#13:(a): Energy of single photon, E = h*c / = 6.626*10-34 J.s * 3*108 m/s / 5.34*10-7 m = 3.722*10-19 J / photon
1 mol photon contains 6.023*1023 photos
=> Energy of 1 mol photon = 6.023*1023 photos * (3.722*10-19 J / photon) = 2.242*105 J
(b): mass of 627 mL water = 627 mL * (1g / 1mL) = 627 g
Initial temperature, Ti = 11.5 oC
Let the final temperature be "T oC"
Q = m*s*deltaT
=> 2.242*105 J = 627 g * 4.184 J/g.oC * (T - 11.5 oC)
=> (T - 11.5 oC) = 2.242*105 J / 627 g * 4.184 J/g.oC
=> (T - 11.5 oC) = 85.5 oC
=> T = 85.5 oC + 11.5 oC = 97.0 oC (Answer)
(c): In (a), the energy liberated = 2.242*105 J * (1kJ/1000 J) = 224.2 kJ
Required energy = 187 kJ.
Since the liberated energy by the light 224.2 kJ is higher than 187 kJ, this light provides sufficient energy.
#14: (a): Manganese(III) chloride is Mn(ClO3)3
Ammonium sulfide is (NH4)2S
When Mn(ClO3)3 and (NH4)2S react, a precipitate of Mn2S3(s) formed.
Balanced equation: 2Mn(ClO3)3(aq) + 3(NH4)2S (aq) ----> Mn2S3(s) + 6NH4ClO3(aq)
(b):Since both the ions are displaces, the reaction type is double displacement reaction.
(c): Formation of a solid precipitate
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