Q: Chemistry
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Q: calculate density in g cm^-3 - molar mass is 200.5 g.mol - simple cubic lattice - radius of 185 pm
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Q: The pressure above a pure sample of solid Substance X at -221. °C is lowered. At what pressure will…
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Q: Four liquids are described in the table below. Use the second column of the table to explain the…
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Q: Which of the following has the highest boiling point? O CH O C2 O CH,CI O CH3OH O Kr
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A: Intermolecular forces are the forces that act between molecules and holds them together.
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Q: Cite some possible applications of determining the melting point of a substance. Explain briefly
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Q: Which substance will have the highest boiling point Oa) CHBry OD) CHCH, Oa CHF
A: Boiling point is the temperature at which liquid converts into its vapor state.
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Q: A solid will melt to its liquid phase if enough heat is applied. O True 3 False
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Q: What do supercritical fluids help explain? Give an example of application of supercritical fluids.
A: Supercritical fluids: Supercritical fluids are the substances are in an intermediate state between…
Q: The pressure above a pure sample of solid Substance X at -221. °C is lowered. At what pressure will…
A: Answer: Sublimation is a process in which substance gets converted from its solid form into liquid…
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A: We have been asked the order of freezing point and boiling point of different solutions
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Q: Identify which sample will have the strongest intermolecular forces and explain why. Sample Melting…
A: Melting point is the temperature at which a substance fuses or melts to liquid.
Q: Four liquids are described in the table below. Use the second column of the table to explain the…
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Q: The pressure above a pure sample of solid Substance X at -180. °C is lowered. At what pressure will…
A: Temp. = -180.°C + 273 = 93. K @ 93. K, using the graph we can: Step 1: Project a vertical line from…
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- 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 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) ŚWhich phase has a fixed shape? Solid O Gas O LiquidSubstance X is known to exist at 1 atm in the solid, liquid, or vapor phase, depending on the temperature. Additionally, the values of these other properties of X have been determined: temperature ("C) melting point enthalpy of fusion E density 130- DE 120- 118- You may also assume X behaves as an ideal gas in the vapor phase. Suppose a small sample of X at 50 °C is put into an evacuated flask and heated at a constant rate until 6.0 kJ/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment. IM- 00 75. "C 8.00 kJ/mol 2.80 g/cm² (solid) 2.30 g/ml. (liquid) 10- boiling point enthalpy of vaporization heat capacity 1 110, "C 48.00 kJ/mol X 26. J-K 39, J-K mol mol (solid) 1 (liquid) 35. J-K-mol (vapor) FA 5
- The temperature on a sample of pure X held at 1.13 atm and -9. °C is increased until the sample boils. The temperature is then held constant and the pressure is decreased by 0.39 atm. On the phase diagram below draw a path that shows this set of changes. 200 400 temperature (K) pressure (atm)The vapor pressure of Substance X is measured at several temperatures: temperature vapor pressure 4. °C 0 16. °C 28. °C 0.0584 atm 0.0961 atm 0.152 atm Use this information to calculate the enthalpy of vaporization of X. Round your answer to 2 significant digits. Be sure your answer contains a correct unit symbol. x10 ロ・ロ X I olo Ś3. Explain the process of sublimation Name one substance that sublimes at room temperature and pressure.
- 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)A metallic element, Q, has a body-centered cubic lattice structure as a solid. If Q has an atomic radius of 186 pm and an atomic weight of 88.8, what is the theoretical density of Q in grams per cubic centimeters (g/cm3)?If the final answer is an inexact number, round off to two decimal places.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 6.4 g of glucose (C6H1206) dissolved in 300. mL of water (choose one) O (choose one) 6.4 g of potassium sulfate (K2SO4) dissolved in 300. mL of water (choose one) (choose one) O 6.4 g of sodium bromide (NaBr) dissolved in 300. mL of water (choose one) (choose one) O 300. mL of pure water (choose one) E (choose one) E