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disa [49]
2 years ago
13

Can someone help with #6 Will mark brainliest too!

Chemistry
1 answer:
lidiya [134]2 years ago
6 0

Answer:

okey brooooooooooooooo

no se ingles solo spanish

Explanation:

todoooooooooooooooooooooo bien bro

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svetlana [45]

Answer:

A. How well a current will flow in a material and it's measured in volts.

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2 years ago
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Which reagent is the limiting reactant when 0.700 mol al(oh)3 and 0.700 mol h2so4 are allowed to react?
lisov135 [29]

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3 years ago
Which statement is true about the relationship between entropy and spontaneity? O Spontaneous reactions tend to lead to higher e
dimulka [17.4K]

Answer:

The true statement is: Spontaneous reactions tend to lead to higher entropy.

Explanation:

The spontaneity of a reaction is linked to the value of Gibbs free energy (ΔG°). The more negative is this value, the more spontaneous is a reaction. At the same time, Gibbs free energy depends on enthalpy (ΔH°) and entropy (ΔS°), according to the following expression:

ΔG° = ΔH° - T.ΔS°

We can see that higher entropies (higher ΔS°) lead to more negative ΔG°, thus, more spontaneous reactions.

3 0
2 years ago
2. Which pair of elements does not form an ionic bond?
Gekata [30.6K]

\mathfrak{\huge{\orange{\underline{\underline{AnSwEr:-}}}}}

Actually Welcome to the concept of Bond Formation.

Answer is :-

B.) O and Cl

These both are Non-Metals with high Electronegativity nature, hence none of them can share electrons to foram any bond to eventually form a Electro valentines Compound.

5 0
2 years ago
Calculate the partial pressure of each gas and the total pressure if the temperature of the gas is 21 ∘C∘C. Express the pressure
Volgvan

The question is incomplete, complete question is ;

A deep-sea diver uses a gas cylinder with a volume of 10.0 L and a content of 51.8 g of O_2 and 33.1 g of He. Calculate the partial pressure of each gas and the total pressure if the temperature of the gas is 21°C.Express the pressures in atmospheres to three significant digits separated by commas.

Answer:

Partial pressure of the oxygen gas is 3.91 atm.

Partial pressure of the helium gas is 20.0 atm

Total pressure of the gases is 24.0 atm

Explanation:

Moles of oxygen gas = n_1=\frac{51.8}{32 g/mol}=1.619 mol

Moles of helium gas = n_2=\frac{33.1 g}{4 g/mol}=8.275 mol

Total moles of gas = n_1+n_2=(1.619 +8.275 ) mole=9.894 mol

Volume of the cylinder = V = 10.0 L

Total pressure in the cylinder = P = ?

Temperature of the gas in cylinder = T = 21°C = 21 + 273 K = 294 K

PV = nRT ( ideal gas equation )

P=\frac{nRT}{V}

=\frac{9.894 mol\times 0.0821 atm L/mol K\times 294 K}{10.0 L}

P = 23.88 atm ≈ 23.9

Partial pressure of the individual gas will be determined by the help of Dalton's law:

partial pressure = Total pressure × mole fraction of gas

Partial pressure of the oxygen gas

p_{1}=P\times \chi_{1}=P\times \frac{n_1}{n_1+n_2}

p_1=23.88 atm\times \frac{1.619 mol}{9.894 mol}=3.91 atm

Partial pressure of the helium gas

p_{2}=P\times \chi_{2}=P\times \frac{n_2}{n_1+n_2}

p_2=23.88 atm\times \frac{8.275 mol}{9.894 mol}=19.97 atm\approx 20.0 atm

6 0
3 years ago
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