Answer:
The temperature of the gas rises.
Explanation:
This is classified as an ISOCHORIC process where the volume remains unchanged. There is no work done by the system.
The gas only receives internal energy from the heat transferred to it from the surroundings.
In this situation, the pressure also increases.
Specific enthalpy is defined as the overall energy in a system attributed to its temperature and pressure, measured per unit mass. It is essential in thermodynamic calculations when one needs to determine the energy for a specific unit mass of a component.
Specific enthalpy can be computed with the equation:
H = U + PV
For this example, the specific volume is 4.684 cm³/g or 149.888 cm³/g moles, which translates to 149.888 × 10⁻³ J/g moles.
The specific internal energy (U) is 1706 J/mol, and the pressure measured is 41.64.
Calculating gives us H = 1706 + 41.64 × 149.888 × 10⁻³ × 101.3 joules
= 2428 joules / mole
<span>The mass percentage represents the weight of a substance within a mixture in relation to a total mass of 100 units. It's also referred to as %w/w. To find this, you divide the mass of the solute by the total mass of the mixture. Given that we know the volume of water, we need to convert that volume into mass using its density. The calculation is as follows:
Mass of the solution = 100 mL (0.99993 g/mL) water + 25 g EtOH
Mass of the solution = 124.993 g of solution
%w/w = (25 g / 124.993 g) x 100
%w/w = 20% for EtOH</span>
The vapor pressure of a substance varies with temperature. To identify which compound has a vapor pressure of 58 kilopascals at 65 degrees Celsius, we consult standard tables that list temperature against vapor pressure.
According to the tables or graphs, the answer is:
<span>2. ethanol</span>
