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Blank = 5.6 (I believe)
Rain having a pH of 5.6 would be designated as acid rain.
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Answer:
The answer is here, this isn't a scam btw you can trust me. :)
Explanation:
https://www.clutchprep.com/chemistry/practice-problems/2606/when-1-mole-of-glucose-c6h12o6-is-completely-burned-into-co2-how-many-moles-of-h
he value for the equilibrium constant for the following chemical reaction, the auto-ionization of water, is 1.0x10-14 at 298 K <u>1x10-14 0.5x10-14 2x10-14 -1x10-14 1x1014 1x10-15</u>
<h3>What is
chemical reaction?</h3>
A chemical reaction is a procedure that causes one group of chemical components to change chemically into another. Chemical reactions, which can frequently be described by a chemical equation, traditionally include changes that only affect the locations of electrons in the formation and dissolution of chemical bonds between atoms, with no change to the nuclei (no change to the elements present). The study of chemical processes involving unstable and radioactive elements, where both electronic and nuclear changes may take place, is known as nuclear chemistry.
Reactants or reagents are the substance(s) or substances that are initially utilized in a chemical reaction.
To learn more about chemical reaction, from the given link:
brainly.com/question/14197404
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A. This is not a redox reaction. It is an example of combustion.
<h3>Combustion reaction of hydrocarbon</h3>
During the combustion of a hydrocarbon, the hydrocarbon reacts with oxygen to create carbon dioxide, water, and heat.
<h3>Example of combustion reaction</h3>
2C8H18 + 25O2 → 16CO2 + 18H2O
Thus, we can conclude that, this is not a redox reaction. It is an example of combustion.
Learn more about combustion here: brainly.com/question/9425444
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Answer: 3.115 atm
Solution:
Firstly, the temperature and pressure at STP is 273 K and 1 atm respectively.
Now, the question mentions a change in temperature from 273 K to 850 K, which has resulted in a change in pressure from 1 atm. Based on this, it is evident that this question is based on Gay- Lussac's Gas Law which notes that an increase in temperature, causes an increase in pressure since the two are directly proportional (once volume remains constant). As such, we can find the new pressure by employing Gay-Lussac's Equation :
P₁ ÷ T₁ = P₂ ÷ T₂
Since the initial temperature (T₁) is 273 K, the final temperature is 850 K (T₂) and the initial pressure (P₁) is 1 atm, then we can substitute these into the equation to find the final pressure (P₂).
⇒ (1 atm) ÷ (273 K) = P₂ ÷ (850 K)
⇒ P₂ = (0.00366 K · atm) × 850 K
⇒ P₂ = 3.115 atm
Thus the new pressure is 3.115 atm.