Homework Answers
The volume of H2 = 243mL = 0.243 L
Pressure of H2 gas collected = 745 mm
Pressure of H2 dry gas = P of H2 collected - vapor pressure of water = 745- 23.78 = 721.22 mm
= 721.22mm /760mm/atm
Temperature = 25C = 25+273= 298 K
Using the ideal gas equation
PV = nRT
or PV = (mass/molar mass) RT
(721.22/760)atm x 0.243L = (mass/ 2g/mol) x 0.0821L.atm/mol.K x 298K
Thus mass of H2 formed = 0.0188 g
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INSTRUCTION: Give your answers in the space provided. You MUST show your work to get credit...
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need all questions answered please !!!!!!
1. The following reaction is used to generate hydrogen gas in the laboratory: Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g). If 243 mL of hydrogen gas is collected at 25°C and has a total pressure of 745 mm Hg, calculate the mass of hydrogen produced. Vapor pressure of water at 25°C is 23.78 mm Hg. (2 Pts.) 2. Sulfurous acid can form water and sulfur dioxide upon heating. How much sulfur dioxide is formed...
6. The following reaction is used to generate hydrogen gas in the laboratory. If 85.7 ml...
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A-D
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need all questions answered please !!!!!!
1. The following reaction is used to generate hydrogen gas in the laboratory: Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g). If 243 mL of hydrogen gas is collected at 25°C and has a total pressure of 745 mm Hg, calculate the mass of hydrogen produced. Vapor pressure of water at 25°C is 23.78 mm Hg. (2 Pts.) 2. Sulfurous acid can form water and sulfur dioxide upon heating. How much sulfur dioxide is formed...
6. The following reaction is used to generate hydrogen gas in the laboratory. If 85.7 ml of gas is collected at 21°C and has a total pressure of 767 mm Hg, what mass of hydrogen (in grams) is produced? A possibly useful table of water vapor pressures is provided below. Mg(s) + 2 HCl(aq) - MgCl2(aq) + H2(g) I(C) P (mm Hg) 20 17.55 25 23.78 30 31.86
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please show work
How many grams of HCl, are needed to produce 125 ml of carbon dioxide gas at STP in the following reaction? CaCO3(s) + 2 HCl(aq) - -> CaCl(aq) + CO2(g) + H20(1) In a reaction similar to this laboratory experiment, 0.625 g of aluminum metal was completely consumed and the H, gas collected over water at 55.0°C and atmospheric pressure of 759 mm Hg. What was the volume of H, gas produced? (Be sure to correct H2...
Suppose you are performing a gas-producing reaction to experimentally determine the molar volume of the gas at STP. Mg(s) + 2 HCl(aq) + MgCl2 (aq) + H2(g) A sample of 0.0883 g of Mg, which has a molar mass of 24.31 g/mol, produces 82.5 mL of H2 gas. The gas is collected over water at an atmospheric pressure of 774.5 mm Hg at 22 °C, at which the vapor pressure of water is 19.8 mm Hg. What is the experimental...
A-D
A student performed an experiment in which they collected hydrogen gas from the reaction of magnesium with hydrochloric acid using the same apparatus that you will be using in today's lab. The reaction is: Mg(s) + 2 HCl(aq) → H2(g) + MgCl2 (aq) The data they collected are shown below: Mass of Mg Volume of HCI Volume of H2 collected Temperature of H2 collected Barometric pressure 0.100 g 10 mL 57.5 mL 22 °C 29.94 in Hg a. Barometric...
Calculate the gas constant, R O Convert your measured temperature to Kelvin and record it in your Notebook. Using the table found under "Resources," determine the vapor pressure of water at your measured temperature. Record the water vapor pressure in your Notebook. Calculate the pressure of hydrogen gas produced from your reaction. This will be the difference between the atmospheric pressure and the vapor pressure of water at your measured temperature. Record the hydrogen gas pressure in your Notebook. For...
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