How many calories is required to change the temperature of 2.18g of water from 15.3°c to 69.5°c. the specific heat of liquid water is 1.00cal/g°c.

The number  of calories that are  required  to change the temperature  of 2.18 g of water from 15.3 c to 69.5 c is  118.16 cal

    calculation

 heat is therefore= 2.18 g x 1.00 cal/g/c  x 54.2 c=118.16  cal

Given:

Mass of water, m = 2.18 g

Initial temperature of water, T1 = 15.3 C

Final temperature, T2 = 69.5 C

Specific heat, c = 1.00 cal/gC

To determine:

Heat required to raise the water temperature

Explanation:

The amount of heat, Q, required to raise the temperature of water from T1 to T2 is:

Q = mcΔT = mc(T2-T1)

Q = 2.18 * 1 * (69.5-15.3) = 118.16 cal

Ans: Heat required is 118.16 cal

it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2

explanation:

two years ago, when picking flowers in the mountains back of yosemite valley, i found a book. it was blotted and storm-beaten; all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however; many of the inner pages were well preserved. and although all were more or less stained and torn, whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today; its granite pages have been torn and blurred by the same storms that wasted the castaway book.

two years ago, when picking flowers in the mountains back of yosemite valley; i found a book. it was blotted and storm-beaten, all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however, many of the inner pages were well preserved. and although all were more or less stained and torn; whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today, its granite pages have been torn and blurred by the same storms that wasted the castaway book.