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irinina [24]
3 years ago
6

A student designs an ammeter (a device that measures electrical current) that is based on the electrolysis of water into hydroge

n and oxygen gases. When electrical current of unknown magnitude is run through the device for 2.00 min , 12.4 mL of water-saturated H2(g) is collected. The temperature and pressure of the system are 25 ∘C and 715 torr. Part A How many moles of hydrogen gas are produced? Express your answer to three significant figures and include the appropriate units.
Chemistry
1 answer:
Aleks04 [339]3 years ago
3 0

Answer:

4.61 x 10ˉ⁴ mole H₂(g)

Explanation:

Given electric current for 2 min. => 12.4ml of wet H₂(g) at 25⁰C & 715Torr => ? moles H₂(g)

PV = nRT => n = PV/RT

• P = P(H₂) + P(H₂O) = 715Torr = 715mm = P(H₂) + 23.8mm  

     => P(H₂) = (715 – 23.8)mm = 619.2mm = 619.2mm/760mm/Atm = 0.815Atm

• V = 12.8ml = 0.0128L

• R = 0.08206 L∙Atm/mol∙K  

• T = 25⁰C = 298K

Substituting …  n = PV/RT

=>  n = (0.815Atm)(0.0128L)/(0.08206 L∙Atm/mol∙K)(298K) = 4.61 x 10ˉ⁴ mole H₂(g)

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