If 125 cal of heat is applied to 60.0 g piece of copper at 22.0 c, what will the final temperature be? the specific heat of cooper is 0.0920 cal/g

The final temperature will be 44.64 °C

Explanation:

Step 1: Data given

Amount of heat = 125 cal

Mass of copper = 60.0 grams

Initial temperature of copper = 22.0 °C

Specific heat of copper = 0.0920 cal/g

Step 2: Calculate the final temperature

Q = m*c*ΔT

⇒ Q = the heat transfer = 125 cal

⇒ m = the mass of copper = 60.0 grams

⇒ c = the specific heat of copper = 0.0920 cal/g°C

⇒ ΔT = the change in temperature = T2 - T1 = T2 - 22.0 °C

125 cal = 60.0 g * 0.0920 cal/g *  ΔT

ΔT = 22.64

ΔT = T2 - T1

T2 = 22.64 + 22.0 °C

T2 = 44.64 °C

The final temperature will be 44.64 °C

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml