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 ..

This may not be the answer you are looking for but if the water is at zero and the ice is at zero and you are adding heat you know that SOME of the ice will melt. You don't know if all of it will melt until you calculate it but the problem doesn't ask for that. Nor does it ask for the final temperature.

To determine if the ice will melt when the sodium metal is dropped into the water-ice mixture, we need to consider the energy changes involved.

First, let's break down the given chemical equation:

2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2

This equation tells us that when two moles of sodium (2Na) react with two moles of water (2H2O), they produce two moles of sodium hydroxide (2NaOH) and one mole of hydrogen gas (H2). The reaction also says that the enthalpy change (∆H) for this reaction is -368 kJ, meaning it releases 368 kJ of energy.

So, when the sodium reacts with water, energy is released in the form of heat. This heat can raise the temperature of the surroundings, including the water and ice mixture.

Now let's consider the given conditions: We have 50g of water and 50g of ice, both at 0°C.

The heat released from the reaction can be used to melt the ice and raise the temperature of the water. We know that for ice to melt, it requires energy in the form of heat. The amount of heat required to melt one gram of ice is called the heat of fusion (∆Hf), which is 334 J/g.

To determine if the ice will melt, we need to calculate the total amount of heat released by the reaction and compare it to the heat required to melt the ice.

First, let's convert the mass of sodium from grams to moles using its molar mass. The molar mass of sodium (Na) is approximately 23 g/mol.

Given: Mass of sodium (Na) = 0.25 g
Molar mass of Na = 23 g/mol

Number of moles of Na = Mass of Na / Molar mass of Na
= 0.25 g / 23 g/mol
≈ 0.0109 mol

Since the reaction equation shows that two moles of sodium react with two moles of water, we can conclude that 0.0109 mol of sodium will react with 0.0109 mol of water.

Now, to calculate the heat released by the reaction, we need to use the stoichiometry of the reaction equation.

Given: ∆H = -368 kJ

Number of moles of water (H2O) = 0.0109 mol (from above)
∆H = -368 kJ

To calculate the heat released by the reaction, we use the equation:

Heat released = ∆H × moles of water
= -368 kJ/mol × 0.0109 mol

Calculating this value gives us the total heat released by the reaction.

Now, if this value is greater than the heat required to melt the ice, which is given as 334 J/g, it means there is enough heat released to melt the ice.

Therefore, by performing the necessary calculations, we can determine if the ice will melt or not.