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magentamammoth658Lv1

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A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at 22.5 ^oC to vapor at 59.0 ^oC. Using the provided data, answer the following.

(a) What is the for converting liquid bromine from 22.5 ^oC to 59.0 ^oC?

(b) What is the for the transition of liquid bromine at 59.0 ^oC to gaseous bromine at the same temperature?

(c) Using Hess' Law, what is the of the overall process?

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Brian HingpitLv10

3 Dec 2020

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A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at room temperature (22.5^oC) to vapor at 59.0^oC. To do this, one must use Tables 8.1 and 8.2 for information on the specific heat, boiling point, and heat of vaporization of bromine. In addition, the following step-wise process must be followed.

A. Calculate for:

B. Calculate for:

C. Using Hess' law, calculate for:

azuregoldfish555

When a solute is added to a liquid, the boiling point of the resulting solution is __________ than the freezing point of the pure liquid.

A. no different

B. higher

C. lower

When a solute is added to a liquid, the boiling point of the resulting solution is __________ than the freezing point of the pure liquid.

A. higher

B. no different

C. lower

Solution properties are defined as _______________ if the property depends solely on the number of particles of solute and solvent in the solution, not the identity of the solute.

A. vapor pressure

V.colligative

chemical

hydrogen bonding

The advantage of using ________________ rather than the more commonly used unit of ___________________ is that it is independent of temperature effects on density (and thus, volume) of the solution

A. molarity, ppb

B. molarity, % mass

C. molality, molarity

D. molarity, ppm

If a 6.75 g sample of NaCl were dissolved in 8.41 kg of methanol, the molality would be ___________________ m.

A. 0.0137

B. 1.602

C. 0.803

D. 0.0445

The only information needed to determine the freezing point depression of a non-electrolyte is ______________________________ and _________________________________. f

A. the freezing point constant for the solvent, the temperature

B. the boiling point constant, the boiling point elevation

C. the delta T, the color of the most concentrated sample

D. the molality of the solute, the Kf of the solvent

An aqueous solution boils at 100.50oC. What is the freezing point of the solution? Kb(H2O) = 0.51 oC/m; Kf(H2O) = 1.86 oC/m

A. 0.50 oC

B. -0.50 oC

C. -1.82 oC

D. -5.50 oC

Bromoform has a normal freezing point of 7.80 oC and its Kf = 14.4 oC/m. A solution of 2.58 g of an unknown in 100 g of bromoform freezes at 5.43 oC. What is the molecular weight of the unknown?

A. 18.02 g / mol

B. 0.165 g / mol

C. 156 g / mol

D. 44.01 g / mol

Calculate the freezing point of 0.200 m solution of fructose, C6H12O6, a) in water (boiling point, 0 oC), and b) in acetic acid (boiling point, 16.6 oC). Kf(water) = 1.86 oC/m and Kf(acetic acid) = 3.9 oC.

A. -0.372 oC and 15.8 oC

B. -0.958 oC and 12.3 oC

C. 3.221 oC and 0.875 oC

D. -4.124 oC and 0.0035 oC

10.

Calculate the boiling point, in Celsius, at 1atm of a solution containing 30.0 of cane sugar (molecular weight = 342 g / mol) and 150 g of water.

A. 100.30

B. 103.00

C. 99.7

D. 301.00

Please help! show calculations and answer

1. On dissolving 5.0 g of sodium hydroxide in 50.0 g of water the temperature in the calorimeter went up from 25.0 oC to 45.5 oC. Is this an exothermic reaction? Calculate the enthalpy of the above reaction in kJ/mol. Use your value for Cp=(27.65).

2. To a calorimeter containing 50. g of water at 25 oC, a student added 30. g of water at 70. oC. The final temperature of solution was measured to be 40.5 oC. What is the heat capacity of the calorimeter?

3. A sample of metal weighing 35.5g at a temperature of 100 oC was placed in a calorimeter containing 50 g of water at 25.0 oC. At equilibrium the temperature of water and metal was 35.5 oC. Calculate the heat capacity of the metal. . Use your value for Cp=(27.65).

4. When 0.50 g of magnesium metal is placed in a calorimeter, and 100. mL of 1.0 M HCl were added the temperature of solution increased from 22.2 oC to 44.2 oC. Assume that the specific heat of solution is 4.18 J/goC and that the density is 1g/mL. Write a balanced equation for the above reaction. Calculate the enthalpy of reaction per mole of magnesium. . Use your value for Cp=(27.65).

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