Considering the combined law equation, you would have a volume of 9.28 mL at 25.0 C and 2.25 atm.
Boyle's lawBoyle's law establishes the relationship between the pressure and the volume of a gas when the temperature is constant.
This law says that volume is inversely proportional to pressure: if pressure increases, volume decreases, while if pressure decreases, volume increases.
Mathematically, Boyle's law states that the multiplication of pressure by volume is constant:
P×V= k
Charles's lawCharles's law establishes the relationship between the temperature and the volume of a gas when the pressure is constant.
This law says that the volume is directly proportional to the temperature of the gas: if the temperature increases, the volume of the gas increases, while if the temperature of the gas decreases, the volume decreases.
Mathematically, Charles' law states that the ratio of volume to temperature is constant:
[tex]\frac{V}{T}=k[/tex]
Gay-Lussac's lawGay-Lussac's law establishes the relationship between the temperature and pressure of a gas when the volume is constant.
This law says that the pressure of the gas is directly proportional to its temperature: if the temperature increases, the pressure increases, while if the temperature of the gas decreases, the pressure decreases.
Mathematically, Gay-Lussac's law states that the ratio of pressure to temperature is constant:
[tex]\frac{P}{T}=k[/tex]
Combined law equationCombined law equation is the combination of three gas laws called Boyle's, Charlie's and Gay-Lusac's law:
[tex]\frac{PV}{T}=k[/tex]
Considering an initial state 1 and a final state 2, the following holds:
[tex]\frac{P1V1}{T1}=\frac{P2V2}{T2}[/tex]
Volume in this caseIn this case, you know:
P1= 1.89 atmV1= 10.9 mLT1= 21 C= 294 K (being 0 C= 273 K)P2= 2.25 atmV2= ?T2= 25 C= 298 KReplacing in the combined law equation:
[tex]\frac{1.89 atmx10.9 mL}{294 K}=\frac{2.25 atmxV2}{298 K}[/tex]
Solving:
[tex]\frac{1.89 atmx10.9 mL}{294 K}\frac{298K}{2.25 atm} =V2[/tex]
9.28 mL= V2
Finally, you would have a volume of 9.28 mL at 25.0 C and 2.25 atm.
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A mixture of 0.600 mol of bromine and 1.600 mol of iodine is placed into a rigid 1.000-L container at 350°C.
Br2(g) + I2(g) ↔ 2IBr(g)
When the mixture has come to equilibrium, the concentration of iodine monobromide is
1.190 M. What is the equilibrium constant for this reaction at 350°C? Show step-by step explanation.
A) 3.55 × 10^3
B) 1.24
C) 1.47
D) 282
E) 325
The equilibrium constant for this reaction at 350°C is D. 282.
Equilibrium constantA dynamic chemical system approaches chemical equilibrium constant when enough time has passed and its composition no longer exhibits any discernible propensity to change further. The equilibrium constant of a chemical reaction is the value of its reaction quotient in this condition. The equilibrium constant is independent of the initial analytical concentrations of the reactant and product species in the mixture for a specific set of reaction conditions. Understanding equilibrium constants is crucial for comprehending many chemical systems as well as biological processes like the transport of oxygen by hemoglobin in the blood and the maintenance of acid-base homeostasis in the human body. There are many different kinds of equilibrium constants, including stability constants, formation constants, binding constants, association constants, and dissociation constants.
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A mixture of 0.600 mol of bromine and 1.600 mol of iodine is placed into a rigid 1.000-L container at 350°C.
Br2(g) + I2(g) ↔ 2IBr(g)
When the mixture has come to equilibrium, the concentration of iodine monobromide is
1.190 M. What is the equilibrium constant for this reaction at 350°C? Show step-by step explanation.
A) 3.55 × 10^3
B) 1.24
C) 1.47
D) 282
E) 325
Hydrochloric Acid would best be described as a:
Group of answer choices
A. Arrhenius, BrØnsted-Lowrey and Lewis Base
B. Arrhenius, BrØnsted-Lowrey and Lewis Acid
C. BrØnsted-Lowrey and Lewis Acid
D. Arrhenius and Lewis Acid
Hydrochloric acid would best be described as a Arrhenius acid, Lewis acid and Brønsted-Lowry acid (option B).
What is Arrhenius, Brønsted-Lowry acid?Arrhenius acid is any substance that dissociates in an aqueous solution to form hydrogen ions (H+) or proton.
On the other hand, a Brønsted-Lowry acid is any substance that can donate a proton or hydrogen ion to another substance.
Hydrochloric acid (HCl) can be categorized as an Arrhenius acid and Brønsted-Lowry acid because it has the ability to donate H+ and increase the hydrogen ion concentration of an aqueous solution.
Also, Lewis cids are the chemical substances that are able to accept electron pairs.
Therefore, Hydrochloric acid would best be described as a Arrhenius acid, Lewis acid and Brønsted-Lowry acid.
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#44) Draw the complete chemical equation for the hydrohalogenation reaction of 1-
pentene by HBr. You must show the structures in your reaction; you may NOT use
molecular formulas!
Hydrohalogenation Reaction:
The substitution of hydrogen and halide levels across a double bond takes place. The halide group is connected to the carbon with more substituents. The product will affect by the presence of peroxide
What is the hydrohalogenation reply with example?
Ethene is a symmetrical alkene having two carbon atoms. It reacts with HBr in the presence of CCl4, producing bromoethane or ethyl bromide (CH3CH2Br). Propene is an unsaturated alkene consisting of a three-carbon chain with two carbon particles on either side of the double bond.
What is the hydrohalogenation reaction with example?Ethene is a symmetrical alkene including two carbon atoms. It reacts with HBr in the presence of CCl4, producing bromoethane or ethyl bromide (CH3CH2Br). Propene is an unsaturated alkene consisting of a three-carbon chain with two carbon atoms on either flank of the double bond.
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