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Temperature °C Water Vapor Pressure (mmHg) Magnesium metal is reacted with hydrochloric acid to produce hydrogen...
Station 2: Calculations with the Ideal Gas Law A Station Letter: A student reacted a strip of magnesium metal with 4.00 mL of 4.0 M hydrochloric acid and collected the hydrogen gas produced using the experimental setup you see at the station. Unfortunately, the student forgot to record the mass of the metal before they reacted it with acid. Determine the mass of the magnesium metal the student used in the experiment. For this experiment assume the pressure of the...
Data Sheet Unknown Number Sample 2 Sample 1 Volume of Ha gas (ml.) 22.65 22.12 Temperature of water (C) 20 8 0 20.8 C Height of water column (mm) 324.9 210.2 Vapor pressure of water at above temperature (mmlig) 7.5 17.5 Barometric pressure (mmHg) 747.776 구4구. 구구6 CALCULATIONS (Show calculations) Pressure ofthe column of water (mmHg) Pressure of dry hydrogen (mmHg) Moles of Hydrogen Mass of Magnesium ribbon (g) Average mass of magnesium ribbon (g) Vapor Pressure of Water at...
Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s)+ 2HCIaq) ZnCh(aq)+H() The product gas, He, is collected over water at a temperature of 20 °C and a pressure of 760 mm Hg. If the wet H gas formed occupies a volume of 7.53 L, the number of moles of Zn reacted was Hg at 20 °c mol. The vapor pressure of water is 17.5 mm
zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCl(aq)ZnCl2(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 20 °C and a pressure of 745 mm Hg. If the wet H2 gas formed occupies a volume of 9.32 L, the number of moles of Zn reacted was __mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.
14. The reaction of magnesium metal with hydrochloric acid produces hydrogen gas as a product. I would like to collect 125 mL of hydrogen gas from the experiment. The temperature of the lab is 23.5°C and the pressure is 762 mmHg. How many grams of magnesium metal should I use if the hydrochloric acid is kept in excess? Mg(s) + 2 HCl(aq) MgCl2(aq) + H2(g)
-REPORT FO SECTION DATA Mass of magnesium strip: 2402 Temperature of water from the thermometer: 71 3705 Atmospheric pressure (inches) 29.3Sx 2513 Volume of gas collected: CALCULATIONS: (Show work) 20 94A0つ Moles of magnesium: OS10X 24.30 2.094316 3 Moles of hydrogen produced 12 29215K Temperature of gas in Kelvins: Volume of hydrpgen gas in liters: Atmospheric pressure (mm. Hg): Vapor pressure of water in eudiometer: Pressure of hydrogen gas in eudiometer (mm.Hg.): Pressure of hydrogen gas (atmosphere): Calculated value of...
Consider the reaction of magnesium metal with hydrochloric acid to produce magnesium chloride and hydrogen gas. If 4.34 mol of magnesium and 4.34 mol of hydrochloric acid are reacted, how many moles of hydrogen gas are produced? a. 8.68 mol b. 2.17 mol c. 4.34 mol d. 6.34 mol e. none of these
Magnesium metal reacts with hydrochloric acid to give hydrogen gas. Mg + 2 HCl → MgCl2 + H2 Use the following reaction information to answer the subsequent questions. Show all of your work. 92 mm Length of Magnesium ribbon: Barometric Pressure: 762.9 mmHg Water Temperature: 29 °C Initial Gas Volume: 0.00 mL Final Gas Volume: 67.35 mL 0.7559 Mass = Length (in mm) x (1000 mm) 1. Magnesium is usually found in the laboratory as a ribbon strip. Find the...
Date: 7 Record the barometric pressure. 8. Repeat this experiment with the second piece of magnesium ribbon. 9. Untwist the wire from the piece of fiberglass. Rinse the wire, fiberglass square, and stopper, place them in the container, and return the container to the instructor's desk. The table of temperature/Vapor pressure of water is in your textbook and in the back of your laboratory manual. The density of mercury is 13.6 g/mL. 61302083 Data Sheet Unknown Number Sample 2 40.8m2...
2. A 0.865g sample of an unknown metal (X) reacted with hydrochloric acid according to the balanced chemical equation shown below. XC12 (aq) + H2() X+ 2 HCl(q) The volume of the hydrogen gas collected over water was measured at 191 mL at 22C and an atmospheric pressure of 762 mmHg. Calculate the molar mass of the unknown metal, and use a periodic table to identify the metal. Molar mass: The metal is 127