How long would it take for 1.50 mol of water at 100.0 ∘c to be converted completely into steam if heat were added at a constant rate of 19.0 j/s ?

will be required to convert 1.50 mol of water completely into steam.

Further explanation:

Enthalpy of vaporization

It is the amount of energy that is required to convert a substance from its liquid state to a vapor or gaseous state. It is also known as the latent heat of vaporization or heat of evaporation. It is represented by .

The expression for the heat of vaporization is as follows:

                                                               …… (1)

Here,

q is the energy of the substance.

n is the number of moles of the substance.

is the heat of vaporization.

Substitute 1.50 mol for n and 40.7 kJ/mol for in equation (1).

The amount of energy is to be converted into J. The conversion factor for this is,

Therefore the amount of energy can be calculated as follows:

The time required for conversion of water into steam is calculated as follows:

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Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Thermodynamics

Keywords: enthalpy of vaporization, q, n, 1.50 mol, water, steam, 3213.15 s, 61050 J, 61.05 kJ, 40.7 kJ/mol, liquid state, vapour state, substance, time, amount of energy.

h let me think

answer: a chemical reaction

explanation:

im not wrong