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Luda [366]
3 years ago
6

Which law states that the volume and absolute temperature of a fixed quantity of gas are directly proportional under constant pr

essure conditions? A. Boyle’s law B. Charles’s law C. Dalton’s law D. Gay-Lussac’s law
Chemistry
1 answer:
spin [16.1K]3 years ago
5 0

Answer: B. Charles’s law

Explanation:

To calculate the final temperature of the system, we use the equation given by Charles' Law. This law states that volume of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

\frac{V_1}{T_1}=\frac{V_2}{T_2}

where,

V_1\text{ and }T_1 are the initial volume and temperature of the gas.

V_2\text{ and }T_2 are the final volume and temperature of the gas.

Boyle's law law states that pressure is directly proportional to the volume of the gas at constant temperature.

Gay-Lussac Law states that pressure of the gas is directly proportional to the temperature of the gas at constant pressure.

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Onsider the following reaction at equilibrium:
11111nata11111 [884]

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For the given equation:

C(s)+H_2O(l)\leftrightharpoons CO(g)+H_2(g)

A. C is added to the reaction mixture.

If the concentration of reactant specie is increased , according to the Le-Chatlier's principle , the equilibrium will shift in the direction where decrease in concentration of reactant specie occurs. So, on increasing C ,equilibrium will shift in right direction.

B. H_2O is condensed and removed from the reaction mixture.

If the concentration of reactant specie is decreased , according to the Le-Chatlier's principle , the equilibrium will shift in the direction where increase in concentration of reactant specie occurs. So, on removing water vapor ,the equilibrium will shift in left direction.

C. CO is added to the reaction mixture.

If the concentration of product specie is increased , according to the Le-Chatlier's principle , the equilibrium will shift in the direction where decrease in concentration of product specie occurs. So, on increasing CO, the equilibrium will shift in left direction.

D. H_2 is removed from the reaction mixture.

If the concentration of product specie is decreased , according to the Le-Chatlier's principle , the equilibrium will shift in the direction where increase in concentration of product specie occurs. So, on removing hydrogen , the equilibrium will shift in right direction.

5 0
3 years ago
The distance from the sun to earth would be ______.
Dvinal [7]
C- more than one light year or B-exactly one light year
8 0
3 years ago
Read 2 more answers
How many moles of C2H2 are needed to react completely with 84.0 mol O2?
Airida [17]
33.6 moles are needed to completely react with 84.0 moles of O2
3 0
3 years ago
Read 2 more answers
Hydrogen gas reacts with chlorine gas to form hydrogen chloride as shown in the following reaction: H2 (9) + Cl2 (g) + 2HCl (9)
vivado [14]

Answer:

467

Explanation:

ncl2 = 454.4x1/(71.0 g/mol) = 6.40 mols cl2

6.40 mols cl2 x 2molsHCL/1moleCL2 x 36.5g/1moleHCL = <u>467 g HCL</u>

8 0
3 years ago
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2NO (g) + O2 (g) →2NO2 (g) At equilibrium [NO] = 2.4 × 10 -3 M, [O2] = 1.4 × 10 -4 M, and [NO2] = 0.95 M.
azamat

Answer:

K=1.12x10^9

Explanation:

Hello there!

Unfortunately, the question is not given in the question; however, it is possible for us to compute the equilibrium constant as the problem is providing the concentrations at equilibrium. Thus, we first set up the equilibrium expression as products/reactants:

K=\frac{[NO_2]^2}{[NO]^2[O_2]}

Then, we plug in the concentrations at equilibrium to obtain the equilibrium constant as follows:

K=\frac{(0.95)^2}{(0.0024)^2(0.00014)}\\\\K=1.12x10^9

In addition, we can infer this is a reaction that predominantly tends to the product (NO2) as K>>>>1.

Best regards!

4 0
3 years ago
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