Problem 2. Using the following data, what is the total...

Problem 2. Using the following data, what is the total quantity of heat, in kJ, is required to convert 1.27 moles of compound X from -15.1 $^\circ$C to steam at 148.9 $^\circ$C? $T_{melting}$ = 3.7 $^\circ$C $T_{boiling}$ = 105.2 $^\circ$C molar mass = 32.042 $\frac{g}{mol}$ $\Delta H_{fus}$ = 321 $\frac{J}{g}$ $\Delta H_{vap}$ = 2105 $\frac{J}{g}$ $C_{solid}$ = 1.55 $\frac{J}{g\cdot ^\circ C}$ $C_{liquid}$ = 3.36 $\frac{J}{g\cdot ^\circ C}$ $C_{gas}$ = 1.25 $\frac{J}{g\cdot ^\circ C}$

Transcript

00:01 In this question, we have two more sample of water, which is at 35 degrees minus 35 degrees celsius, and we heated until the gaseous water is reached to 165 degrees celsius.

00:10 We need to calculate the q for the entire process using the following data.

00:14 And the data which is given to us is the specific heat of ice.

00:17 So c for ice is given as 2 .03 jule, degree celsius, inverse, gram inverse.

00:27 Then we have c for h2o.

00:30 That is water in liquid form is given as 4 .18 jule degree celsius inverse gram inverse and then see specific heat okay specific heat for the gaseous that means steam is going to be equal to it is said 2 .02 jule degree celsius inverse gram inverse so this is data given okay and the delta h fusion value is given to us so delta h fusion is equal to 6 .000.

01:00 1 .01 kilojoule per mole and the delta h vaporization value is given to be 40 .0 40 .7 itself it is 40 .7.

01:15 The value is given us 40 .7 kilojoule per mole.

01:19 So here what do you need to find out? we need to find out the q for the entire process.

01:24 Q, that means heat.

01:26 How much is for the entire process? to answer this, first of what we can do, there are five processes.

01:32 Process involved in this case.

01:33 So mass of ice first of all we see the mass of ice will be equal to moles into molecular weight.

01:43 So the moles of we have is two moles and the molecular weight is 18.

01:47 So we have 36 gram as the mass of ice.

01:51 Now the q1 value when we talk about the q1 process it is basically the heat change heat change to increase temperature from minus 35 degree minus 35 degrees celsius to 0 degrees celsius so here what we can do we can use the formula that is m into specific heat specific heat here we will use for ice into the temperature change into the temperature chain so this is the formula which we are going to apply throughout and then we will have mass is 36 gram specific heat value for ice is given as 2 .03 multiplied by the temperatures changed so it is going to be 0 minus of minus 35.

02:40 So this comes out to be equal to 255 .8 jule.

02:45 So this can be written as 2 .56 kilojoule.

02:51 This is the q1 value we got.

02:53 Now the second process, q2.

02:54 It is basically the heat change to melt ice to water.

02:57 Heat change to melt ice to water.

03:05 It is happening at 0 degrees celsius itself.

03:07 So this is going to be moles of water, moles, into delta edge fusion.

03:14 That is equal to two times.

03:16 Deltax fusion value 6 .01...

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