Chemistry Solutions and Thermodynamics Quiz

<p>0.514 K/mol*Kg (A)</p> Signup and view all the answers

<p>Freezing point depression (D)</p> Signup and view all the answers

<p>The solute molecules reduce the energy of the solvent molecules, making it harder for them to escape into the vapor phase. (A)</p> Signup and view all the answers

<p>The solute molecules decrease the vapor pressure of the solution. (A)</p> Signup and view all the answers

<p>The freezing point of the pure solvent minus the freezing point of the solution. (A)</p> Signup and view all the answers

<p>W = - P(∆V) (B)</p> Signup and view all the answers

<p>The work done is zero. (D)</p> Signup and view all the answers

<p>The relationship between work and internal energy is complex and not easily defined. (C)</p> Signup and view all the answers

<p>Both A and B. (D)</p> Signup and view all the answers

<p>1 L*atm = 101.3 J (C)</p> Signup and view all the answers

<p>Work done by a system is always negative. (A)</p> Signup and view all the answers

<p>The transfer of energy due to a temperature difference. (D)</p> Signup and view all the answers

<p>Heating water in a pot on a stove. (A)</p> Signup and view all the answers

<p>$m = \frac{\Delta Tb}{Kb}$ (B)</p> Signup and view all the answers

<p>0.1 kg (B)</p> Signup and view all the answers

<p>128 g/mol (B)</p> Signup and view all the answers

<p>80.1 °C (D)</p> Signup and view all the answers

<p>To determine the molality of the naphthalene solution (A)</p> Signup and view all the answers

<p>It depends on the number of solute particles in solution (A)</p> Signup and view all the answers

<p>Heat of vaporization (A)</p> Signup and view all the answers

<p>0.020 mol/kg (D)</p> Signup and view all the answers

<p>3 (A)</p> Signup and view all the answers

<p>0.800 mol/kg (C)</p> Signup and view all the answers

<p>-8.19 °C (A)</p> Signup and view all the answers

<p>1.23 °C (B)</p> Signup and view all the answers

<p>-8.19 °C (B)</p> Signup and view all the answers

<p>Colligative properties depend on the concentration of the solute. (B)</p> Signup and view all the answers

<p>Boiling point elevation is directly proportional to solute concentration. (D)</p> Signup and view all the answers

<p>Tb(solution) = Tb(solvent) + ∆Tb (D)</p> Signup and view all the answers

<p>Internal energy change equals the heat added and work done on the system. (B)</p> Signup and view all the answers

<p>∆Tf = Kfm (D)</p> Signup and view all the answers

<p>It reflects the number of particles into which a solute dissociates. (C)</p> Signup and view all the answers

<p>The freezing point depression constant of the solvent. (D)</p> Signup and view all the answers

<p>Ensure the flask is labeled with the corresponding solution name. (A)</p> Signup and view all the answers

<p>The solute disrupts the alignment of solvent molecules in the solution. (B)</p> Signup and view all the answers

<p>Total internal energy change depends on the sum of Q and W. (B)</p> Signup and view all the answers

<p>-100 Joules (C)</p> Signup and view all the answers

<p>-334 Joules (C)</p> Signup and view all the answers

<p>Enthalpy accounts for heat transfer at constant pressure. (C)</p> Signup and view all the answers

<p>To determine the energy absorbed or released in chemical reactions. (D)</p> Signup and view all the answers

<p>Heat is a form of energy transfer, while temperature measures the thermal energy of a substance. (B)</p> Signup and view all the answers

<p>Heat (C)</p> Signup and view all the answers

<p>W decreases by the same amount as Q increases. (A)</p> Signup and view all the answers

The mass of one mole of a substance, expressed in g/mol.

The increase in boiling point due to solute presence: ∆Tb = Kb * m.

Measure of solute concentration: m = moles of solute per kg of solvent.

The decrease in freezing point due to solute: ∆Tf = Tf° - Tf.

Freezing point of the pure solvent.

Freezing point of the solution.

The pressure exerted by a vapor in equilibrium with its liquid or solid state.

State where freezing and melting rates are balanced.

Properties that depend on the number of solute particles in solution, not their nature.

A factor that represents the number of particles an electrolyte produces in solution.

Substances that dissociate into ions in solution, impacting colligative properties.

Substances that do not dissociate into ions and do not conduct electricity in solution.

The increase in boiling point of a solvent due to solute addition, calculated using ∆Tb = iKbm.

The decrease in freezing point of a solvent when a solute is dissolved, calculated using ∆Tf = iKf m.

A strong electrolyte that dissociates into three ions: one Ca²⁺ and two Cl⁻.

The process where ionic compounds separate into individual ions in solution.

The mass of naphthalene used in the calculation, 250 mg or 0.250 g.

The mass of benzene used in the solution, which is 100 g.

Formula to find molality: m = ΔTb / Kb.

Transposing equations to solve for desired variable, like molality.

Calculated as moles = molality × mass of solvent.

Molar mass obtained using the number of moles and mass of substance.

The chemical formula for naphthalene is C10H8.

The final molar mass of naphthalene calculated to be 128 g/mol.

The product of force (F) and distance (d), defined as W=Fxd.

Work defined by compression and expansion of gases, among others.

W = -P(∆V), where ∆V is the change in volume and P is external pressure.

The difference between final and initial volume, ∆V = Vf - Vi.

When gas expands against a vacuum, no work is performed: W = 0.

Gas expands against a constant pressure; work is calculated using W = -P(∆V).

4184 J needed to raise 100 g of water from 20°C to 30°C.

Heat can be gained directly, via work, or a mix of both methods described.

The equation to calculate boiling point elevation: ∆Tb = Kb * m.

The boiling point elevation constant is 0.514 K/mol*Kg.

Calculated using the equation: Tb(solution) = Tb(solvent) + ∆Tb.

The equation to calculate freezing point depression: ∆Tf = Kf * m.

The freezing point depression constant is 1.86 °C*Kg/mol.

States energy cannot be created or destroyed, only transformed: ∆U = Q + W.

A thermodynamic property representing heat content of a system.

A factor used in colligative property equations to represent ion production.

The total energy contained within a system due to both heat and work: ∆U = Q + W.

The energy transferred to or from a system due to temperature difference in a process.

A sequence of changes in a system involving heat transfer and work done.

A principle stating that the total enthalpy change for a reaction is the sum of the enthalpy changes for individual steps.

A measurement of energy in a thermodynamic system, often denoted as H, describing the heat content.

The difference in enthalpy between the products and reactants of a reaction.

Heat is energy transfer; temperature is a measure of thermal energy intensity.