Calculate the amount of heat needed to raise the temperature of 4 ml of water from 10C to 30C

Heat energy (Q) = 334.72

Explanation:

Volume = 4mL

Initial temperature (T1) = 10°C

Final temperature (T2) = 30°C

Mass = ?

Specific heat capacity of water = 4.184J/g°C

Density of water = 1.0g/mL

Heat energy = ?

Density = mass / volume

ρ = mass / vol

Mass = volume × density (ρ)

Mass = 4 × 1.0

Mass = 4g

Heat energy (Q) = mc∇T

Q = heat energy

M = mass of the substance

C = specific heat capacity of the substance

∇T = change in temperature of the substance = T2 - T1

Q = mc(T2 - T1)

Q = 4 × 4.184 ×(30 - 10)

Q = 16.736 × 20

Q = 334.72J

The heat energy required to raise 4ml of water from 10°C to 30°C is 334.72J

Explanation:

Hello,

In this case, for the given heating process, we should use the following equation in order to compute the amount of heat needed for such change in the temperature of water:

Now, since the density of water is 1 g/mL and its heat capacity is 4.18 J/(g*°C), we are able to compute the heat as follows:

Best regards.

the answer is 0.42 is that is an option. this question provides no info

a). in this case, dh> 0 and sd> 0. if t becomes larger, the term "-tds" will become more negative. at some point, it is possible that -dts will be more negative than the dh is positive, and the reaction will become spontaneous. this is probably the correct answer, but you should look at all of the other possibilities and make sure of that.