules also move around and collide with each other as well as with the walls of the container. These collisions generate pressure. The pressure of a gas can be measured in different units. One convenient unit of measure is called the atmosphere (atmatm) because it is based on atmospheric pressure. At sea level, the average pressure is 1 atmatm. As you get higher in altitude, the pressure steadily drops until you leave the atmosphere, where the pressure is very close to 0 atmatm. The table below shows the different commonly used units of measuring gas pressure. Use this table in the pressure unit conversions. Unit Abbreviation 1 atm equivalent atmosphere atmatm 1.00 atmatm (exact) millimeters of mercury mmHgmmHg 760 mmHgmmHg torr torrtorr 760 torrtorr inches of mercury in.Hgin.Hg 29.9 in.Hgin.Hg pounds per squareinch (psi) lb/in.2lb/in.2 14.7 lb/in.2lb/in.2 pascal…
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Given the reaction: 2 Al (s) + 6 HCI (aq) --> 2 AICI3 (aq) + 3 H2 (g) A strip of aluminum of unknown mass is reacted with excess hydrochloric acid. When the hydrogen gas is collected over water, it is done so at a temperature of 22.0 °C and fills a flask of volume 43.9 mL. The pressure inside the collection tube is 751.5 mmHg and the water vapor pressure at 22.0 °C is 19.83 torr. Determine the mass of the aluminum strip in milligrams (mg).
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EXERSICE 7 (A) Let A and B be two ideal gases at the same temperature. If mÃ>m³ (where mÃ, m³ are the masses of molecules of gases A and B, respectively) and EA, E, the average kinetic energies of the two gases, choose the correct phrase, giving a justification. (1) EA = EB (ii) EA > EB (iii) EA < EB (iv) Data are insufficient to compare EA, EB.
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