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3 years ago

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Which of the following elements has the smallest first ionization energy

1 answer:

dsp733 years ago

7 0

Answer: Its B. Rb

Explanation:Apex

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What must be true of the free energy change, trangle G, for a reaction to be spontaneous?

Vesnalui [34]

Answer:

A) It must be negative

Explanation:

A spontaneous reaction in Chemistry is that which is proceeding in a particular direction without the intervention of any external effect. As a spontaneous reaction proceeds (which can be relatively slow), free energy ΔG, which is the available energy for work, is released.

Gibbs free energy, ΔG, is released during a spontaneous process and hence the ΔG is negative because the reactants have more free energy than the products, hence, no energy input is needed for the reaction to proceed forward but rather an energy output. This is what makes a negative ΔG depict a spontaneous reaction.

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4 years ago

What does lowercase v represent in this formula?

kaheart [24]

Lowercase v = velocity

6 0

3 years ago

How fast a reactant is used up to how fast a product is formed is _____.

tester [92]

<span>B.)the rate of reaction</span>

7 0

4 years ago

Read 2 more answers

The standard free-energy change for this reaction in the direction written is 23.8 kJ/mol. The concentrationsof the three interm

Natali [406]

Answer: The actual free-energy change for the reaction -8.64 kJ/mol.

Explanation:

The given reaction is as follows.

Fructose 1,6-bisphosphate $\rightleftharpoons$ Glyceraldehyde 3-phosphate + DHAP

For the given reaction, $\Delta G^{o}$ is 23.8 kJ/mol.

As we know that,

$\Delta G = \Delta G^{o} + RT ln Q$

Here, R = 8.314 J/mol K, T = $37^{o} C$

= (37 + 273) K

= 310.15 K

Fructose 1,6-bisphosphate = $1.4 \times 10^{-5}$ M

Glyceraldehyde 3-phosphate = $3 \times 10^{-6}$ M

DHAP = $1.6 \times 10^{-5}$ M

Expression for reaction quotient of this reaction is as follows.

Reaction quotient = $\frac{[DHAP][\text{glyceraldehyde 3-phosphate}]}{[/text{Fructose 1,6-bisphosphate}]}$

Q = $\frac{1.6 \times 10^{-5} \times 3 \times 10^{-6}}{1.4 \times 10^{-5}}$

= $3.428 \times 10^{-6}$

Now, we will calculate the value of $\Delta G$ as follows.

$\Delta G = \Delta G^{o} + RT ln Q$

= $23800 + 8.314 \times 310.15 \times ln(3.428 \times 10^{-6})$

= -8647.73 J/mol

= -8.64 kJ/mol

Thus, we can conclude that the actual free-energy change for the reaction -8.64 kJ/mol.

7 0

3 years ago

Sodium carbonate can be prepared by heating sodium bicarbonate. 2 NaHCO3(s) ----> Na2CO3(s) + CO2(g) + H2O(g). Given that DHo

Likurg_2 [28]

Answer:

T = 401.6 K

Explanation:

Given reaction:

$NaHCO3(s) ----> Na2CO3(s) + CO2(g) + H2O(g)$

The thermodynamic parameters; ΔG°, ΔH° and ΔS° are related via the Gibbs -Helmholtz equation given as:

$\Delta G^{0}=\Delta H^{0}-T\Delta S^{0}----(1)$

For a given reaction, the gibbs free energy change ΔG° is related to the equilibrium constant K as:

$\Delta G^{0}=-RTln(K) ---(2)$

It is given that K = 1,

Therefore,

$\Delta G^{0}=-RTln(1) = 0$

Substituting for ΔG° in equation (1)

$0=\Delta H^{0}-T\Delta S^{0}$

$\Delta H = T\Delta S$

$T = \Delta H^{0}/\Delta S^{0}=\frac{128.9 kJ}{0.321 kj/mol-K}=401.6 K$

5 0

3 years ago