A) In an electrochemical cell, a metal anode lost 0.133 g while a total volum of 0.08921 L of hydrogen gas was produced. The temperature was 298 K and the barometric pressure was 742.4 mm Hg. At 298 K, the vapor pressure of water is 23.8 mm Hg. What is the pressure of dry hydrogen gas collected (in mm Hg)? B) In an electrochemical cell, a metal anode lost 0.248 g while a total volume of 0.08721 L of hydrogen gas was produced. The temperature was 298 K and the barometric pressure was 748.7 mm Hg. At 298 K, the vapor pressure of water is 23.8 mm Hg. How many moles of hydrogen gas were collected? C) In an electrochemical cell, a metal anode lost 0.101 g while a total volume of 0.04875 L of hydrogen gas was produced. The temperature was 298 K and the barometric pressure was 764.5 mm Hg. At 298 K, the vapor pressure of water is 23.8 mm Hg. What is the molar mass of the metal? D) A student uses a strip of metal in an electrolysis circuit in which the metal strip serves as the anode and is connected to the positive terminal of a power supply. The negative terminal of the power supply is connected to an insulated copper wire. An ammeter is placed in the circuit and the power supply is turned on. A current of 1.04 A flows for 5 min and 54 sec. During this time the mass loss of the metal is 0.109 g. What is the molar mass of the metal?
A) In an
B) In an electrochemical cell, a metal anode lost 0.248 g while a total volume of 0.08721 L of hydrogen gas was produced. The temperature was 298 K and the barometric pressure was 748.7 mm Hg. At 298 K, the vapor pressure of water is 23.8 mm Hg. How many moles of hydrogen gas were collected?
C) In an electrochemical cell, a metal anode lost 0.101 g while a total volume of 0.04875 L of hydrogen gas was produced. The temperature was 298 K and the barometric pressure was 764.5 mm Hg. At 298 K, the vapor pressure of water is 23.8 mm Hg. What is the molar mass of the metal?
D) A student uses a strip of metal in an
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