It is known that 0 5 moles of hydrocarbon are completely burned to produce 56 liters of carbon dioxi

Calculate the amount of matter of c and h with the conservation of elements.

56, CO2 is, indicating that there is a c atom, in the same way 54 18 = 3, there is 3molH2O, so there is 6mol of H atom.

In summary, the hydrocarbon has a C atom and a 6mol H atom, and the molecular formula is C5H12

This hydrocarbon is generated, about = 6molh

So the molecular formula is: C5H12

That is, pentane. The isomers are:

Also known as n-pentane (without branched chains), isopentane (with one branched chain), neopentane (with two branched chains).

The molecular formula of this hydrocarbon is C5H12 isomers are CH3CH2CH2CH2CH3CH3CH(CH3)CH2CH3 (CH3)4C

They are pentane, isopentane, and neopentane.

First write the reaction equation CXHY+(X+Y4)O2 XCo2+Y2 H2O, after a hydrocarbon is completely combusted, it produces 56L (standard condition) carbon dioxide gas and 54 grams of water, that is, 56 carbon dioxide and 54 18=3mol water. You can solve x=5 y=12 so the hydrocarbon is c5h12

C5H1256L fit.

54g to 3mol

So 1mol of hydrocarbons gives 5mol CO2 and 6mol H2OC:H=5:12

A C produces a CO2. So 56 , CO2 is, indicating that there is a c atom, and in the same way 54 18=3, there is 3molH2O, so there is a 6mol h atom.

In summary, the hydrocarbon has a C atom and a 6mol H atom, and the molecular formula is C5H12

First, we need to determine the molecular formula of the hydrocarbon. Since the hydrocarbon is completely burned to produce water and carbon dioxide, we can list the following reaction formulas:

cnhm + n + m/4)o2 → nco2 + m/2 h2o

where n and m represent the number of carbon and hydrogen in the hydrocarbon molecule, respectively. According to the reaction formula, the mass ratio of water to carbon dioxide produced should be:

9 g h2o / 22 g co2 =

This ratio can be converted into molar ratios, i.e.:

2 mol H2O with 1 mol CO2

So, based on the molar ratio of the generated, we can get the number of moles of the generated CO2 as:

22 g / 44 g/mol = mol

The number of moles of water generated is the key car:

9 g / 18 g/mol = mol

Since this hydrocarbon is completely combusted, the number of moles of the product should be equal to the number of moles of the fuel. Therefore, the molar number of this hydrocarbon is:

mol CO2 = mol H2O = mol hydrocarbon.

The molar mass of the hydrocarbon is:

Molar mass = mass Molar number = 22 g + 9 g) mol = 310 g mol

Next, we need to calculate the molar mass of the molecule based on its chemical formula and try to match the above results. Assuming that the molecular formula of this hydrocarbon is CNH2N, according to the reaction formula, the following chemical formula can be listed:

cnh2n + 3n/2)o2 → nco2 + nh2o

where n is the number of carbon atoms in the hydrocarbon molecule. Based on the above calculation of molar mass, we can get:

Molar mass = n 12 g mol + 2n 1 g mol = 310 g mol

Solving the equation gives n = 10. Thus, the hydrocarbon has the molecular formula C10H20 which is a decane alkane.

Finally, we find the amount of heat released when burning. When alkanes are completely combusted, the energy produced is only the bond energy of the C-H bond and the C-C bond in the hydrocarbon, regardless of heat loss and other reactions. According to the reaction formula, the heat released by combustion is:

h = n × hc(c-h) ×m + hc(c-c) ×n-1))

where δhc(c-h) and δhc(c-c) are the standard heat of combustion for c-h and c-c bonds, respectively, and m is the number of carbon atoms in each molecule of the hydrocarbon. According to the criteria of common keys.

n(h)=n(h) n(hydrocarbon)=2*n(h2o) n(hydrocarbon)=2*n(c)=n(c) n(hydrocarbon)=n(CO2) n(hydrocarbon)=so the hydrocarbon is C6H12

If the hydrocarbon can not discolor the bromine water, but under certain conditions can substitute with pure bromine, and there is a bromine substitution substance, the hydrocarbon belongs to the [naphthenic hydrocarbon], and the structure is simply [(the figure is not easy to play, draw a regular hexagon)] The name is [cyclohexane].

If the hydrocarbon can discolor bromine water, and the hydrocarbon is added with hydrogen under the action of a catalyst to form 2,2-dimethylbutane, then the structure of the simple formula (CH3)3CCH=CH2 is called [3,3-dimethyl1-butene], and the polyaddition reaction that occurs under the action of the catalyst is written as N(CH3)3CCH=CH2 - catalyst-> CH=CH2-]N-

c（ch3）3

It's 1mol, and the water is.

There is 1 mol of C in 1 mol of CO2, and the original organic matter is only, so there is 10 C in water and 18 H

The chemical formula is C10H18

The molar mass is 120 + 18 = 138g mol

c2h2

The amount of matter of c is.

The amount of substance of h is.

The gaseous hydrocarbon contains c atom and h atom, so it is c2h2

The molecular formula of this hydrocarbon is cxhy

The amount of the substance of carbon dioxide is the amount of the substance of water.

CXHy+(x+y 4)O2 ignites XCo2+y 2H2O1 x y 2

x=2 y=2

So the molecular formula of this hydrocarbon is C2H2

If a hydrocarbon is completely burned in a sufficient amount of oxygen to produce water and carbon dioxide, then n(c)= in the hydrocarbon molecule

6、n（h）=

Catalyst catalyst.

Carbon = grams, equivalent to.

Contains the hydrogen = grams, which is equivalent to.

That is, each mole of the auspicious or hydrocarbon contains 2 moles of carbon, 4 moles of hydrogen per mu, C2H4, ethylene.

The amount of substance of c is repentant 44=

The amount of the substance of h

c: H = Wide: 4

A of the pre-branched C2H4

Analysis: +xO2 + H2O is expanded by a factor of 10, then there is:

1CNHM + XO2 --6CO2 + 6 H2OC, H is conserved, then n=6 m=12

So the molecular formula of this hydrocarbon is C6H12

cxhy + x+y/4)o2 ==xco2 + y/2h2o1 . x y/2

Solve the system of equations to obtain: x=6 y=12

Therefore, the structure of this hydrocarbon is simply C6H12

Solution: Let the chemical formula of the hydrocarbon be cxhy, and the chemical equation of combustion is:

CXHy+(x+y 4)O2 ignites XCo2+Y 2H2O1 Y 2*18

x=4y=8

Then the ratio of the number of carbon and hydrogen atoms in the hydrocarbon molecule is 4:8=1:2, and the molecular formula of the hydrocarbon is C4H8