Consider a 67-g chunk of ice (∆Hfus = 6.0 kkJ/mol) in a beaker immersed in a water bath. To produce just enough heat to melt the ice, how many moles of solid NaOH (∆Hsoln = -445.1 kJ/mol) must you dissolve in the water bath?
Please show all work.

Thanks in advance.

  1. 👍
  2. 👎
  3. 👁
  1. 67g of ice is 67/18 = 3.72moles. 6.0kJ/mol means it takes 6.0 kJ to convert 1mole of solid ice into liquid water. so, for 3.72moles requires 3.72x6= 22.333kJ energy input.

    the energy released is 445.1kJ/mol from NaOH. so 22.333kJ energy from NaOH must be used/provided..isn't it???..that means we are to find how many mole of NaOH is required to produce 22.333kJ..getting there???...we know that 1mole of NaOH releases 445.1kJ..How many moles are required to release 22.333kJ????

    hope that helps..

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    Calculate the enthalpy change (in kJ) associated with the conversion of 25.0 grams of ice at -4.00 °C to water vapor at 109.0 °C. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K,

  2. chem

    A voltaic cell consists of a strip of cadmium metal in a solution of Cd(NO3)2 in one beaker, and in the other beaker a platinum electrode is immersed in a NaCl solution, with Cl2 gas bubbled around the electrode. A salt bridge

  3. Chemistry

    A .25 g chunk of sodium metal is cautiously dropped into a mixture of 50g of water and 50 g of ice both at 0 C 2Na(s) + 2h2o(l) -> 2naoh(aq) + H2 Delta H = -368 kj Will the ice melt Assuming the final mixture has a heat capacity

  4. Chemistry

    Calculate the amount of energy in kilojoules needed to change 225 g of water ice at -10 C to steam at 125 C. The following constants may be useful: Cm(ice)=36.57 J/(mol*C) Cm(water)=75.40 J/(mol*C) Cm(steam)=36.04 J/(mol*C) Delta

  1. Physical Science

    A 100-g chunk of 72 ∘C iron is dropped into a cavity in a very large block of ice at 0∘C. What is the mass of ice that melts. (The specific heat capacity of iron is 0.11 cal/g⋅∘C.).

  2. Chemistry

    How much energy does it take to convert 0.800 kg ice at -20.°C to steam at 250.°C? Specific heat capacities: ice, 2.1 J g-1 °C-1 liquid, 4.2 J g-1 °C-1 steam, 2.0 J g-1 °C-1 ΔHvap = 40.7 kJ/mol, ΔHfus = 6.02 kJ/mol This is

  3. Science

    In the simulation shown below, each insulated beaker contains equal amounts of the same fluid.The starting temperature of beaker A was 100.0 °C and the starting temperature of beaker B was 0.0 °C. Assuming no heat is lost, what

  4. chemistry

    How much energy (in kilojoules) is needed to heat 4.00g of ice from -11.0∘C to 21.5∘C? The heat of fusion of water is 6.01kJ/mol, and the molar heat capacity is 36.6 J/(K⋅mol) for ice and 75.3 J/(K⋅mol) for liquid water.

  1. Chemistry

    How much ice (in grams) be added to lower the temperature of 355 mL of water from 25 ∘C to 5 ∘C ? (Assume the following: the density of water is 1.0 g/mL, the ice is at 0 ∘C, the heat of fusion of ice is 6.02 kJ/mol, and the

  2. chemistry

    How much energy (in kilojoules) is needed to heat 5.45g of ice from -12.0 C to 32.0 C? The heat of fusion of water is 6.01kJ/mol, and the molar heat capacity is 36.6 J/(K x mol) for ice and 75.3 J/(k x mol) for liquid water

  3. science

    The two systems shown below are identical except for the rod connecting the two beakers. Initially the temperatures of the beakers are as follows: Beaker A = 88°C Beaker B = 42°C Beaker C = 88°C Beaker D = 42°C Four minutes

  4. Chemistry - Energy: Phase Changes

    If 13.4 kJ of energy are added to 1.00 kg of ice at 0 degrees Celsius, how much water at 0 degrees Celsius is produced? How much ice is left? The molar heat of melting is 6.01 kJ/mol. So... 6.01 kJ -> 1 mol (6.01 kJ of energy can

You can view more similar questions or ask a new question.