Question

1a) A gaseous system absorbs 97 J of heat and increases its internal energy by 85 J. Which of the following statements is correct? The volume of the system decreases and a positive amount of work is done. The volume of the system increases and a positive amount of work is done. The volume of the system increases and a negative amount of work is done. The volume of the system remains constant and no work is done The volume of the system decreases and a negative amount of work is done. 1b)A 27.1-g piece of iron initially at 92.9 °C is submerged into 194.4 g of water at 18.1 °C. What is the final temperature of the metal once the metal and water reaches thermal equilibrium? The specific heats of iron and water are 0.449 J/g·°C and 4.18 J/g·°C, respectively.

Answer #1

1a) Δq **=**+97 J

ΔU = +85J

ΔU = Δq + W , W =P ΔV = 85-97 = -12 J of work is
done

The volume of the system increases and negative amount of work is done

1b) q _{lost} = q_{gain} ,
(mc_{p}Δt)_{iron} =
(mc_{p}Δt)_{water}

27.1 * (92.9 - x) * 0.449 = 194.4 * (x- 18.1) *
4.18

12.1679 ( 92.9 - x) = 812.592 (x- 18.1)

1130.3971 - 12.1679x = 812.592x - 14707.9152

15838.3123 = 824.7599 x

x = 19.2035

The final temperature of the metal once the metal reaches thermal
equilibrium is 19.2 ^{o}C

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