A bowl containing 150 grams of water, is heated from 25 °C to 100 °C. The specific heat of water is 4.184 J/g°C. How much heat energy is required to heat the water?

4.7 × 10⁴ J

Explanation:

Step 1: Given data

Step 2: Calculate the temperature change (ΔT)

ΔT = 100 °C - 25 °C = 75 °C

Step 3: Calculate the heat required (Q) to raise the temperature of the water

We will use the following expression.

Q = c × m × ΔT

Q = 4.184 J/g.°C × 150 g × 75 °C = 4.7 × 10⁴ J

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

може ли да зареждате повече информация, моля