Four substances at the same temperature absorb equal amounts of energy. the specific heats of the four substances are 1.01 j/g °c, 0.38 j/g °c, 0.45 j/g °c, and 2.00 j/g °c. what is the specific heat value of the substance that will have least increase in temperature? 0.38 j/g °c 0.45 j/g °c 1.01 j/g °c 2.00 j/g °c

2.00 J/g.°C

Explanation:

To solve this problem, we can use the relation:

Q = mcΔT,

Where, Q is the amount of heat needed to raise the temperature of the substance (J).

m is the mass of the substance (g).

c is the specific heat capacity of the substance (J/g.°C).

ΔT is the temperature difference (ΔT = final T - initial T).

As clear from the relation; ΔT = Q / mc,

∵ ΔT ∝ 1/c,

The temperature difference is inversely proportional to the specific heat of the substance.

∴ The substance that will have least increase in temperature will be that has the highest specific heat capacity (2.00 J/g.°C).

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-