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In a laboratory experiment, the freezing point of an aqueous solution of glucose is found to be -0.235 Â°C. What is the molal concentration (m) of this solution? (Kf of water is -1.86 Â°C/m and normal freezing point is 0.0Â°C). Select one: a. 0.437 b. 0.235 c. 0.109 Question 9 Not yet answered Marked out of 1 Flag question Question text What is the pH of a 0.0010 M HNO3? Select one: a. 5.0 b. 1.0 c. 3.0 d. 4.0 Question 10 Not yet answered Marked out of 1 Flag question Question text The standard enthalpy change, Î”HÂ°, for the thermal decomposition of silver nitrate according to the following equation is +78.67 kJ: AgNO3(s) ---> AgNO2(s) + Â½O2(g) The standard enthalpy of formation of AgNO3(s) is âˆ’123.02 kJ/mol. Calculate the standard enthalpy of formation of AgNO2(s) Select one: a. âˆ’32.37 kJ b. âˆ’55.73 kJ c. âˆ’44.35 kJ d. âˆ’88.21 kJ

          In a laboratory experiment, the freezing point of an aqueous solution of glucose is found to be -0.235 Â°C. What is the molal concentration (m) of this solution? (Kf of water is -1.86 Â°C/m and normal freezing point is 0.0Â°C).

Select one:
a. 0.437
b. 0.235
c. 0.109

Question 9
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Marked out of 1
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Question text
What is the pH of a 0.0010 M HNO3?

Select one:
a. 5.0
b. 1.0
c. 3.0
d. 4.0

Question 10
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Marked out of 1
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Question text
The standard enthalpy change, Î”HÂ°, for the thermal decomposition of silver nitrate according to the following equation is +78.67 kJ:

AgNO3(s) ---> AgNO2(s) + Â½O2(g)

The standard enthalpy of formation of AgNO3(s) is âˆ’123.02 kJ/mol. Calculate the standard enthalpy of formation of AgNO2(s)

Select one:
a. âˆ’32.37 kJ
b. âˆ’55.73 kJ
c. âˆ’44.35 kJ
d. âˆ’88.21 kJ

Added by William H.

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