Various members of a class of compounds, alkenes, react with hydrogen to produce a corresponding alkane. Termed hydrogenation, this type of reaction is used to produce products such as margarine. A typical hydrogenation reaction is C10H20() + H2(g) → C10H22(5) Decene Decane How much decane can be produced in a reaction of excess decene with 2.45 g hydrogen? Give your answer in scientific notation. O *10 g decane


Answer 1

Answer: The mass of decane produced is 1.743* 10^2g


To calculate the number of moles, we use the equation:  

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}       ......(1)

Mass of hydrogen gas = 2.45 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1:, we get:

\text{Moles of }H_2=(2.45g)/(2g/mol)=1.225mol

The chemical equation for the hydrogenation of decene follows:

C_(10)H_(20)(l)+H_2(g)\rightarrow C_(10)H_(22)(s)

As, decene is present in excess. So, it is considered as an excess reagent.

Thus, hydrogen gas is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of hydrogen gas produces 1 mole of decane.

So, 1.225 moles of hydrogen gas will produce = (1)/(1)* 1.225=1.225mol of decane

Now, calculating the mass of decane by using equation 1, we get:

Moles of decane = 1.225 mol

Molar mass of decane = 142.30 g/mol

Putting values in equation 1, we get:

1.225mol=\frac{\text{Mass of decane}}{142.30g/mol}\n\n\text{Mass of carbon dioxide}=(1.225mol* 142.30g/mol)=174.3g=1.743* 10^2g

Hence, the mass of decane produced is 1.743* 10^2g

Related Questions

The transamination of a-ketoglutarate leads to the formation of this amino acid A. Aspartate B. Glutamate C. Asparagine D. Glutamine E. Valine
Which of the following statement best defines matter?
The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of water from 25.1°C to 65.3°C?
(01.04 LC)What phase of matter has particles that are held together but can flow past eachother and takes the shape of a container, filling it from the bottom up? (3 points)1) Gas2) Liquid3) Plasma4) Solid
Determine the rate of a reaction that follows the rate law:rate = k[A]”[B]", where:k= 1.5[A] = 1 M[B] = 3 Mm = 2n = 1

Which of the following are properties of acids? Check all that apply. • A. Corrosive • B. Reacts with certain metals • C. Tastes bitter □ D. Turns litmus paper blue



a) Corrosive and b) Reacts with certain metals

Classify each of the following chemical reactions as a synthesis decomposition and single displacement or double displacement reaction


1. Synthesis reaction : there is only 1 product formed from 2 or more reactant


H_2(g)+N_2(g)\text{ }\Rightarrow2NH_3(g)\text{ }

2. Decomposition : reaction that occurs in presence of UV light and only 1 reactant that decomposes into 2 or more products.


CH_3Br(g)+UV_(light)\Rightarrow CH_3(g)\text{ + Br (g)}

3. Single displacement :reaction that occurs when 1 reactant displaces other reactant from its compound:


Zn(s)+CoCl_2(aq)\text{ }\Rightarrow ZnCl_2(aq)\text{ + Co(s)}

4. Double displacement :reaction that occurs when both reactant displaces each other.

E.g :

K_2S(aq)+Co(NO_3)_2\Rightarrow2KNO_3(aq)\text{ + }CoS(s)\text{ }

What would be the effect on the observed melting point of sample were poorly packed?


if a sample is packed poorly, the sample will not heat evenly and will take longer to melt.

During photosynthesis ____ energy is transferred into chemical energy.


Photosynthesis converts solar energy into chemical energy title

g Acetic acid is diluted with water to make a solution of vinegar. You have a sample of vinegar that contains 16.7 g of acetic acid. Determine the number of moles of acetic acid in the vinegar sample.



0.278 mol


Step 1: Given and required data

Mass of acetic acid (m): 16.7 g

Chemical formula of acetic acid: CH₃COOH (C₂H₄O₂)

Step 2: Calculate the molar mass (M) of acetic acid

We will use the following expression.

M(C₂H₄O₂) = 2 × M(C) + 4 × M(H) + 2 × M(O)

M(C₂H₄O₂) = 2 × 12.01 g/mol + 4 × 1.01 g/mol + 2 × 16.00 g/mol = 60.06 g/mol

Step 3: Calculate the number of moles (n) of acetic acid

We will use the following expression.

n = m/M

n = 16.7 g/(60.06 g/mol) = 0.278 mol

Complete combustion of 4.20 g of a hydrocarbon produced 12.9 g of CO2 and 6.15 g of H2O. What is the empirical formula for the hydrocarbon?


We calculate first the number of moles of CO2 and H2O produced by dividing the given masses by the molar masses of CO2 and H2O.
 moles CO2 = (12.9 g CO2) x (1 mole CO2 / 12 g CO2) = 1.075 moles.
 moles H2O = (6.15 g H2O) x (1 mole H2O / 18 g H2O) = 0.36 moles
Then, we count the number of C, H, and O moles. This gives us 1.075 moles C, 2.5 moles O and 0.72 moles H. The empirical formula is,