If I had a quantity of this substance at a pressure of 0.25 atm and a temperature of -100°C, what phase change(s) would occur if I increased the pressure to 1.00 atm? At what temperature(s) would they occur? The image displays a phase diagram that illustrates the states of matter (solid, liquid, and gas) for a substance under varying temperatures and pressures.**Axes:**- The x-axis represents Temperature in degrees Celsius (°C), ranging from -200 to 900.- The y-axis represents Pressure in atmospheres (atm), ranging from 0 to 2.**Key Features:**- **Solid Phase:** Occupies the lower left region of the graph. - **Liquid Phase:** Found between the solid and gas phases at higher pressures.- **Gas Phase:** Covers the lower right area, indicating higher temperatures and lower pressures.**Critical Points:**- **Triple Point:** The unique set of conditions where all three phases coexist, depicted as an intersection close to the y-axis.- **Critical Point:** The endpoint of the liquid-gas boundary, beyond which the liquid and gas phases are indistinguishable.**Standard Temperature and Pressure (STP):**- Indicated by a dashed line at 1 atm pressure, showing typical laboratory conditions.This diagram is a useful tool in understanding phase transitions and the conditions under which a substance changes its state.

According to Amonton's volume remaining constant ,pressure of a given mass of gas is directly proportional to the absolute temperature .In other word it can be describe as the pressure of a given mass of a gas increases or decreases by 1/273 of its original pressure at 0 0 C vary at 10 C rise or fall of temperature .Given fix quantity of substance with pressure (P1) is 0.25 atm Given temperature of a that substance (T1) is -1000 C or ( -273+100 =173 kelvin ) Given the increase in pressure is 1.00 atm.According to Amontons 's law P1T1=P2T2 To calculate the new temperature we put the value in the above equation 0.25173=1T20.25×T2=173×1T2=1730.25T2=692 kelvin Now we convert T2 temperature in Celsius =692-273 =4190 C Here from the above calculation at 4190 C the phase change will occur .Since the pressure increases from 0.25 atm to 1.00 atm so its phase changes from Gas→liquid →solid .

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Chemistry

If I had a quantity of this substance at a pressure of 0.25 atm and a temperature of -100° C, what phase change(s) would occur if I increased the pressure to 1.00 atm? At what temperature(s) would they occur?

If I had a quantity of this substance at a pressure of 0.25 atm and a temperature of -100° C, what phase change(s) would occur if I increased the pressure to 1.00 atm? At what temperature(s) would they occur?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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