What are the respective central-metal oxidation state, coordination number, and overall charge on the complex ion in Na2[Cr(NH3)

An r-selected species has a significantly faster reproductive rate compared to K-selected species.

The focus of r-selected species is on quick maturation and reproduction. They are likely to breed during short periods when water supply is available, thus enhancing their survival chances.

Conversely, K-selected species prioritize nurturing their young and tend to reproduce later. Due to the longer maturation time before breeding, by the time K-selected species are ready, the water supply may be depleted, leading to lower survival odds.

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Answer:

• A. Which element, X or Z, has a higher molar mass?

Explanation:

Heating the original compounds intensely to remove all oxygen causes chemical decomposition reactions:

• 2XClO₃ (solid) → 2XCl + 3O₂ (gas)

• 2ZClO₃ (solid) → 2ZCl + 3O₂ (gas)

By measuring the initial mass of each sample and the mass remaining after heating, the student can compute the oxygen gas mass released:

• Mass of oxygen released = initial sample mass minus residue mass

Using this oxygen mass, she can calculate how many moles of oxygen were present in each sample:

• Moles of oxygen = oxygen mass (g) divided by molar mass of oxygen

Next, the moles of the original sample are determined:

• Each mole of XClO₃ or ZClO₃ has 3 moles of oxygen atoms.

So, dividing the moles of oxygen released by 3 gives the moles of the sample.

Applying the formula molar mass = mass / moles, the student finds the molar masses of XClO₃ and ZClO₃.

Thus, this data allows answering question A: Which of X or Z has the higher molar mass?

The enthalpy change associated with the precipitation reaction is 84 kJ/mole

Why?

The chemical equation for the reaction can be written as

AgNO₃(aq) + NaCl (aq) → AgCl(s) + NaNO₃(aq)

To determine the enthalpy change, the following equation applies

To calculate the heat (Q):

Next, we need to calculate the number of moles involved in the reaction (n):

With these two values, we can substitute them into the first equation:

Have a great day!

Answer: 0.0007 moles of are released when the temperature rises.

Explanation:

To determine the moles, we utilize the ideal gas law, as follows:

where,

P = gas pressure = 1.01 bar

V = gas volume = 1L

R = gas constant =

• Calculated moles at T = 20° C

The gas temperature = 20° C = (273 + 20)K = 293K

Substituting values into the equation gives:

• Calculated moles at T = 25° C

The gas temperature = 25° C = (273 + 25)K = 298K

Substituting values into the equation gives:

• Released moles =

Therefore, 0.0007 moles of are released when the temperature increases from 20° C to 25° C.

The total number of moles of oxygen contained in the sample is 11.3 moles. Explanation: Based on the stoichiometry of the compound, 1 mole of corresponds with 4 moles of CO or can be stated as 1 mole containing 1 mole of Ni, 4 moles of C, and 4 moles of O, leading to the conclusion that moles of C and O are equal. Therefore, since there are 11.3 moles of carbon present, there are likewise 11.3 moles of oxygen.