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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Concept explainers

States of Matter

The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).

Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.

Question

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.

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