A 0.0665 g sample of aluminum metal reacts with hydrochloric acid to give 90.5 mL of hydrogen gas at 23 oC and an atmospheric pressure of 756 mm Hg. The hydrogen gas is collected over water. Write a balanced chemical equation for the reaction between solid aluminum metal and aqueous hydrochloric acid. Using stoichiometry, determine the theoretical yield of hydrogen gas (in moles) that will be produced by the complete reaction of the aluminum metal. Refer to Table 1 and calculate the partial pressure of hydrogen gas. Temperature Pressure Temperature Pressure Temperature Pressure 16 °C 14 mm Hg 21 °C 19 mm Hg 26 °C 24 mm Hg 17 °C 15 mm Hg 22 °C 20 mm Hg 27 °C 25 mm Hg 18 °C 16 mm Hg 23 °C 21 mm Hg 28 °C 26 mm Hg 19 °C 17 mm Hg 24 °C 22 mm Hg 29 °C 27 mm Hg 20 °C 18 mm Hg 25 °C 23 mm Hg 30 °C 28 mm Hg Using the Ideal Gas Law, determine the experimental moles of hydrogen gas collected.
A 0.0665 g sample of aluminum metal reacts with hydrochloric acid to give 90.5 mL of hydrogen gas at 23 oC and an atmospheric pressure of 756 mm Hg. The hydrogen gas is collected over water. Write a balanced chemical equation for the reaction between solid aluminum metal and aqueous hydrochloric acid. Using stoichiometry, determine the theoretical yield of hydrogen gas (in moles) that will be produced by the complete reaction of the aluminum metal. Refer to Table 1 and calculate the partial pressure of hydrogen gas. Temperature Pressure Temperature Pressure Temperature Pressure 16 °C 14 mm Hg 21 °C 19 mm Hg 26 °C 24 mm Hg 17 °C 15 mm Hg 22 °C 20 mm Hg 27 °C 25 mm Hg 18 °C 16 mm Hg 23 °C 21 mm Hg 28 °C 26 mm Hg 19 °C 17 mm Hg 24 °C 22 mm Hg 29 °C 27 mm Hg 20 °C 18 mm Hg 25 °C 23 mm Hg 30 °C 28 mm Hg Using the Ideal Gas Law, determine the experimental moles of hydrogen gas collected.
A 0.0665 g sample of aluminum metal reacts with hydrochloric acid to give 90.5 mL of hydrogen gas at 23 oC and an atmospheric pressure of 756 mm Hg. The hydrogen gas is collected over water. Write a balanced chemical equation for the reaction between solid aluminum metal and aqueous hydrochloric acid. Using stoichiometry, determine the theoretical yield of hydrogen gas (in moles) that will be produced by the complete reaction of the aluminum metal. Refer to Table 1 and calculate the partial pressure of hydrogen gas. Temperature Pressure Temperature Pressure Temperature Pressure 16 °C 14 mm Hg 21 °C 19 mm Hg 26 °C 24 mm Hg 17 °C 15 mm Hg 22 °C 20 mm Hg 27 °C 25 mm Hg 18 °C 16 mm Hg 23 °C 21 mm Hg 28 °C 26 mm Hg 19 °C 17 mm Hg 24 °C 22 mm Hg 29 °C 27 mm Hg 20 °C 18 mm Hg 25 °C 23 mm Hg 30 °C 28 mm Hg Using the Ideal Gas Law, determine the experimental moles of hydrogen gas collected.
A 0.0665 g sample of aluminum metal reacts with hydrochloric acid to give 90.5 mL of hydrogen gas at 23 oC and an atmospheric pressure of 756 mm Hg. The hydrogen gas is collected over water.
Write a balanced chemical equation for the reaction between solid aluminum metal and aqueous hydrochloric acid.
Using stoichiometry, determine the theoretical yield of hydrogen gas (in moles) that will be produced by the complete reaction of the aluminum metal.
Refer to Table 1 and calculate the partial pressure of hydrogen gas.
Temperature
Pressure
Temperature
Pressure
Temperature
Pressure
16 °C
14 mm Hg
21 °C
19 mm Hg
26 °C
24 mm Hg
17 °C
15 mm Hg
22 °C
20 mm Hg
27 °C
25 mm Hg
18 °C
16 mm Hg
23 °C
21 mm Hg
28 °C
26 mm Hg
19 °C
17 mm Hg
24 °C
22 mm Hg
29 °C
27 mm Hg
20 °C
18 mm Hg
25 °C
23 mm Hg
30 °C
28 mm Hg
Using the Ideal Gas Law, determine the experimental moles of hydrogen gas collected.
Calculate the % yield of the reaction based on the actual yield (d) and the theoretical yield (b) calculations above.
Definition Definition Any of various laws that describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. At a constant temperature, the pressure of a particular amount of gas is inversely proportional with its volume (Boyle's Law) In a closed system with constant pressure, the volume of an ideal gas is in direct relation with its temperature (Charles's Law) At a constant volume, the pressure of a gas is in direct relation to its temperature (Gay-Lussac's Law) If the volume of all gases are equal and under the a similar temperature and pressure, then they contain an equal number of molecules (Avogadro's Law) The state of a particular amount of gas can be determined by its pressure, volume and temperature (Ideal Gas law)
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