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2 years ago

PLEASEEE HELPPPP....PLEASEEEE

Chemistry

2 answers:

julia-pushkina [17]2 years ago

5 0

Answer: Choice B is correct. $\Delta G=-89kJ$ and $E^0_c_e_l_l=+0.46V$

Explanation: $\Delta G$ stands for Gibbs free energy equation. A reaction is spontaneous if $\Delta G$ is negative and the reaction non spontaneous if $\Delta G$ is positive.

For a cell, $\Delta G$ is calculated from the cell potential using the equation:

$\Delta G=-nFE^0_c_e_l_l$

where, n is the moles of electrons transferred in a balanced equation, F is the faraday constant and $E^0_c_e_l_l$ is standard cell potential.

From the above equation, $\Delta G$ could only be negative if $E^0_c_e_l_l$ is positive as the equation has negative sign.

So, the only correct choice is the one for which $E^0_c_e_l_l$ is positive and $\Delta G$ is negative.

Hence. choice B is correct.

Kobotan [32]2 years ago

4 0

For a reaction to be spontaneous, ΔG has to be negative and E° cell is positive.

the answer is B

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Why are most solid ionic compounds electrically nonconductive, whereas aqueous solutions of ionic compounds are good conductors

Allisa [31]

Answer:

there must be free-moving electrons in a compound to conduct electricity.

in solid ionic compounds, there are no free electrons so it can't conduct electricity.

But in aqueous form the forces of attraction are broken and the ions (cations and anions) are free to move. This means there are free electrons that allow the aqueous compound to conduct electricity.

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2 years ago

Write the balanced reaction using the fewest whole number coefficients to describe the reaction between gaseous hydrogen and gas

Anastasy [175]

<u>Answer:</u> The percentage yield of water is 9.5 %

<u>Explanation:</u>

We are given:

Moles of hydrogen = 14 moles

Moles of oxygen = 10 moles

The chemical equation for the formation of water from hydrogen and oxygen follows:

$2H_2+O_2\rightarrow 2H_2O$

By Stoichiometry of the reaction:

2 moles of hydrogen gas reacts with 1 mole of oxygen gas

So, 14 moles of hydrogen gas will react with = $\frac{1}{2}\times 14=7mol$ of oxygen gas

As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent

Thus, hydrogen gas is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of hydrogen gas produces 2 moles of water

So, 14 moles of hydrogen gas will produce = $\frac{1}{2}\times 14=7mol$ of water

To calculate the percentage yield of water, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Experimental yield of water = 1.33 moles

Theoretical yield of water = 14 moles

Putting values in above equation, we get:

$\%\text{ yield of water}=\frac{1.33mol}{14mol}\times 100\\\\\% \text{yield of water}=9.5\%$

Hence, the percent yield of the water is 9.5 %.

7 0

2 years ago

Which best describes how isotopes of the same element differ?

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3 years ago

6.9 moles of oxygen gas in a fixed volume of 1.33 liters. One of the valves opened and there remains only 1.24 moles oxygen gas.

Romashka [77]

Answer:

The new volume of the gas remains the same. That is new volume of gas is 1.33 litres

Explanation:

This is because gases do not have a definite shape. They therefore take the shape of their containing vessels and hence their volumes are determined by the volume of the container.

For the question above even if some of the gas escapes, as long as there is gas present in the container, its volume remains the same, that is occupies the same space in the container

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2 years ago

How many liters of hydrogen gas are formed from the complete reaction of 1.03 mol of C? Assume that the hydrogen gas is collecte

aliina [53]

Answer:

27 liters of hydrogen gas will be formed

Explanation:

Step 1: Data given

Number of moles C = 1.03 moles

Pressure H2 = 1.0 atm

Temperature = 319 K

Step 2: The balanced equation

C +H20 → CO + H2

Step 3: Calculate moles H2

For 1 mol C we need 1 mol H2O to produce 1 mol CO an 1 mol H2

For 1.03 moles C we'll have 1.03 moles H2

Step 4: Calculate volume H2

p*V = n*R*T

⇒with p = the pressure of the H2 gas = 1.0 atm

⇒with V = the volume of H2 gas = TO BE DETERMINED

⇒with n = the number of moles H2 gas = 1.03 moles

⇒with R = the gas constant = 0.08206 L*Atm/mol*K

⇒with T = the temperature = 319 K

V = (n*R*T)/p

V = (1.03 * 0.08206 *319) / 1

V = 27 L

27 liters of hydrogen gas will be formed

8 0

3 years ago