Thermochemistry

Recording boiling points at various pressures for solutions created from these metals dissolved in identical acid concentrations.

Determining melting points for binary alloys composed of these metals under controlled atmospheric conditions to avoid oxidation.

Analyzing voltage outputs from electrochemical cells made up of pure metal electrodes and those alloyed with nonmetals at standard conditions.

Measuring temperature changes when heating metal samples containing known concentrations of impurities using differential scanning calorimetry (DSC).

4180 J

2089 J

418 J

41.8 J

Melting point

Molar mass

Specific heat capacity

Electrical conductivity

( c = \frac{(50\ g + 100\ g) (4.18 J/g°C) (3 °C )}{(150g) (72 °C )} \

( c = \frac{(50\ g)(4.18\ J/g°C)(28°C - 25°C)}{(100\ g)(100°C - 28°C)} \

( c = \frac{(100\ g)(4.18\ J/g°C)(28°C - 25°C)}{(50\ g)(100°C - 28°C)} \

( c = \frac{(50\ g)(4.18\ J/g°K)(75°K)}{(100\ g)(72°K)} \

By linking unfavorable reactions with ATP hydrolysis, the overall combined processes can become reasonable since ATP hydrolysis provides sufficient negative ∆G value.

Coupling does not affect thermodynamics but merely speeds up kinetics by providing alternative pathways with lower activation energies.

Coupling reactions with ATP hydrolysis make them less favorable because it adds extra steps necessitating further enzyme catalysis.

Enthalpic benefits gained through increased orderliness outweigh any losses incurred during ATP hydrolysis making coupled reactions more feasible.

Little change in overall reaction rate after adding catalyst specific for B → C step only.

Large activation energy barrier between B and C steps compared to others.

Constant concentrations lead to steady rates suggesting stationary points along pathway.

Changing [B] does not affect overall reaction rate.

Third-order

Zero-order

First-order

Second-order

Newtons per meter squared (N/m²)

Calories per mole per Kelvin (cal/mol·K)

Kilowatts per hour (kW·h)

Joules per gram per degree Celsius (J/g°C)

A lower specific heat capacity leads to a greater change in temperature for a given amount of energy absorbed/released

An increase in specific heat capacity does not affect the temperature changes since it depends on the amount of substance

A constant specific heat capacity results in unchanged temperature

A higher specific heat capacity decreases the change in temperature given the same amount of energy absorbed/released

The temperature change of the substance.

The phase of the substance.

The amount of substance.

The color of the substance.