An atom with an equal number of electrons and protons has no _________.A. reactivity
B. weight
C. charge

Answers

Answer 1

Answer: The answer would be C. charge because the protons, which are positively charged particles, and the electrons, negatively charged particles, balance each other out and the atom becomes of a neutral charge (or no charge)

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When a chemical reaction is in equilibrium, a. the reaction is proceeding at its maximum rate.
b. there is no net change in the amount of substrates or products.
c. the reaction has stopped.
d. there are equivalent amounts of substrates and products.

Answers

Answer: b. there is no net change in the amount of substrates or products.

Explanation:

The reactions which do not go on completion and in which the reactant forms product and the products goes back to the reactants simultaneously are known as equilibrium reactions.

Equilibrium state is the state when reactants and products are present but the concentrations does not change with time.

$A\rightleftharpoons B$

For a chemical equilibrium reaction, equilibrium state is achieved when the rate of forward reaction becomes equals to rate of the backward reaction.

I need help! In an equilibrium reaction with a Keq of 1 × 108 A. products are favored. B. the reaction is nonspontaneous. C. the reaction is endothermic. D. reactants are favored.

Answers

When K is > than 1 products are favored. When q is < less than 1 reactants are favored. 1 x 108 = 108 which is > 1 so products are favored.

Answer: The correct answer is Option A.

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants. It is represented as $K_(eq)$

For the general reaction:

$A+B\rightarrow C+D$

Expression for equilibrium constant is given as:

$K_(eq)=([C][D])/([A][B])$

Conditions for $K_(eq)$ are:

$K_(eq)>1$ , then products are favored

$K_(eq)=1$ , then forward reaction is equal to backward reaction

$K_(eq)<1$ , then reactants are favored

As, $K_(eq)=1* 10^8$ and is very much greater than 1, so products will be favored.

Hence, the correct answer is Option A.

Look closely at the valence electrons in all eight columns of your table from part C. Which element's location does notmatch the pattern shown in the table?
o helium (He)
o hydrogen (H)
sodium (Na)
O argon (Ar)

Answers

Answer: helium(He)

Explanation: Helium has only 2 electrons in the outermost energy level, but all of the other elements in its column have eight.

If a liquid spontaneously turns into a gas below the critical temperature, it has evaporated.TRUE

FALSE

Answers

Answer:

FALSE

Explanation:

Critical temperature can be defined as the temperature at which a substance can exist as a liquid. Below the critical temperature, the substance will freeze and above the critical temperature, the substance will evaporate.

Note: Liquid cannot evaporate below it's critical temperature

False because if the water goes below critical temp it would be frozen

An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl2(g) is injected into the mixture, and the total pressure jumps to 263.0 Torr (at the moment of mixing). The system then re-equilibrates. The appropriate chemical equation is:PCl3(g) + Cl2(g) ---> PCl5(g)

Calculate the new partial pressures after equilibrium is reestablished. [in torr]

PPCl3

PPCl2

PPCl5

Answers

equilibrium is a situation in which economic forces such as supply and demand are balanced and in the absence of external influences the values of economic variables will not change

The equilibrium constant depends on the following:-

Pressure
Volume

The formula used in the question is as follows:-

$k_p = (P_1)/(P_1*P_2)$ , After putting the value, the equilibrium constant is as follows:-

$k_p = (217)/(13.2*13.2)$

After solving it, the equilibrium constant is 1.245.

The pressure in different systems is as follows:-

Hence, the total pressure is:- $P_1 + P_2+ P_3$

$263 = 13.2 + P_2 + 217$

After solving it, the P2 is 32.8torr.

The equilibrium constant in the second case is:-

$k_p = (P_1^')/(P_1^' * P_2^')$

After putting the value,

$1.245= (217+x)/((13.2-x )* (32.8-x))$

After solving, the value of x is 6.402torr

Hence, the partial pressure $PCL_3,\ CL2, \ PLC_5\$ is 6.798, 26.398, and 223.402 respectively.

For more information, refer to the link;-

brainly.com/question/18222206

Answer:

The new partial pressures after equilibrium is reestablished for $PCl_3$ :

$P_1'=6.798 Torr$

The new partial pressures after equilibrium is reestablished $Cl_2$ :

$P_2'=26.398 Torr$

The new partial pressures after equilibrium is reestablished for $PCl_5$ :

$P_3'=223.402 Torr$

Explanation:

$PCl_3(g) + Cl_2(g)\rightleftharpoons PCl_5(g)$

At equilibrium before adding chlorine gas:

Partial pressure of the $PCl_3=P_1=13.2 Torr$

Partial pressure of the $Cl_2=P_2=13.2 Torr$

Partial pressure of the $PCl_5=P_3=217.0 Torr$

The expression of an equilibrium constant is given by :

$K_p=(P_1)/(P_1* P_2)$

$=(217.0 Torr)/(13.2 Torr* 13.2 Torr)=1.245$

At equilibrium after adding chlorine gas:

Partial pressure of the $PCl_3=P_1'=13.2 Torr$

Partial pressure of the $Cl_2=P_2'=?$

Partial pressure of the $PCl_5=P_3'=217.0 Torr$

Total pressure of the system = P = 263.0 Torr

$P=P_1'+P_2'+P_3'$

$263.0Torr=13.2 Torr+P_2'+217.0 Torr$

$P_2'=32.8 Torr$

$PCl_3(g) + Cl_2(g)\rightleftharpoons PCl_5(g)$

At initail

(13.2) Torr (32.8) Torr (13.2) Torr

At equilbriumm

(13.2-x) Torr (32.8-x) Torr (217.0+x) Torr

$K_p=(P_3')/(P_1'* P_2')$

$1.245=((217.0+x))/((13.2-x)(32.8-x))$

Solving for x;

x = 6.402 Torr

The new partial pressures after equilibrium is reestablished for $PCl_3$ :

$P_1'=(13.2-x) Torr=(13.2-6.402) Torr=6.798 Torr$

The new partial pressures after equilibrium is reestablished $Cl_2$ :

$P_2'=(32.8-x) Torr=(32.8-6.402) Torr=26.398 Torr$

The new partial pressures after equilibrium is reestablished for $PCl_5$ :

$P_3'=(217.0+x) Torr=(217+6.402) Torr=223.402 Torr$

The ph of a buffer does not depend much on the concentrations of its acid–base conjugate pair because

Answers

Answer:

It could react with the present hydride or hydroxile ions.

Explanation:

Hello,

One the main features of buffers, is that when the acid-base conjugates are formed they could react with the added $H^+$ or $OH^(-1)$ in order to keep the pH as constant as its buffer capacity allows it.

Best regards.

Final answer:

A buffer solution maintains a stable pH primarily through the action of its acid-base conjugate pair reacting to counter changes, a property known as buffer capacity. High concentrations increase buffer capacity, allowing more acid or base to be neutralized. However, exceeding the buffer capacity can lead to pH changes.

Explanation:

The pH of a buffer solution doesn't greatly depend on the concentrations of its acid-base conjugate pair as the buffer's job is to keep the pH relatively constant. This is achieved by having appreciable amounts of its weak acid–base pair in the solution. If a strong acid or base is introduced into the system, the buffer pair reacts to counteract these changes. This is called buffer capacity.

For instance, consider a buffered solution composed of acetic acid and its conjugate base, acetate. The system can resist changes in pH upon addition of small quantities of an acid or base. This is because acetic acid and acetate can consume small additions of hydrogen ions (from an acid) or hydroxyl ions (from a base), keeping the overall pH stable.

When concentrations of the acid-base pair are high, the buffer capacity increases and hence more amounts of acid or base can be neutralized without a significant change in pH. However, there are limits to this capacity. If excessive amounts of acid or base are added, they may exceed the buffer's capacity, and its acid/base pairs will be either largely consumed or overrun, leading to changes in pH.