Which one has a large entropy? 0.0200 moles of NaBr dissolved in 2.00 L of water or 0.0200 moles of CaCl 2 dissolved in 2.00 L of water. Explain

What is the entropy change, in J mol-1 K-1, when 100.0 g of water boils at 100.0 oC?  (ΔHvaporization = 40.7 kJ/mol)  Type in your answer as a whole number with no units.

Does the entropy increase or decrease in these reactions? Why? a) 4 Al + 3 O2 → 2 Al2O3 b) C + 2 Cl2 → CCl4 c) H2O (l) → H2O (g) d) CCl4 → C + 2 Cl2

How does the molar entropy of a substance change with increasing temperature? The molar entropy of a substance increases with increasing temperatures. O The molar entropy of a substance decreases with increasing temperatures.

Calculate the entropy change of 63.4 g of water that freezes into ice at 273.15 K. AHfus for water is 6.01 kJ/mol. J/K

Compare what will happen to the entropy of the whole system in the following two scenarios: A) if the oil molecules are all clumped together and the clump is surrounded by water and B) if the oil molecules are spread out evenly throughout the water, each individual oil molecule surrounded by water?

. Chloroform, CHC13, has a normal boiling point of 61 °C and it enthalpy of vaporization is 29.24 kJ/mol, what is its entropy of vaporization in J/mol·K at 61 °C? Before you calculate it write a chemical equation for this process and predict do you expect entropy to be positive or negative?

list any physical changes you can think of in which entropy increases (ΔS = +)

Determine the total entropy change when 15.00 g of ice at –15°C is heated to 75°C. The molar heat of fusion of ice is 6.02 kJ/mol, and its specific heat is 2.11 J/g °C. The specific heat of water is 4.184 J/g °C