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3 years ago

Given the Vapour Density of a hydrocarbon is 150, what is it's molecular formula.

1 answer:

6 0

Molecular formula = C4H10.

or

Simplest ratio
Empirical formula mass = 12 1 + 1 1+ 16 1 = 29.

Molecular mass = 2 vapour density. = 2 58. = 116.

Molecular formula mass = n Empirical formula mass.

Molecular formula = n Empirical formula.

= 4 (CHO)

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Consider this reaction: 6 CO2 + 6 H2O + light equation C6H12O6 + 6 O2 If there were 2.38 x 102 g of H2O, 18.6 moles of CO2, and

alisha [4.7K]

H₂O would be the limiting reactant.

Balanced chemical equation:

6CO₂ + 6H₂O + light equation → C₆H₁₂O₆ + 6O₂

The amount of product that can be created is constrained by the reactant that is consumed first in a chemical reaction, commonly referred to as the limiting reactant (or limiting reagent).

Given

No. of moles of CO₂ = 18.6

Mass of H₂O = 2.38 × 10² g = 238g

No. of moles of H₂O = Given mass/ Molar mass

= 238 / 18 = 13.22 moles

Moles of H₂O = 13.22

According to the balanced chemical equation

6 moles of CO₂ react with 6 moles of H₂O

So the reactant that has less number of moles will be consumed first.

As the No. of moles of H₂O < No. of moles of CO₂

So, H₂O is the limiting reactant with 13.22 moles.

Hence, H₂O would be the limiting reactant.

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7 0

1 year ago

Consider the following gas phase reaction:

snow_tiger [21]

Answer:

2NO(g) + O2(g) --> 2NO2(g)

now 400 ml of NO × 2 mol of NO2/2 mol of NO

= 400 ml of NO2

now 500 ml of O2 × 2 mol of NO2/1 mol of O2

= 1000 ml of NO2

now 400 ml of NO2 × 1 mol of O2/2 mol of NO

= 200 ml

subtract that from 500 ml of total i.e. 500-200 =300 ml

The total volume of the reaction mixture is 1000 ml -300ml = 700 ml

6 0

2 years ago

DUPLICATE. The half-equivalence point of a titration occurs half way to the end point, where half of the analyte has reacted to

Law Incorporation [45]

At the half equivalence point [HA] = [A-] and pH = pKa

<span>if Ka is 5.2e-5 then pKa = pH = 4.28</span>

5 0

3 years ago

2C2H2(g)+5O2(g)=4CO2(g)+2H2O(g)

balandron [24]

The volume of ethyne, C₂H₂ required to produce 12 moles of CO₂ assuming the reaction is at STP is 134.4 L

<h3>Balanced equation</h3>

2C₂H₂(g) + 5O₂(g) --> 4CO₂(g) + 2H₂O(g)

From the balanced equation above,

4 moles of CO₂ were produced by 2 moles of C₂H₂

<h3>How to determine the mole of C₂H₂ needed to produce 12 moles of CO₂</h3>

From the balanced equation above,

4 moles of CO₂ were produced by 2 moles of C₂H₂

Therefore,

12 moles of CO₂ will be produce by = (12 × 2) / 4 = 6 moles of C₂H₂

<h3>How to determine the volume (in L) of C₂H₂ needed at STP</h3>

At standard temperature and pressure (STP),

1 mole of C₂H₂ = 22.4 L

Therefore,

6 moles of C₂H₂ = 6 × 22.4

6 moles of C₂H₂ = 134.4 L

Thus, we can conclude that the volume of C₂H₂ needed for the reaction at STP is 134.4 L

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3 0

2 years ago

4. If the DNA nitrogen bases were TACCGGAT, how would the other half of

Elena L [17]

Answer:

<u>ATGGCCTA</u>

Explanation:

For this we have to keep in mind that we have a <u>specific relationship between the nitrogen bases</u>:

-) <u>When we have a T (thymine) we will have a bond with A (adenine) and viceversa</u>.

-) <u>When we have C (Cytosine) we will have a bond with G (Guanine) and viceversa</u>.

Therefore if we have: TACCGGAT. We have to put the corresponding nitrogen base, so:

TACCGGAT

<u>ATGGCCTA</u>

<u></u>

I hope it helps!

6 0

2 years ago

Given the Vapour Density of a hydrocarbon is 150, what is it's molecular formula.​

Given the Vapour Density of a hydrocarbon is 150, what is it's molecular formula.