All categories

4 years ago

What are doldrums? Give an example.

Chemistry

2 answers:

qaws [65]4 years ago

4 0

Answer:

Doldrums- a state or period of inactivity, stagnation, or depression.

Example:

Doldrums is defined as a gloomy feeling, low spirits or a time of inactivity. An example of doldrums is being stuck in the house during a week long snow storm.

dusya [7]4 years ago

4 0

Answer:

doldrums-a state or period of inactivity, stagnation, or depression.

Ex. being stuck in the house during a week long snow storm

Explanation:

You might be interested in

2CO2 + 3H2O + 4Br2 C = O = H = Br =

devlian [24]

Explanation:

2CO2 + 3H2O + 4Br2

C = 2

O = 5

H = 6

Br =8

8 0

3 years ago

If 50 ml of 0.235 M NaCl solution is diluted to 200.0 ml what is the concentration of the diluted solution

Helen [10]

This is a straightforward dilution calculation that can be done using the equation

$M_1V_1=M_2V_2$

where M₁ and M₂ are the initial and final (or undiluted and diluted) molar concentrations of the solution, respectively, and V₁ and V₂ are the initial and final (or undiluted and diluted) volumes of the solution, respectively.

Here, we have the initial concentration (M₁) and the initial (V₁) and final (V₂) volumes, and we want to find the final concentration (M₂), or the concentration of the solution after dilution. So, we can rearrange our equation to solve for M₂:

$M_2=\frac{M_1V_1}{V_2}.$

Substituting in our values, we get

$\[M_2=\frac{\left ( 50 \text{ mL} \right )\left ( 0.235 \text{ M} \right )}{\left ( 200.0 \text{ mL} \right )}= 0.05875 \text{ M}\].$

So the concentration of the diluted solution is 0.05875 M. You can round that value if necessary according to the appropriate number of sig figs. Note that we don't have to convert our volumes from mL to L since their conversion factors would cancel out anyway; what's important is the ratio of the volumes, which would be the same whether they're presented in milliliters or liters.

5 0

3 years ago

1. A 18 M solution of an acid that ionizes only slightly in solution would be termed___

kondor19780726 [428]

A 18 M solution of an acid that ionizes only slightly in solution would be termed
concentrated and weak. The concentration of the acid is high. The acid which dissociates partially in water is a weak acid.

Calculate the [H^+] for the aqueous solution in which [OH^-] is 1 x10^-9. Is this solution acidic, basic or neutral. To determine [H+] use:

1x10^-14 = [OH-][H+]
solve for [H+]
[H+] = 1x10^-14/1x10^-9
= 1x10^-5

4 0

3 years ago

Which of the following are accurate descriptions of closed and open thermodynamic processes? open processes are 'flow through' p

Shalnov [3]

Answer: Option (a) is the correct answer.

Explanation:

According to thermodynamics, a closed system is defined as the system in which there will be no exchange of matter takes place but there will be exchange of energy between the system and surrounding.

On the other hand, an open system is defined as the system in which there will be exchange of both matter and energy takes place between system and surrounding.

Hence, we can conclude that out of the given options accurate descriptions of closed and open thermodynamic processes is that open processes are 'flow through' processes.

7 0

3 years ago

An ionic compound has a solubility of 30 g per 100 mL of water at room temperature. A solution containing 70 g of the compound i

Llana [10]

Answer: A. unsaturated.

Explanation:

Unsaturated solution is defined as the solution in which more solute particles can be dissolved in the solvent.

Saturated solution is defined as the solution in which no more solute particles can be dissolved in the solvent.

Supersaturated solution is defined as the solution in which more amount of solute particles is present than the solvent particles.

Given: Solubility = 30g/100ml

If 100 ml can dissolve ionic compound = 30 g

300 ml can dissolve ionic compound = $\frac{30}{100}\times 300=90g$

Thus solubility is 90g/300 ml and dissolved salt is only 70 g , the solution is said to be unsaturated.

3 0

3 years ago