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How many grams of...
How many grams of Mg(NO3)2 (MM = 148.33 g/mol) would it take to lower the freezing...
How many grams of Mg(NO3)2 (MM = 148.33 g/mol) would it take to lower the freezing point of (4.95x10^2) grams of water by 4.00°C? The freezing point depression constant of water is Kp = 1.86°C/m. Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: X10 Answer
1h. A certain pure solvent freezes at 39.8°C and has a freezing point depression constant Kf...
1h. A certain pure solvent freezes at 39.8°C and has a freezing point depression constant Kf = 0.777°C/m. What is the predicted freezing point (in °C) of a solution made from this solvent that is (1.90x10^0) m in a non-electrolyte solute? 1i. When (8.23x10^1) g of a non-electrolyte is dissolved in (5.2600x10^2) g of a solvent (with Kb = 0.416°C/m) the boiling point of the solution is 1.50°C higher than the boiling point of the pure solvent. What is the...
8. Please help is due in 30 mins, will rate, Thank you! A certain pure solvent...
8. Please help is due in 30 mins,
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A certain pure solvent freezes at 39.8°C and has a freezing point depression constant Kp = 0.777°C/m. What is the predicted freezing point in °C) of a solution made from this solvent that is (1.42x10^0) m in a non-electrolyte solute?
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At an unknown temperature a solution made of (6.550x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.21x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at this unknown temperature? The molar mass of the solute is (4.080x10^1) g/mol.
10. Please help is due in 30 mins, will rate, Thank you! A reaction has AG°...
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A reaction has AG° = (1.88x10^1) kJ/mol. What is the value of the equilibrium constant, K, at 298 K for this reaction?
9. Please help is due in 30 mins, will rate, Thank you! When (8.8800x10^1) g of...
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When (8.8800x10^1) g of a non-electrolyte is dissolved in (5.84x10^2) g of a solvent (with Kb = 0.416°C/m) the boiling point of the solution is 1.50°C higher than the boiling point of the pure solvent. What is the molar mass (in g/mol) of the non- electrolyte solute?
9 Please help is due in 30 mins, will rate, Thank you! AGº for the reaction...
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AGº for the reaction 2 A(g) = 3 B(g) is -25.5 kJ/mol. What is the value of AG (in kJ/mol) at 298 K when the pressure of each gas is: A = (1.17x10^-5) atm and B = (5.5100x10^0) atm.
Please help is due in 30 mins, will rate, Thank you! At what temperature (in K)...
Please help is due in 30 mins,
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At what temperature (in K) will a reaction be at equilibrium if AHsys = -(4.67x10^2) kJ/mol and ASsys = -(3.7900x10^2) J/K mol?
When 0.60 grams of a non-electrolyte unknown compound is dissolved in 10 grams of water, the...
When 0.60 grams of a non-electrolyte unknown compound is dissolved in 10 grams of water, the freezing point of the solution is -1.86o C. Given that the freezing point of pure water is 0o C and that the freezing-point depression constant for water is 1.86 o C/mol/kg, calculate the molecular mass (g/mol) of the unknown compound.
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A solution is made of two volatile solutes: Chemical A (with a pure vapor pressure of 80.0 mm Hg) and Chemical B (with a pure vapor pressure of 100.0 mm Hg). The solution has a total vapor pressure of (9.88x10^1) mm Hg. If the solution is known to be made from 3.00 mol of A, how many moles of B must there be in the solution? HINT: The...
How many grams of Mg(NO3)2 (MM = 148.33 g/mol) would it take to lower the freezing point of (4.95x10^2) grams of water by 4.00°C? The freezing point depression constant of water is Kp = 1.86°C/m. Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: X10 Answer
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A certain pure solvent freezes at 39.8°C and has a freezing point depression constant Kp = 0.777°C/m. What is the predicted freezing point in °C) of a solution made from this solvent that is (1.42x10^0) m in a non-electrolyte solute?
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At an unknown temperature a solution made of (6.550x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.21x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at this unknown temperature? The molar mass of the solute is (4.080x10^1) g/mol.
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A reaction has AG° = (1.88x10^1) kJ/mol. What is the value of the equilibrium constant, K, at 298 K for this reaction?
9. Please help is due in 30 mins,
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When (8.8800x10^1) g of a non-electrolyte is dissolved in (5.84x10^2) g of a solvent (with Kb = 0.416°C/m) the boiling point of the solution is 1.50°C higher than the boiling point of the pure solvent. What is the molar mass (in g/mol) of the non- electrolyte solute?
9 Please help is due in 30 mins,
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AGº for the reaction 2 A(g) = 3 B(g) is -25.5 kJ/mol. What is the value of AG (in kJ/mol) at 298 K when the pressure of each gas is: A = (1.17x10^-5) atm and B = (5.5100x10^0) atm.
Please help is due in 30 mins,
will rate, Thank you!
At what temperature (in K) will a reaction be at equilibrium if AHsys = -(4.67x10^2) kJ/mol and ASsys = -(3.7900x10^2) J/K mol?
7. Please help is due in 30 mins,
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A solution is made of two volatile solutes: Chemical A (with a pure vapor pressure of 80.0 mm Hg) and Chemical B (with a pure vapor pressure of 100.0 mm Hg). The solution has a total vapor pressure of (9.88x10^1) mm Hg. If the solution is known to be made from 3.00 mol of A, how many moles of B must there be in the solution? HINT: The...
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