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3 years ago

An extremely soluble salt is added to water, and all of it dissolves. Is it at equilibrium? Explain.

1 answer:

5 0

Once the substance stops dissolving, the system is at equlibrium with the water and the undissolved salt now, if it is in the process of dissolving because it is completely soluble but has not been able to completely dissolve, it is not at equilibrium

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Consider phosphoric acid, H3PO4. What is the total number of moles of H+ available for reaction in 4.50 L of 0.750 MH3PO4? Write

NeX [460]

Idk.................

8 0

3 years ago

If you have 250 mL of 0.75 M LINO2.<br> How many grams of this substance<br> would you have?

Vesna [10]

Mass of this substance = 9.928 g

<h3>Further explanation</h3>

Molarity is a way to express the concentration of the solution

Molarity shows the number of moles of solute in every 1 liter of solute or mmol in each ml of solution

$\large{\boxed {\bold {M ~ = ~ \frac {n} {V}}}$

Where

M = Molarity

n = Number of moles of solute

V = Volume of solution

So to find the number of moles can be expressed as

$\boxed{\bold{n=V\times M}}$

mol of substance -Lithium nitrite - LiNO₂ :

V = 250 ml = 0.25 L

M = 0.75 M

$\tt n=0.25\times 0.75=0.1875$

So mass of this substance - LiNO₂ (MW=52,947 g/mol) :

$\tt mass=mol\times MW\\\\mass=0.1875\times 52,947 g/mol\\\\mass=9.928~g$

4 0

3 years ago

The center of the earth is very hot

Arturiano [62]

true. is this what you were looking for?

8 0

3 years ago

How much energy was absorbed by the water?

Lorico [155]

<h2>Answer: <u><em>Precisely, water has to absorb 4,184 Joules of heat (1 calorie) for the temperature of one kilogram of water to increase 1°C.</em></u></h2>

Explanation:

4 0

3 years ago

Read 2 more answers

Consider the following equation: SiO2 (s) + 3C (graphite) --> SiC (s) + 2CO (g) ΔH rxn = 624.6 kJ / mol rxn. Using the follow

DerKrebs [107]

<u>Answer:</u> The enthalpy of the formation of $SiC(s)$ is coming out to be -65.3 kJ/mol

<u>Explanation:</u>

Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles. It is represented as $\Delta H^o$

The equation used to calculate enthalpy change is of a reaction is:

$\Delta H^o_{rxn}=\sum [n\times \Delta H^o_f_{(product)}]-\sum [n\times \Delta H^o_f_{(reactant)}]$

For the given chemical reaction:

$SiO_2(s)+3C\text{ (graphite)}(s)\rightarrow SiC(s)+2CO(g)$

The equation for the enthalpy change of the above reaction is:

$\Delta H^o_{rxn}=[(1\times \Delta H^o_f_{(SiC(s))})+(2\times \Delta H^o_f_{(CO(g))})]-[(1\times \Delta H^o_f_{(SiO_2(s))})+(3\times \Delta H^o_f_{(C(s))})]$

We are given:

$\Delta H^o_f_{(CO(g))}=-110.5kJ/mol\\\Delta H^o_f_{(SiO_2(s))}=-910.9kJ/mol\\\Delta H^o_f_{(C(s))}=0kJ/mol\\\Delta H^o_{rxn}=624.6kJ$

Putting values in above equation, we get:

$624.6=[(1\times \Delta H^o_f_{(SiC(s))})+(2\times (-110.5))]-[(1\times (-910.9))+(3\times (0))]\\\\\Delta H^o_f_{(SiC(s))}=-65.3kJ/mol$

Hence, the enthalpy of the formation of $SiC(s)$ is coming out to be -65.3 kJ/mol.

8 0

4 years ago