Ideal Gas Law for analysis. Preliminary chemical analysis of the metal found it to be trivalent and reactive with strong acids. Henry, a laboratory analyst, took 0.194 g of the metal to determine its identity using the ideal gases experiment. The results of the experiment are reported as follows in his lab notebook: An archaeologist found a chunk of metal and send it to a chemical laboratory Determination of Unknown Metal Using Ideal Gas Experiment mass of unknown metal: 0.194 g barometric pressure (Pbar ): 745 torr Pressure of water vapor: 26.7 torr Temp.: 27 °C Volume of trapped gas: 148 ml height difference of water levels: 11.29 cm A. What is the pressure, in torr, of the dry gas? B. How much moles of hydrogen gas are produced by the reaction? Assuming that the strong acid was in excess. C. What is the identity of the unknown metal M? Assume that the metal is pure. Show your solution.
Ideal Gas Law for analysis. Preliminary chemical analysis of the metal found it to be trivalent and reactive with strong acids. Henry, a laboratory analyst, took 0.194 g of the metal to determine its identity using the ideal gases experiment. The results of the experiment are reported as follows in his lab notebook: An archaeologist found a chunk of metal and send it to a chemical laboratory Determination of Unknown Metal Using Ideal Gas Experiment mass of unknown metal: 0.194 g barometric pressure (Pbar ): 745 torr Pressure of water vapor: 26.7 torr Temp.: 27 °C Volume of trapped gas: 148 ml height difference of water levels: 11.29 cm A. What is the pressure, in torr, of the dry gas? B. How much moles of hydrogen gas are produced by the reaction? Assuming that the strong acid was in excess. C. What is the identity of the unknown metal M? Assume that the metal is pure. Show your solution.
Ideal Gas Law for analysis. Preliminary chemical analysis of the metal found it to be trivalent and reactive with strong acids. Henry, a laboratory analyst, took 0.194 g of the metal to determine its identity using the ideal gases experiment. The results of the experiment are reported as follows in his lab notebook: An archaeologist found a chunk of metal and send it to a chemical laboratory Determination of Unknown Metal Using Ideal Gas Experiment mass of unknown metal: 0.194 g barometric pressure (Pbar ): 745 torr Pressure of water vapor: 26.7 torr Temp.: 27 °C Volume of trapped gas: 148 ml height difference of water levels: 11.29 cm A. What is the pressure, in torr, of the dry gas? B. How much moles of hydrogen gas are produced by the reaction? Assuming that the strong acid was in excess. C. What is the identity of the unknown metal M? Assume that the metal is pure. Show your solution.
Transcribed Image Text:Ideal Gas Law
for analysis. Preliminary chemical analysis of the metal found it to be trivalent and reactive with strong
acids. Henry, a laboratory analyst, took (0.194 g of the metal to determine its identity using the ideal gases
experiment. The results of the experiment are reported as follows in his lab notcbook:
An archaeologist found a chunk of metal and send it to a chemical laboratory
Determination of Unknown Metal Using Ideal Gas Experiment
mass of unknown metal: 0.194 g
barometric pressure (Pbar ): 745 tor
Pressure of water vapor: 26.7 torr
Temp.: 27 °C
Volume of trapped gas: 148 ml
height difference of water levels: 11.29 cm
A. What is the pressure, in torr, of the dry gas?
B. How much moles of hydrogen gas are produced by the reaction? Assuming that the strong acid was
in excess.
C. What is the identity of the unknown metal M? Assume that the metal is pure. Show your solution.
Definition Definition Law that is the combined form of Boyle's Law, Charles's Law, and Avogadro's Law. This law is obeyed by all ideal gas. Boyle's Law states that pressure is inversely proportional to volume. Charles's Law states that volume is in direct relation to temperature. Avogadro's Law shows that volume is in direct relation to the number of moles in the gas. The mathematical equation for the ideal gas law equation has been formulated by taking all the equations into account: PV=nRT Where P = pressure of the ideal gas V = volume of the ideal gas n = amount of ideal gas measured in moles R = universal gas constant and its value is 8.314 J.K-1mol-1 T = temperature
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