Water to prepare 170.3 mL of solution at 26.27°C. The ideal gas constant is 0.0821 L atm/K mol.
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CHEMISTRY · IDEAL GAS LAW CONSTANT INTRODUCTION LABORATORY SIMULATION Lab Data Mass of magnesium (g) 0.020 Moles of magnesium (mol) 0.00082 Temperature of water (°C) 21.0 Temperature of water (K) 294.15 Vapor pressure of water (mmHg) 18.6 Barometric pressure (mmHg) 776.0 Observations pockets of gas being released from magnesium. Volume of hydrogen gas collected (mL) 19.6 Volume of hydrogen gas collected (L) 0.0196 Pressure of hydrogen gas (mmHg) Pressure of hydrogen gas (atm) Moles of hydrogen gas produced (mol) Ideal gas constant (L·atm·mol⁻¹·K⁻¹) How to calculate ideal gas constant Water Vapor Pressure Table METHODS
Adi S.
Gases produced by a chemical reaction can easily be collected over water. To determine the pressure of the dry gas, the vapor pressure of the water at that temperature must be subtracted from the total pressure. 1) Consider the following reaction: Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) The total pressure of gas collected over water is 785.0 mmHg and the temperature is 21.5°C What is the pressure of hydrogen gas formed in mmHg? Pressure = [ ] mmHg
Sri K.
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