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Harrizon [31]
3 years ago
12

Pls this is very important for me. Whoever answer this whole I'll mark them as brainliest..... The question is many cars have ca

talytic converters in their exhaust systems. In a catalytic converter most of the Co and No are formed in a car engine is changed into less harmful products. Identify these products and state the metal catalyst used.
Chemistry
1 answer:
Crank3 years ago
7 0

Answer:

A catalytic converter is a device used to reduce the emissions from an internal combustion engine (used in most modern day automobiles and vehicles). Not enough oxygen is available to oxidize the carbon fuel in these engines completely into carbon dioxide and water; thus toxic by-products are produced. Catalytic converters are used in exhaust systems to provide a site for the oxidation and reduction of toxic by-products (like nitrogen oxides, carbon monoxide, and hydrocarbons) of fuel into less hazardous substances such as carbon dioxide, water vapor, and nitrogen gas.

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What occurs during a chemical reaction?
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What is the pH of a buffer solution upon mixing 15.0 mL of 0.40 M HCl and 20.0 mL of 0.50 M NH? Kb (NH3) = 1.8 x 10 E. 7.00 A. 9
vladimir2022 [97]

<u>Answer:</u> The pH of resulting solution is 9.08

<u>Explanation:</u>

To calculate the number of moles for given molarity, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in mL)}}       ........(1)

  • <u>For HCl:</u>

Molarity of HCl = 0.40 M

Volume of solution = 15.0 mL

Putting values in equation 1, we get:

0.40M=\frac{\text{Moles of HCl}\times 1000}{15.0mL}\\\\\text{Moles of HCl}=0.006mol

  • <u>For ammonia:</u>

Molarity of ammonia = 0.50 M

Volume of solution = 20.0 mL

Putting values in equation 1, we get:

0.50M=\frac{\text{Moles of ammonia}\times 1000}{20.0mL}\\\\\text{Moles of ammonia}=0.01mol

The chemical reaction for hydrochloric acid and ammonia follows the equation:

                  HCl+NH_3\rightarrow NH_4Cl

Initial:          0.006      0.01

Final:             -         0.004              0.006

Volume of solution = 15.0 + 20.0 = 35.0 mL = 0.035 L    (Conversion factor:  1 L = 1000 mL)

  • To calculate the pOH of basic buffer, we use the equation given by Henderson Hasselbalch:

pOH=pK_b+\log(\frac{[salt]}{[base]})

pOH=pK_b+\log(\frac{[NH_4Cl]}{[NH_3]})

We are given:

pK_b = negative logarithm of base dissociation constant of ammonia = -\log (1.8\times 10^{-5})=4.74

[NH_4Cl]=\frac{0.006}{0.035}

[NH_3]=\frac{0.004}{0.035}

pOH = ?

Putting values in above equation, we get:

pOH=4.74+\log(\frac{0.006/0.035}{0.004/0.035})\\\\pOH=4.92

To calculate pH of the solution, we use the equation:

pH+pOH=14\\pH=14-4.92=9.08

Hence, the pH of the solution is 9.08

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4 years ago
If I have 5.00g of solid CO₂ that is allowed to sublimate (turn to gas) in an empty balloon. How many moles of CO₂ are present i
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56g is the coreect acsnw

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