c. How much heat will be released when 6.44 g of sulfur reacts with exess accord

Question

c. How much heat will be released when 6.44 g of sulfur reacts with exess according to the following equation? 2S+3 022 SOs AH--791.4 kJ -79.5 kJ 11. The specific heat of copper is 0.385 J/(g·°C). If 34.2 g of copper, initially at 25.0°C, absorbs 4.689 kJ, what will be the final temperature of the copper? A) 25.4°C 0y4 M. 81°C 12. A system undergoes a reaction and losses a total of 30kJ of energy at a constant pressure of 1 atm. If the change in heat of the reaction is-27kJ, how much did-th volume expand. 29.615 L 13. Calculate the energy required to bring 1kg of water at 20*C to 120*C. (The AHvap 42k/mol) 2749 kJ 14. Increasing Frequency (v) 1024 1022 1020 1018 1016 1014 1012 1010 108 106 104 102 100 v (s-1) Microwave FMAM Radio waves r-rays X-rays UV IR Long radio waves 10'16 1014 10'12 10-10 10-8 ::10-6 10-4 10-2 109 102 104 106 108 ?(nm) Increasing Wavelength )- Types of Atomic&Molecular; Tra Visible Spectrum Y-rays: nuclear x-rays: core-level electrons Ultraviolet (UV): valence electrons Visible (Vis): valence electrons Infrared (IR): molecular vibrations CS Microwave: molecular roations; electr 400 500 600 700 Radio waves: nuclear spin

Explanation / Answer

C)

Number of moles of sulfur = 6.44 g / 32.066 g/mol=0.201
From the equation we can see,

2 moles of sulfur release = 791.4 kJ of heat

1 mol of sulfur release = 791.4 kJ / 2 = 395.7 kJ of heat

So, 0.200 mol release = 395.7 x 0.200 = 79.5 kJ of heat

11)

Since, q = (m) (?t) (Cp, metal)
Where, (?t) = temperature change
Cp =specific heat of the metal
m = mass of the metal

Putting the respective values in the eqation, we get

4685 J = 34.2 g x 0.385 J/g°C x (T2 - 25°C)

T2 = 381° C

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