How much heat (in kj) is needed to convert 856 g of ice at −10.0°c to steam at 126.0°c? (the specific heats of ice, water, and steam are 2.03 j/g · °c, 4.184 j/g · °c, and 1.99 j/g · °c, respectively. the heat of fusion of water is 6.01 kj/mol, the heat of vaporization is 40.79 kj/mol.)

The heat required for the given process is 2659.3 kJ

Explanation:

The processes involved in the given problem are:  

Pressure is taken as constant.

To calculate the amount of heat absorbed at different temperature, we use the equation:

       .......(1)

where,

q = amount of heat absorbed = ?

= specific heat capacity of medium

m = mass of water/ice

= final temperature

= initial temperature

To calculate the amount of heat released at same temperature, we use the equation:

      ......(2)

where,

q = amount of heat absorbed = ?

m = mass of water/ice

= latent heat of fusion or vaporization

Calculating the heat absorbed for each process:

We are given:

Putting values in equation 1, we get:

Converting the latent heat of fusion in J/g, we use the conversion factor:

Molar mass of water = 18 g/mol

1 kJ = 1000 J

So,

We are given:

Putting values in equation 2, we get:

We are given:

Putting values in equation 1, we get:

Converting the latent heat of vaporization in J/g, we use the conversion factor:

Molar mass of water = 18 g/mol

1 kJ = 1000 J

So,

We are given:

Putting values in equation 2, we get:

We are given:

Putting values in equation 1, we get:

Total heat absorbed =

Total heat absorbed =

Hence, the heat required for the given process is 2659.3 kJ

plants need sunlight, water, and carbon dioxide to make food. plants use the raw materials of water, nutrients they absorb from soil, and carbon dioxide to make sugars the plant can use. energy from the sun and chlorophyll are also needed.