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3 years ago

Which of these is a unique property of bases?

Chemistry

1 answer:

tatuchka [14]3 years ago

7 0

Answer:

A. Feels slippery

Explanation:

Bases are the only types of compounds that have a slippery feel.

B is wrong. Most bases do not contain carbon, but organic compounds always do.

C is wrong. Aqueous solutions of bases conduct electricity, but so do aqueous solutions of salts.

D is wrong. Most bases have a bitter taste. Acids have a sour taste.

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A sample of neon gas occupies 105 L at 27°C under a pressure of

Viefleur [7K]

Answer: Volume occupied by given neon sample at standard condition is 123.84 L.

Explanation:

Given: $V_{1}$ = 105 L, $T_{1} = 27^{o}C = (27 + 273) K = 300 K$ , $P_{1}$ = 985 torr

At standard conditions,

$T_{2}$ = 273 K, $P_{2}$ = 760 K, $V_{2}$ = ?

Formula used to calculate the volume is as follows.

$\frac{P_{1}V_{1}}{T_{1}} = \frac{P_{2}V_{2}}{T_{2}}$

Substitute the values into above formula as follows.

$\frac{P_{1}V_{1}}{T_{1}} = \frac{P_{2}V_{2}}{T_{2}}\\\frac{985 torr \times 105 L}{300 K} = \frac{760 torr \times V_{2}}{273 K}\\V_{2} = \frac{94116.75}{760} L\\= 123.84 L$

Thus, we can conclude that volume occupied by given neon sample at standard condition is 123.84 L.

8 0

3 years ago

FILL IN THE BLANKWORD BANK (can use more than once): less, increases, decreases, greaterNO2Cl(g)+NO(g)⇌NOCl(g)+NO2(g)1.Disturbin

Jlenok [28]

Explanation:

If we have the following reaction at equilibrium:

aA + bB ⇄ cC + dD

where a, b, c, and d are the stoichiometric coefficients for the reacting species A, B, C, and D. For the reaction at a particular temperature:

Kc=([C]^c *[D]^d)/([A]^a *[B]^b)

where Kc is the equilibrium constant, which holds that for a reversible reaction at equilibrium and a constant temperature, a certain ratio of reactant and product concentrations has a constant value, Kc (the equilibrium constant). Note that although the concentrations may vary, as long as the reaction in in equilibrium and temperatura don't change, the value of K remains constant.

For reactions that have not reached equilibrium, we obtain the reaction quotient (Qc), instead of the equilibrium constant by substituting the initial concentrations into the equilibrium constant expression.

Qc=([Co]^c *[Do]^d)/([Ao]^a *[Bo]^b)

To determine the direction in wich the net reaction will proceed to reach equilibrium, que compare the values of Qc and Kc.

Qc < Kc: To reach equilibrium, reactants must be converted to products (→)
Qc = Kc: The initial concentrations are equilibrium concentrations. The system in at equilibrium.
Qc > Kc: To reach equilibrium, products must be converted to reactants (←)

Solution:

We have the following reaction:

NO2Cl(g)+NO(g)⇌NOCl(g)+NO2(g)

So:

Kc=([NOCl]^1*[NO2]^1)/([NO2Cl]^1 *[NO]^1)

=([NOCl][NO2])/([NO2Cl][NO])

1. In the equation above, [NO2Cl] it's in the denominator, so if we increase it's numericall value by adding NO2Cl decreases Qc to a value less than Kc.

(From the chemical point of view, if we disturb the equilibrium adding NO2Cl (a reactant), to reach equilibrium again the system proceeds from left to right (→) consuming this reactant.)

2. To reach a new state of equilibrium (where Qc = Kc), Qc therefore increases wich means that the denominator of the expression for Qc decreases (in order to increase the denominator as mention above).

3. To accomplish this, the concentration of reageants decreases (reagents are being consumed), and the concentration of prodcuts increases (products are being formed).

4 0

3 years ago