If a water electrolysis cell operates at a current of 7.6 AA , how long will it take to generate 27.0 LL of hydrogen gas at a pressure of 27.0 atm and a temperature of 26 ∘C∘C?
R = 0.08206 L atm mol-1 K-1
Reduction of H2O to give H2 is as follows
thus 2 mole of electron is used up in formation of one mole of
hydrogen gas.
here, mole of hydrogen can be calculated using PV=nRT
Thus, n = 29.711 ( P=27 atm, V= 27 litre and T = 299 K)
from above we had obtained 1 mole H2 is liberated from 2 mole electron thus to obtain 29.711 mole H2 we need 59.422 mole of electron
Charge on one mole electron =
thus charge on 59.422 mole = 5728280.8 coulomb
now we know
thus T = 753721.15 sec ( I = 7.6 A)
= 209.36 hours
If a water electrolysis cell operates at a current of 7.6 AA , how long will...
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If a water electrolysis cell operates at a current of 7.9 A , how long will it take to generate 27.0 L of hydrogen gas at a pressure of 26.0 atm and a temperature of 23 ∘C?
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Taking into account the vapor pressure of water, how many moles of hydrogen gas, n, are present in 343 mL at 752 torr and 29 ∘C?The value of the gas constant R is 0.08206 L⋅atm/(mol⋅K). You may also find the conversion factors 1 atm=760 torr and TK=TC+273 useful. Express the number of moles to three significant figures.
Constant R = 0.08206 L atm mol K 1. (1 pt) Convert 187.2 Torr to atmospheres. 2. (2 pts) Calculate the pressure of 1.64 mol of a perfect gas that occupies a volume of 21.4 L at room temperature (25°C). 3. (2 pts) What is the molar mass of a 28.0 g sample of a perfect gas that occupies a volume of 22.4 L at a pressure of 1.00 atm and at a temperature of 0°C? Name (print): Section No....