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3 years ago

How many seconds long is this chemistry class if it last 40.0 minutes

Chemistry

2 answers:

Westkost [7]3 years ago

6 0

Answer:

2,400 seconds

Explanation:

I multiplied the time value by 60 to get my answer

Hope this helped!

ziro4ka [17]3 years ago

4 0

Around 2,400 seconds would be in a 40.0 minute class

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A potassium permanganate solution is prepared by dissolving 22.14g of KMnO4 in water and diluting to a total volume of 1.000 L.

gladu [14]

Answer:

The concentration of H₂C₂O₄ is 7,1800x10⁻³ M

Explanation:

The reaction of the titration is:

2 KMnO₄ + H₂C₂O₄ → 2 CO₂ + K₂O + 2 MnO₃ + H₂O

22.14g of KMnO₄ in 1,00L of water have a molarity of:

22,14g KMnO₄/L× $\frac{1mol}{158,034g}$ = 0,14 M of KMnO₄

The moles you required for a complete reaction are:

0,14 mol KMnO₄/L× 0,02050L = 2,872x10⁻³ mol KMnO₄

By the reaction 2 moles of KMnO₄ reacts with 1 mole of H₂C₂O₄, thus, the moles of H₂C₂O₄ that react were:

2,872x10⁻³ mol KMnO₄× $\frac{1mol H_{2}C_{2}O_{4}}{2molKMnO_{4}}$ = 1,436x10⁻³ moles of H₂C₂O₄

As the volume of the sample was 200,0mL≡ 0,2000L, The concentration of H₂C₂O₄ is:

$\frac{1,436x10^{-3} mol}{0,2000L}$ = 7,1800x10⁻³ M

I hope it helps!

4 0

4 years ago

(easy)+(20 points)

Vitek1552 [10]

Liquid to solid and solid to liquid

4 0

3 years ago

Read 2 more answers

If 3.8 moles of zinc metal react with 6.5 moles of silver nitrate, how many moles of silver metal can be formed, and how many mo

bulgar [2K]

Answer: 6.5 moles of silver metal is formed in the given chemical reaction. The moles of excess reagent left are 0.55 moles.

Explanation:

To calculate the moles of silver formed and the moles of excess reagent left after the reaction, we need to balance the equation first and need to find the limiting and excess reagent.

The balanced chemical equation is:

$Zn+2AgNO_3\rightarrow Zn(NO_3)_2+2Ag$

By Stoichiometry:

2 moles of Silver nitrate reacts with 1 mole of Zinc metal

So, 6.5 moles of silver nitrate will react with = $\frac{1}{2}\times 6.5=3.25moles$ of zinc metal

The required amount of zinc metal is less than the given amount of zinc metal, hence, it is considered as an excess reagent.

Therefore, silver nitrate is the limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of silver nitrate produces 2 moles of silver metal

So, 6.5 moles of silver nitrate will produce = $\frac{2}{2}\times 6.5=6.5moles$ of silver metal.

Number of moles of excess reagent left after the completion of reaction = (3.8 - 3.25)moles = 0.55 moles

Hence, 6.5 moles of silver metal is formed in the given chemical reaction. The moles of excess reagent left are 0.55 moles.

7 0

3 years ago

How many microliters are in 0.68 liters?

kolezko [41]

There are 680,000 microliters in 0.68 liters.

8 0

3 years ago

Does this seem like a good hypothesis?

kondaur [170]

Yeah it uses some valuable scientific vocabulary and background knowledge, I hope this hypothesis will be good enough for your teacher (don't worry it will be)

6 0

3 years ago