Thermodynamics ...

$$10\ g$$ of liquid at $$300\ K$$ are heated to $$350\ K$$. The liquid absorbs $$6\ kcal$$. What is the specific heat of the liquid (in $$cal/g^{\circ}C)$$?

Which set of the conditions given below guarantees that a reaction will be spontaneous?

Which is the amount of energy that must be added to raise the temperature of 1 gram of a substance by $$\displaystyle { 1 }^{ \circ  }C$$?

Which of the following condition guarantee a spontaneous reaction?

$$I$$. The energy content of reactants in a chemical reaction must be equal to the energy content of the products.
$$II$$. Energy is conserved in chemical processes.

Which portion of the heating curve for water shown would there be ONLY liquid water present?

Statement I: A reaction with a positive enthalpy and a negative entropy will be spontaneous
BECAUSE
Statement II: The Gibbs free energy for a spontaneous reaction is negative

At what point of the heating curve are intermolecular forces at their greatest level?

How much energy is needed to melt $$100g$$ of water?
$$\Delta {H}_{v}=540\ cal/g$$
$$\Delta {H}_{f}=80\ cal/g$$
$${C}_{water}=1\ cal/{g}^{o}C$$

Which portion of the heating curve for water shown above would there be both liquid and solid water present?