The pressure above a pure sample of solid Substance X at -142. °C is raised. At what pressure will the sample melt? Use the phase diagram of X below to find your answer. بالا pressure (atm) solid liquid 200 temperature (K) gas 400
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- Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution freezing point boiling point 9.0 g of potassium hydroxide (KOH) dissolved in 200. mL of water (choose one) e (choose one) 9.0 g of glycerin (C3H8O3) dissolved in 200. mL of water (choose one) (choose one) 9.0 g of glucose (C6H1206) dissolved in 200. mL of water (choose one) (choose one) 200. mL of pure water (choose one) (choose one)A motorist fill his radiator with an anti-freeze mixture that states that the mixture is good to -35 °C. At what temperature on the Kelvin scale will the liquid anti-freeze solidify? 238 K O-35K 202 K 308 K it does not because the label says anti-freeze.Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution freezing point boiling point 2.7 g of potassium sulfate (K2SO4) dissolved in 100. mL of water (choose one) (choose one) 2.7 g of nitric acid (HNO3) dissolved in 100. mL of water (choose one) |(choose one) - 2.7 g of glycerin (C3H8O3) dissolved in 100. mL of water (choose one) (choose one) v 100. mL of pure water (choose one) |(choose one) v ?
- Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution freezing point boiling point (choose one) ↑ 6.7 g of potassium iodide (KI) dissolved in 350. mL of water (choose one) O (choose one) (choose one) ↑ 6.7 g of hydroiodic acid (HI) dissolved in 350. mL of water 6.7 g of sucrose (C₁2H22011) dissolved in 350. mL of water (choose one) (choose one) î 350. mL of pure water (choose one) ✪ (choose one) × Ś ?Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution 2.2 g of ethylene glycol (C₂H602) dissolved in 200. mL of water 2.2 g of sucrose (C12H22011) dissolved in 200. mL of water 2.2 g of potassium nitrate (KNO3) dissolved in 200. mL of water 200. mL of pure water freezing point (choose one) (choose one) (choose one) (choose one) X boiling point (choose one) (choose one) O (choose one) (choose one)The pressure above a pure sample of solid Substance X at -10. °C is lowered. At what pressure will the sample melt? Use the phase diagram of X below to find your answer. pressure (atm) 04- 02- 6 0 atm solid liquid 400 temperature (K) Note: your answer must be within 0.025 atm of the exact answer to be graded correct. gas 600
- Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution 6.0 g of ethylene glycol (C₂H6O2) dissolved in 200. mL of water 6.0 g of potassium sulfate (K₂SO4) dissolved in 200. mL of water 6.0 g of sucrose (C12H22011) dissolved in 200. mL of water 200. mL of pure water freezing point ✓ (choose one) 1(lowest) 2 3 4(highest) (choose one) X boiling point (choose one) (choose one) (choose one) (choose one) ŚStudy the following phase diagram of Substance X. pressure (atm) 24 solid 100 liquid 200 temperature (K) Use this diagram to answer the following questions. a gas 300 Suppose a small sample of pure X is held at -12. °C and 12.0 atm. What will be the state of the sample? Suppose the temperature is held constant at -12. °C but the pressure is decreased by 6 atm. What will happen to the sample? Suppose a small sample of pure X is held at -12. °C and 12.0 atm. What will be the state of the sample? Suppose the temperature is held constant at -12. °C but the pressure is decreased by 6 atm. What will happen to the sample? Suppose, on the other hand, the pressure is held constant at 12.0 atm but the temperature is decreased by 116. °C. What will happen to the sample? (choose one) (choose one) (choose one) (choose one) (choose one)The pressure above a pure sample of solid Substance X at -146. °C is lowered. At what pressure will the sample sublime? Use the phase diagram of X below to find your answer. pressure (atm) solid 200 liquid temperature (K) 400 gas Note: your answer must be within 0.5 atm of the exact answer to be graded correct.
- Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution freezing point (choose onel Ⓒ boiling point (choose one) > 8.1 g of sodium bromide (NaBr) dissolved in 100. mL of water 8.1 g of glycerin (CyHyO₂) dissolved in 400. mL of water (choose one) (choose one) B 8.1 g of hydrolodic acid (HI) dissolved in 400. mL of water Ichoose onel (choose one) 400. mL of pure water [choose one) (choose one)Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution freezing point boiling point 7.3 g of glycerin (C3H8O3) dissolved in 100. mL of water (choose one) (choose one) 7.3 g of glucose (C6H1206) dissolved in 100. mL of water (choose one) (choose one) 7.3 g of potassium iodide (KI) dissolved in 100. mL of water (choose one) (choose one) 100. mL of pure water (choose one) (choose one)Labelling a typical simple phase diagram.