The ________ orbital is degenerate with 5py in a many-electron atom.

Solution:

The gas's new temperature is 604K

Justification:

Assuming standard temperature and pressure, we can determine the gas's temperature using the ideal gas law;

Step 1: Formulate the general gas law equation

P1V1/T1 = P2V2/T2

Step 2: Insert the values, converting as needed to standard units.

P1 = 0.800 atm

V1 = 0.180 L

T1 = 29°C = 273 + 29 = 302K

P2 = 3.20 atm

V2 = 90 mL = 90 * 10^-3 L = 0.09 L

Step 3: Solve for T2

The new gas temperature T2 is calculated as:

T2 = P2V2T1/(P1V1)

T2 = 3.20 * 0.09 * 302 / (0.800 * 0.180)

T2 = 86.976 / 0.144

T2 = 604K

The gas's new temperature is 604K.

Answer:

Explanation:

In a desert cave, an artifact has been discovered. The anthropologists investigating this artifact want to determine its age. They note that the current activity level of the artifact is 9.25 decays/s, and the carbon mass present is 0.100 kg. To ascertain the artifact's age, they will employ specific constants:

r=1.2

The formula for carbon 14 activity is

where,

is the initial activity of the substance

Now, solve for t

since,

Thus, the age of the artifact is

to two significant figures = 6300 years

Answer:

The amount of calcium sulfate that precipitates is 6.14 grams.

Explanation:

Step 1: Provided data

We are mixing 500.0 mL of 0.10 M Ca^2+ with 500.0 mL of 0.10 M SO4^2−

The Ksp for CaSO4 is 2.40×10^−5.

Step 2: Determine moles of Ca^2+

Moles of Ca^2+ = Molarity of Ca^2+ * Volume

Moles of Ca^2+ = 0.10 * 0.500 L

Moles of Ca^2+ = 0.05 moles

Step 3: Determine moles of SO4^2-

Moles of SO4^2- = 0.10 * 0.500 L

Moles SO4^2- = 0.05 moles

Step 4: Compute total volume

Total volume = 500.0 mL + 500.0 mL = 1000 mL = 1L

Step 5: Compute Q

Q = [Ca2+] [SO42-]

[Ca2+] = 0.050 M and [SO42-]

Qsp = (0.050)(0.050) = 0.0025 >> Ksp

This indicates that precipitation will take place.

Step 6: Calculate molar solubility

Ksp = 2.40 * 10^-5 = [Ca2+][SO42-] =(x)(x)

2.40 * 10^-5 = x²

x = √(2.40 * 10^-5)

x = 0.0049 M (molar solubility)

Step 7: Determine total dissolved CaSO4

Total CaSO4 dissolved = 0.0049 M * 1 L * 136.14 g/mol = 0.667 g

Step 8: Calculate initial mass of CaSO4

Initial moles of CaSO4 = 0.050

Initial mass of CaSO4 = 0.050 * 136.14 g/mol

Initial mass of CaSO4 = 6.807 grams

Step 9: Calculate precipitate mass

6.807 - 0.667 = 6.14 grams.

The mass of calcium sulfate that will emerge as a precipitate is 6.14 grams.

Step 1: Convert density from g/mL to g/L; 0.807 g/mL is equivalent to 807 g/L. Step 2: Calculate Moles of N₂; Density = Mass / Volume, or Mass = Density × Volume. Plugging in values, Mass = 807 g/L × 1 L gives us Mass = 807 g. Similarly, Moles = Mass / M.mass, which leads to Moles = 807 g / 28 g.mol⁻¹, giving us Moles = 28.82 moles. Step 3: Apply the Ideal Gas Law to determine Volume of gas occupied; P V = n R T, thus V = n R T / P. Remember to convert temperature to Kelvin (25 °C + 273 = 298 K). Hence, V = (28.82 mol × 0.08206 atm.L.mol⁻¹.K⁻¹ × 298 K) ÷ 1 atm, resulting in V = 704.76 L.

Answer:

• The density of ethanol measures 0.80 g/ml.

Explanation:

The density of water is known to be 1 g/ml, indicating that 158 g of water occupies a volume of 158 ml.

            d = m/v = 258/258 = 1 g/ml

This implies the volume will remain the same for ethanol.

            hence, the density of ethanol = 127/158 = 0.80 g/ml