AP CHEM Unit 3 Day 5 Review

What is the average current generated in the
Cu(s) + Fe³⁺(aq) → Cu²⁺(aq)+ Fe(s)
electrochemical cell if 50.0 g of Cu(s) are used up in a 24 hour period?
Cu²⁺ + 2 e⁻ → Cu E^◦_red = +0.22 V
Fe³⁺ + 3 e⁻ → Fe E^◦_red = −0.04 V

• 2.64 amp 
• 42.17 amp 
• 1.76 amp
• 13.00 amp

The reaction
2 Ag⁺(aq) + Fe(s) → Fe²⁺(aq) + 2 Ag(s)
taking place in a battery generates a current of 2 amp.
How much Fe(s) is consumed in 1 hour? 

• 4.16 g 
• 8.32 g
•  1.04 g 
• 2.08 g

Tags

NGSS.HS-PS1-7

How long would a current of 10 mA take to produce 0.096000 g of Mo(s) from Mo⁵⁺(aq)?
Be careful with units!

• 48,243,000 s
• 48,243 s
• 9, 648.5 s 
• 9, 648, 500 s

Tags

NGSS.HS-PS1-7

A steel surface has been electroplated with 1.02g of vanadium (V, molar mass = 51 g/mol). If 9.65×10³ C of charge were used, what was the original oxidation number of V?

• +2
• +3 
• +4
• +5

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-1

The (ampere, coulomb, volt, joule) is a quantity of electric charge and the (watt, ampere, faraday, volt) is the rate at which that charge flows.

• joule; faraday 
• ampere, volt
• coulomb; ampere
• volt; ampere 

Tags

NGSS.HS-PS2-4

If 6.6 moles of copper metal was deposited from a solution of Cu(NO₃)₂, how many electrons were involved? 

• 8.0 × 10²⁴ electrons
• 6.0 × 10²³ electrons
• 4.0 × 10²⁴ electrons
• 2.0 × 10²⁴ electrons

Tags

NGSS.HS-PS1-2

How many moles of of metallic iron (Fe) could be produced from Fe²⁺ at a current of 0.004amperes for 964,853 seconds?

• 0.02 mol Fe
• 0.2 mol Fe 
• 0.04 mol Fe 
• 0.4 mol Fe

What is the cathode in
Ag(s) + Fe²⁺(aq) → Ag⁺(aq) + Fe(s)
Ag⁺ + e⁻ → Ag    E^◦_red = +0.80
Fe²⁺ + 2 e⁻ → Fe    E^◦_red = −0.44
and what type cell is it? 

• Fe(s); an electrolytic cell
• Fe(s); a battery
• Ag(s); an electrolytic cell
• Ag(s); a battery

Tags

NGSS.HS-PS1-2

You construct a cell for which E = −0.4 V. Which statement about cell convention is NOT true?

• Oxidation occurs at the anode
• The reaction is not spontaneous
• Reduction occurs at the cathode
• The reaction is spontaneous

Tags

NGSS.HS-PS3-5

What would be the E ◦ cell of an electrolytic cell made from the half reactions
AgCl(s) + e⁻ → Ag(s) + Cl⁻(aq)    E^◦= +0.22V
Al³⁺(aq) + 3 e⁻ → Al(s)    E^◦= −1.66 V

• −1.88
• 1.88
• −1.44 
• 1.44

Tags

NGSS.HS-PS1-2