Respuesta :
Additional information:
aqueous silver always has a +1 charge
aqueous copper has a +2 charge in voltameters
solids always have a 0 charge
gaseous oxygen is diatomic and will be notated as oxygen2
*since subscript/superscript is not available full names are written out in place of atomic symbols to add clarity.
1) write a balanced equation (numbers in parenthesis indicate charge):
total reaction: silver(+1) + copper(0) -> silver(0) + copper(+2)
half reaction: silver (+1) + e- -> silver (0)
half reaction: copper(0) -> copper (+2) + 2e-
need to multiple the silver half reaction by two to balance the number of electrons:
half reaction: 2silver (+1) + 2e- -> 2silver (0)
half reaction: copper(0) -> copper (+2) + 2e-
now the electrons cancel out for a total reaction of:
2silver(+1) + copper(0) -> 2silver(0) + copper(+2)
2) convert the amount of silver to moles using the molar mass of silver (make sure units cancel):
4.32g of silver x (1 mole of silver/108g) = 0.04 moles of silver
3) convert silver to copper using the stoichiometry of the balanced equation (make sure units cancel):
0.04 moles of silver x (1 mole copper / 2 moles of silver) = 0.02 moles of copper
4) cover moles of copper to the mass of copper using the molar mass of copper (make sure units cancel):
0.02 moles of copper (64g / 1 mole of copper) = 1.28 of copper
Objects in a series will experience the same current so REPEAT FOR OXYGEN.
1) write a balanced equation
total reaction: silver(+1) + oxygen(-2) -> silver(0) + oxygen2(0)
balance the molecules in the reaction
total reaction: silver(+1) + 2oxygen(-2) -> silver(0) + oxygen2(0)
half reaction: silver (I) + e- -> silver (0)
half reaction: 2oxygen(-2) -> oxygen2(0) + 4e-
need to multiple the silver half reaction by four to balance the number of electrons:
half reaction: 4silver (+1) + 4e- -> 4silver (0)
half reaction: 2oxygen(-2) -> oxygen2(0) + 4e-
now the electrons cancel out for a total reaction of:
4silver(+1) + 2oxygen(-2) -> 4silver(0) + oxygen2(0)
2) convert the amount of silver to moles using the molar mass of silver (make sure units cancel):
4.32g of silver x (1 mole of silver / 108g) = 0.04 moles of silver
3) convert silver to oxygen using the stoichiometry of the balanced equation (make sure units cancel). Remember to compare solid silver to gaseous, diatomic oxygen:
0.04 moles of silver x (1 mole oxygen2 / 4 moles of silver) = 0.01 moles of oxygen2
4) convert moles of oxygen to the liters of oxygen using the G.M.V. (make sure units cancel):
0.01 moles of oxygen x (22.4dm3 / 1 mole of oxygen) = 0.224 dm3 of copper
