Enroll in one of our FREE online STEM summer camps. Space is limited so join now!View Summer Courses

Ohio State University

Problem 1
Problem 2
Problem 3
Problem 4
Problem 5
Problem 6
Problem 7
Problem 8
Problem 9
Problem 10
Problem 11
Problem 12
Problem 13
Problem 14
Problem 15
Problem 16
Problem 17
Problem 18
Problem 19
Problem 20
Problem 21
Problem 22
Problem 23
Problem 24
Problem 25
Problem 26
Problem 27
Problem 28
Problem 29
Problem 30
Problem 31
Problem 32
Problem 33
Problem 34
Problem 35
Problem 36
Problem 37
Problem 38
Problem 39
Problem 40
Problem 41
Problem 42
Problem 43
Problem 44
Problem 45
Problem 46
Problem 47
Problem 48
Problem 49
Problem 50
Problem 51
Problem 52
Problem 53
Problem 54
Problem 55
Problem 56
Problem 57
Problem 58
Problem 59
Problem 60
Problem 61
Problem 62
Problem 63
Problem 64
Problem 65
Problem 66
Problem 67
Problem 68
Problem 69
Problem 70
Problem 71
Problem 72
Problem 73
Problem 74
Problem 75
Problem 76
Problem 77
Problem 78
Problem 79
Problem 80
Problem 81
Problem 82
Problem 83
Problem 84
Problem 85
Problem 86
Problem 87
Problem 88
Problem 89
Problem 90
Problem 91
Problem 92
Problem 93
Problem 94
Problem 95
Problem 96
Problem 97
Problem 98
Problem 99
Problem 100
Problem 101
Problem 102
Problem 103
Problem 104
Problem 105
Problem 106
Problem 107
Problem 108
Problem 109
Problem 110
Problem 111

Need more help? Fill out this quick form to get professional live tutoring.

Get live tutoring
Problem 88

What is the change in entropy when 0.200 mol of potassium freezes at $63.7^{\circ} \mathrm{C}\left(\Delta H_{\text { fus }}=2.39 \mathrm{kJ} / \mathrm{mol}\right) ?$

Answer

Check back soon!

You must be logged in to like a video.

You must be logged in to bookmark a video.

## Discussion

## Video Transcript

we want to calculate the change in entropy. Delta s the results in the freezing of potassium. When we freeze a substance, we go from a liquid state to a solid state. Were given a value for the temperature in the bill to each of fusion. For this process, we knew that for it face changes that the change in Gibbs free Energy Delta G will be equal to zero at constant temperatures and pressures. So now we have everything that we need from this equation to solve four Delta s And so we can rearrange that equation to form an expression four deltas be Delta G minus still to age divided by negative t. And now we plug in everything that we know. See that Delta s equals Delta G, which is again zero or face changes. Then we subtract that given Delta each of fusion 2.39 killing joules per mole. And then we divide that by the negative of the given temperature which when we converted into Kelvin, comes out to 300 36.7. And so our units for we're Delta s. The change in entropy will be killing joules per mole times, Kelvin. And if we want to play our answer by 1000 we can get it in units of jewels per mole. Kelvin, when we do that, we see we get about 7.10 Jules for more times. Kelvin. But remember, this is for the freezing of one mole of potassium. And in this problem, we're interested in the changing entropy for the freezing of 0.2 moles of potassium. So in order to find that total change in entropy, we multiply the change in entropy for one mole by that quantity and 0.2 moles that zero point 200 moles times 7.10 Jules, her mole times killed in So the units of moles cancel out. So we're left with total change in entropy units of jewels per kelvin, we get a final answer of Delta s equals 1.4 Jules Per Kelvin

## Recommended Questions