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2 years ago

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The equilibrium constant for the equation Ag+(aq)+2NH3(aq)↽−−⇀[Ag(NH3)2]+(aq) is Kf=2.5×103 M−2 at 25.0 ∘C . Calculate the value

of Δ????∘rxn at 25.0 ∘C . Δ????∘rxn= kJ/mol Is the reaction spontaneous under standard conditions? yes noCalculate the value of Δ????rxn at 25.0 ∘C when [Ag+]=0.00850 M , [NH3]=0.156 M , and [[Ag(NH3)2]+]=0.00632 M . Δ????rxn= kJ/mol Is the reaction spontaneous under these conditions?

1 answer:

Sati [7]2 years ago

5 0

Answer:

a) spontaneous reaction with Delta G = -19.383KJ/mol

b) Spontaneous reaction with Delta G = -85.56KJ/mol

Explanation:

What is applied is the relationship between the standard Gibb's free energy, gas constant and the equilibrium constant which is other wise known as the Vant Hoff Isotherm Equation.

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An archeologist finds a 1.62 kg goblet that she believes to be made of pure gold. She determines that the volume of the goblet i

katovenus [111]

The answer is

<span>The density (D) is quotient of mass (m) and volume (V):
</span> $D= \frac{m}{V}$
The unit is g/cm³

It is given:
m = 1.62 kg = 1620 g
V = 205 mL = 205 cm³
D = ?

Thus:
$D= \frac{m}{V} = \frac{1620g}{205cm ^{3} } = 7.90 g/cm ^{3}$

The density of the goblet is 7.90 g/cm³.

5 0

2 years ago

According to the equation below, how many moles of Ca(OH)2 are required to react with 1.36 mol H3PO4 to produce Ca3(PO4)2? 3Ca(O

allsm [11]

<u>Answer:</u> The amount of calcium hydroxide needed to react is 2.04 moles

<u>Explanation:</u>

We are given:

Moles of phosphoric acid = 1.36 moles

For the given chemical equation:

$3Ca(OH)_2+2H_3PO_4\rightarrow Ca_3(PO_4)_2+6H_2O$

By Stoichiometry of the reaction:

2 moles of phosphoric acid reacts with 3 moles of calcium hydroxide

So, 1.36 moles of phosphoric acid will react with = $\frac{3}{2}\times 1.36=2.04mol$ of calcium hydroxide

Hence, the amount of calcium hydroxide needed to react is 2.04 moles

3 0

2 years ago

A 85.2 g copper bar was heated to 221.32 degrees Celsius and placed in a coffee cup calorimeter containing 4250 mL of water at 2

VLD [36.1K]

Answer:- 64015 J

Solution: There is 4250 mL of water in the calorimeter at 22.55 degree C.

density of water is 1 g per mL.

So, the mass of water = $4250mL(\frac{1g}{1mL})$ = 4250 g

Final temperature of water after adding the hot copper bar to it is 26.15 degree C.

So, $\Delta T$ for water = 26.15 - 22.55 = 3.60 degree C

Specific heat for water is 4.184 $\frac{J}{g.^0C}$

The heat gained by water is calculated by using the formula:

$q=mc\Delta T$

where, q is the heat energy, m is mass and c is specific heat.

Let's plug in the values in the formula and do the calculations:

$q=4250g*\frac{4.184J}{g.^0C}*3.60^0C$

q = 64015 J

So, 64015 J of heat is gained by the water.

5 0

2 years ago

In a laboratory setting, concentrations for solutions are measured in molarity, which is the number of moles per liter (mol/L).

slamgirl [31]

Answer:

im pretty sure its A or C im leaning more toward A tho

Explanation:

6 0

1 year ago

Read 2 more answers

What is the net ionic equation of the reaction of MgCl2 with NaOH? Express your answer as a chemical equation. View Available Hi

kari74 [83]

Answer:

Net ionic equation for the reaction between MgCl₂ and NaOH in water:

$\rm Mg^{2+}\; (aq) + 2\; OH^{-}\; (aq) \to Mg(OH)_2\;(s)$ .

Net ionic equation for the reaction between MgSO₄ and BaCl₂ in water:

$\rm {Ba}^{2+}\; (aq) + {SO_4}^{2-}\;(aq) \to BaSO_4\; (s)$ .

Explanation:

Start by finding the chemical equations for each reaction:

MgCl₂ reacts with NaOH to form Mg(OH)₂ and NaCl. This reaction is a double decomposition reaction (a.k.a. double replacement reaction, salt metathesis reaction.) This reaction is feasible because one of the products, Mg(OH)₂, is weakly soluble in water and exists as a solid precipitate.

$\rm MgCl_2\; (aq) + 2\; NaOH\; (aq)\to Mg(OH)_2 \; (s) + 2\; NaCl\; (aq)$ .

MgSO₄ reacts with BaCl₂ in a double decomposition reaction to produce BaSO₄ and MgCl₂. Similarly, the solid product BaSO₄ makes this reaction is feasible.

$\rm MgSO_4\; (aq) + BaCl_2\; (aq) \to BaSO_4\; (s) + MgCl_2\; (aq)$ .

How to rewrite a chemical equation to produce a net ionic equation?

Rewrite all reactants and products that ionizes completely in the solution as ions.
Eliminate ions that exist on both sides of the equation to produce a net ionic equation.

Typical classes of chemicals that ionize completely in water:

Soluble salts,
Strong acids, and
Strong bases.

Keep the formula of salts that are not soluble in water, weak acids, weak bases, and water unchanged.

Take the first reaction as an example, note the coefficients:

MgCl₂ is a salt and is soluble in water. Each unit of MgCl₂ can be written as $\rm Mg^{2+}$ and $\rm 2\; Cl^{-}$ .
NaOH is a strong base. Each unit of NaOH can be written as $\rm Na^{+}$ and $\rm OH^{-}$ .
Mg(OH)₂ is a weak base and should not be written.
NaCl is a salt and is soluble in water. Each unit of NaCl can be written as $\rm Na^{+}$ and $\rm Cl^{-}$ .

$\rm Mg^{2+} + 2\; Cl^{-} + 2\; Na^{+} + 2\; OH^{-} \to Mg(OH)_2\;(s) + 2\; Na^{+} + 2\; Cl^{-}$ .

Ions on both sides of the equation:

$\rm 2\; Cl^{-}$ , and
$\rm 2\; Na^{+}$ .

Add the state symbols:

$\rm Mg^{2+}\; (aq) + 2\; OH^{-}\; (aq) \to Mg(OH)_2\;(s)$ .

For the second reaction:

$\rm MgSO_4\; (aq) + BaCl_2\; (aq) \to BaSO_4\; (s) + MgCl_2\; (aq)$ .

$\rm Mg^{2+} + 2\; {SO_4}^{2-} + Ba^{2+} + 2\; Cl^{-} \to BaSO_4\; (s) + Mg^{2+} + 2\; Cl^{-}$ .

$\rm Ba^{2+}\; (aq) + {SO_4}^{2-}\; (aq) \to BaSO_4\; (s)$ .

5 0

2 years ago

Read 2 more answers