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2 years ago

6

Suppose you had a sample of CH4 in a balloon. Assuming the balloon starts out to be the same size as the He and Ar balloon in th

e diagram, what would you predict about its volume at the end?

1 answer:

Bond [772]2 years ago

7 0

Answer:

they all would be the same size

Explanation:

Because they all have the same amount of each particle

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What volume of H2O(g) is produced when 8.00 mol of C2H4(g) reacts at STP?

sweet-ann [11.9K]

* Mole ratio:

C2H4 + 3 O2= 2 CO2 + 2 H2O

1 mole C2H4 --------------- 2 moles H2O
8.00 moles C2H4 ---------- ?

8.00 x 2 / 1 => 16 moles of H2O

Therefore:

1 mole --------- 22.4 L at ( STP)
16 moles ------- ?

16 x 22.4 / 1 => 358.4 L

hope this helps!

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3 years ago

PLEASE HURRY! What is the name of this alkane?

belka [17]

Answer:

C. 1-ethyl, 3-methylcyclohexane

(Photo for proof at the bottom.)

Explanation:

The 1-ethyl is because you start numbering from the longest branch, towards the next closest branch. Prefix "eth-" means two, there are 2 carbons in the longest branch. 3-methyl is because the next branch is at number 3, and prefix "meth-" means 1, there is 1 carbon in that chain. "Cyclo" in cyclohexane means the skeletal model is shaped like a ring, and the "hexane" means there are 6 carbons in the ring. Prefix "hex" means 6.

Here's a photo of the unit review on Edge. Refer to the 2nd attachment for a visualization.

Please click the heart if this helped.

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3 years ago

Sodium metal reacts with water to produce hydrogen gas.

Darina [25.2K]

Answer:

Explanation:

Question 6 options:

1)

A single replacement reaction takes place because sodium is less reactive than hydroxide ions.

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2 years ago

Whats the difference between mass and volume

Lady bird [3.3K]

Answer: Volume – How much space an object or substance takes up. Mass – Measurement of the amount of matter in an object or substance.

Explanation:

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2 years ago

Read 2 more answers

The arsenic in a 1.223 g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, and

Vladimir79 [104]

Answer:

5.471% As₂O₃ in the sample.

Explanation:

<em>...the reaction is: Ag+ + SCN- => AgSCN(s) Calculate the percent As2O3 in the sample. (F.W. As2O3 = 197.84 g/mol).</em>

<em />

First, with the amount of KSCN we can find the moles of Ag in the filtrates. As we know the amount of Ag added we can know the precipitate of Ag and the moles of AsO₄ = 1/2 moles of As₂O₃ in the sample:

<em>Moles KSCN = Moles Ag⁺ in the filtrate:</em>

0.01127L * (0.100mol / L)= 0.001127moles Ag⁺

<em>Total moles Ag⁺:</em>

0.0400L * (0.0781mol/L) = 0.0031564 moles Ag⁺

<em>Moles of Ag⁺ in the precipitate:</em>

0.0031564 - 0.001127 = 0.0020294 moles Ag⁺

<em>Moles AsO₄ = Moles As:</em>

0.0020294 moles Ag⁺ * (1mol As / 3 moles Ag⁺) = 6.765x10⁻⁴ moles AsO₄

<em>Moles As₂O₃:</em>

6.765x10⁻⁴ moles AsO₄ * (1 mol As₂O₃ / 2 mol AsO₄) =

3.382x10⁻⁴ moles As₂O₃

<em>Mass As₂O₃:</em>

3.382x10⁻⁴ moles As₂O₃ * (197.84g/mol) = 0.0669g As₂O₃

Percent is:

0.0669g As₂O₃ / 1.223g sample * 100 =

<h3>5.471% As₂O₃ in the sample</h3>

<em />

7 0

3 years ago