CHEMISTRY COLLEGE

2 SO2 (g) + O2 (g) 2 SO3 (g)If the TEMPERATURE on the equilibrium system is suddenly increased :The value of Kc A. IncreasesB. DecreasesC. Remains the sameThe value of Qc A. Is greater than KcB. Is equal to KcC. Is less than KcThe reaction must: A. Run in the forward direction to restablish equilibrium.B. Run in the reverse direction to restablish equilibrium.C. Remain the same. Already at equilibrium.The concentration of O2 will: A. Increase.B. Decrease.C. Remain the same.

Answers

Answer 1

Answer:

Answer:

Part one: B. Kc decreases

Part two: B. Is equal to Kc

Part three: B. Run in the reverse direction to reestablish equilibrium

Part four: A. Increase

Explanation:

Part one: Sulfur dioxide combines with oxygen to form sulphur trioxide in an exothermic reaction. If the temperature is suddenly is increased, while the reaction is at equilibrium, the backward reaction (the endothermic one) is favored to "sweep up the excess heat". An increase in reactants means a decrease in Kc since the denominator(reactants) is becoming bigger while the numerator (products) become smaller.

Part two: Qc is a varying version of Kc. For this set of circumstances, it will be equal to Kc since Kc varies with temperature

Part three: The reaction must run in the reverse to reestablish the equilibrium.

Part four: The concentration of of oxygen will increase as more of the reactants are formed

Answer 2

Answer:

Final answer:

The increase in temperature for this exothermic reaction will cause the value of Kc to decrease, the value of Qc to be greater than Kc, the reaction to run in the reverse direction, and the concentration of O2 to increase.

Explanation:

The given chemical reaction represents a type of equilibrium reaction, specifically an exothermic reaction, as it produces sulfur trioxide (SO3), which releases heat. According to Le Chatelier's principle, to maintain equilibrium, if a system is disturbed by an external factor, the system will adjust accordingly.

Here are my answers to the specific questions:

When the temperature is increased in an exothermic reaction, the system tries to consume the excess heat by moving in the endothermic direction, which is the reverse reaction in this case. Therefore, the value of Kc decreases (B).
Since the equilibrium has been disturbed, the value of Qc will not be equal to Kc. Considering more products are formed, Qc will be greater than Kc (A).
As a response to the increase in temperature, to re-establish equilibrium, the reaction will run in the reverse direction (B).
As the reaction goes in reverse to establish a new equilibrium, the concentration of reactants increases. Thus, the concentration of O2 will increase (A).

Learn more about Chemical Equilibrium here:

brainly.com/question/3920294

#SPJ3

Related Questions

A gas mixture with a total pressure of 770 mmHg contains each of the following gases at the indicated partial pressures: 128 mmHg CO2, 232 mmHg Ar, and 183 mmHg O2. The mixture also contains helium gas. What is the partial pressure of the helium gas?
Balance the following redox reaction occurring in an acidic solution. The coefficient of Mn2+(aq) is given. Enter the coefficients (integers) into the cells before each substance below the equation. ___ AsO2−(aq) + 3 Mn2+(aq) + ___ H2O(l) \rightarrow→ ___ As(s) + ___ MnO4−(aq) + ___ H+(aq)
Suppose one was doing this experiment in the real world and the stockroom ran out of NaCl solutions. Which other solutions of similar concentration could be used in place of NaCl(aq)
The standard free energy change for a reaction in an electrolytic cell is always:_________ a. Positive b. Negative c. Zero d. Impossible to determine
Aqueous hydrochloric acid HCl will react with solid sodium hydroxide NaOH to produce aqueous sodium chloride NaCl and liquid water H2O. Suppose 9.84 g of hydrochloric acid is mixed with 3.1 g of sodium hydroxide. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to 2 significant digits.

How many iron atoms are in 0.32 mol of Fe2031? 3.9x 1023 jron atoms O 3.9 iron atoms O 6.02 x 1023 iron atoms 1.9 x 1023 iron atoms O 11x 10-24 iron atoms

Answers

Answer: $3.9* 10^(23)$ iron atoms

Explanation:

According to avogadro's law, 1 mole of every substance weighs equal to the molecular mass and contains avogadro's number $6.023* 10^(23)$ of particles.

$1 molecule of [tex]Fe_2O_3$ contains= 2 atoms of iron

$1 mole of [tex]Fe_2O_3$ contains= $2* 6.023* 10^(23)=12.05* 10^(23)$ atoms of iron

thus 0.32 moles of $Fe_2O_3$ contains= $(12.05* 10^(23))/(1)* 0.32=3.9* 10^(23)$ atoms of iron

Thus the sample would have $3.9* 10^(23)$ iron atoms.

Calculate your experimentally determined percent mass of water in Manganese(II) sulfate monohydrate. Report your result to 2 or 3 significant figures, e. g. 9.8% or 10.2%.

Answers

The mass percentage of the water in hydrated magnesium sulfate (MnSO4 . H2O) is 10.6%.

What is percentage mass?

The percentage mass is the ratio of the mass of the element or molecule in the given compound.

The percentage can be given as:

$\text{Percent Mass} = \frac{\text{Mass of molecule}}{\text{total mass of compound}} * 100 \%$

The mass of the water is 18.02 g/mol and the molar mass of hydrated magnesium sulfate (MnSO4 . H2O) is 169.03 g/mol.

Thus,

$\text{Percent Mass} = \frac{\text{18.02}}{\text{169.03 }} * 100 \%\n\n\text{Percent Mass} = 10.6 \%}$

Therefore, the mass percentage of the water in hydrated magnesium sulfate (MnSO4 . H2O) is 10.6%.

Learn more about percentage mass:

brainly.com/question/3940233

Answer:

10.6%

Explanation:

The determined percent mass of water can be calculated from the formula of the hydrate by

dividing the mass of water in one mole of the hydrate by the molar mass of the hydrate and

multiplying this fraction by 100.

Manganese(ii) sulphate monohydrate is MnSO4 . H2O

1. Calculate the formula mass. When determining the formula mass for a hydrate, the waters of

hydration must be included.

1 Manganes 52.94 g = 63.55 g

1 Sulphur 32.07 g =

32.07 g 2 Hydrogen is = 2.02 g

4 Oygen =

64.00 g 1 Oxygen 16.00 = 16.00 g

151.01 g/mol 18.02 g/mol

Formula Mass = 151.01 + (18.02) = 169.03 g/mol

2. Divide the mass of water in one mole of the hydrate by the molar mass of the hydrate and

multiply this fraction by 100.

Percent hydration = (18.02 g /169.03 g) x (100) = 10.6%

The final result is 10.6% after the two steps calculations

Calculate the molality of a 35.4 % (by mass) aqueous solution of phosphoric acid (H3PO4) (35.4 % means 35.4 g of H3PO4in 100 g of solution)

Answers

Answer:

3.6124 m/kg

Explanation:

Molality is calculated as moles of solute (mol) divided by kilogram of solvent (kg). Here, we can find these numbers by using the 35.4%, which gives us 35.4 g of H3PO4 and 100 g of solution to work with.

To go from grams to moles for the phosphoric acid, you need to find the molar mass of the compound or element and divide the grams of the compound or element by that molar mass.

Here, the molar mass for phosphoric acid is 97.9952 g/mol. The equation would look like this:

35.4 g x 1 mol / 97.9952 g = 0.3612422 mol

Next, the 100 g of solvent can easily be converted to 0.1 kg of solvent.

To find the molality, divide the moles of solute and kilograms of solution.

0.3612422 mol / 0.1 kg = 3.6124 m/kg

How many Cal2 formula units are present
in 5.164 g of Call2?

Answers

Answer:

1.06x10²² formula units

Explanation:

First we convert 5.164 g of CaI₂ into moles, using its molar mass:

5.164 g ÷ 293.887 g/mol = 0.0176 mol

Then we convert 0.0176 moles into formula units, using Avogadro's number, which relates the number of formula units present in 1 mol:

0.0176 mol * 6.023x10²³ FormulaUnits/mol = 1.06x10²² formula units

Given the reaction below, how will the concentration of D change if the concentration of B decreases by 0.045 M? 3A(g)+2B(g)⇋2C(g)+5D(g)

Answers

Answer:

0.113 M

Explanation:

Since B and D are on opposite sides of the reaction, the concentration of D increases when the concentration of B decreases. The amount by which D increases is determined by the coefficients of B and D in the balanced chemical equation:

[D]= $(5)/(2)$ (0.045 M)=0.113 M.

A piston confines 0.200 mol Ne(g) in 1.20 at 25 degree C. Two experiments are performed. (a) The gas is allowed to expand through an additional 1.20 L against a constant of 1.00atm. (b) The gas is allowed to expand reversibly and isothermally to the same final volume. Please calculate the work done by the gas system in these two processes, respectively. Which process does more work? (revised from 6/e exercise 8.11) Please show calculation details.

Answers

Answer:

The second experiment (reversible path) does more work

Explanation:

Step 1:

A piston confines 0.200 mol Ne(g) in 1.20L at 25 degree °C

(a) The gas is allowed to expand through an additional 1.20 L against a constant of 1.00atm

Irreversible path: w =-Pex*ΔV

⇒ with Pex = 1.00 atm

⇒ with ΔV = 1.20 L

W = -(1.00 atm) * 1.20 L

W = -1.20L*atm *101.325 J /1 L*atm = -121.59 J

(b) The gas is allowed to expand reversibly and isothermally to the same final volume.

W = -nRTln(Vfinal/Vinitial)

⇒ with n = the number of moles = 0.200

⇒ with R = gas constant = 8.3145 J/K*mol

⇒ with T = 298 Kelvin

⇒ with Vfinal/Vinitial = 2.40/1.20 = 2

W = -(0.200mol) * 8.3145 J/K*mol *298K *ln(2.4/1.2)

W = -343.5 J

The second experiment (reversible path) does more work

Other Questions

What is the principal reason we must consider the uncertainty principle when discussing electrons and other subatomic particles but not when discussing our macroscopic world?

HELPPP PLEASEEE....How does a glass of juice become cold when you add ice to it?aThe ice makes the glass colder so the juice becomes colder.bThe ice cools the glass of juice because the slow moving particles in the ice cause the particles of the juice to slow down.cIce is colder than the juice. The cold travel from cold to warm until both items are the same temperature.dThe juice is warmer than the ice. Heat travels in one direction until both items are the same temperature.

What term is used to describe the formation of ions in an aqueous solution from a molecular compound

Counting atoms worksheet