What is the ratio of carbon to oxygen in the following balanced equation: 2C + O2–> 2CO

Chemistry

2 answers:

Morgarella [4.7K]2 years ago

7 0

Answer:

The ratio is 2:1, that is 2mol C / 1mol O2

Explanation:

First check to see if the equation is balanced. It is so now let's find the ratio.

The ratio is the stoichiomeric coefficient of the element or compound.

Carbon : Oxygen

2C : 1 O2 , so 2:1 ..

NemiM [27]2 years ago

4 0

<u>Answer:</u> The mole ratio of carbon and oxygen in the given chemical reaction will be 2 : 1

<u>Explanation:</u>

Mole ratio is defined as the ratio of number of moles of the two substances taken into account or the ratio of their respective stoichiometric coefficients.

The given chemical equation follows:

$2C+O_2\rightarrow 2CO$

Moles of carbon atom = 2

Moles of oxygen gas = 1

Moles of carbon monoxide gas = 2

So, the mole ratio of carbon and oxygen = 2 : 1

Hence, the mole ratio of carbon and oxygen in the given chemical reaction will be 2 : 1

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11111nata11111 [884]

An ionic bond because ca is a metal and cl is a nonmetal which is an ionic bond

5 0

2 years ago

1 C8H10(l) +21/2O2(g) → 8CO2(g) + 5H2O(g), Hcomb= ? Hf for C8H10(l) = +49.0kJ/mol C8H10(l) Use the balanced combustion reaction

nikklg [1K]

Answer:

$H_{comb}=-4406kJ/mol$

Explanation:

Hello,

In this case, the enthalpy of combustion is understood as the energy released when one mole of fuel, in this case octene, is burned in the presence of oxygen and is computed with the enthalpies of formation of the fuel, carbon dioxide and water as shown below (oxygen is circumvented as it is a pure element):

$H_{comb}=8*\Delta _fH_{CO_2}+5\Delta _fH_{H_2O}-\Delta _fH_{C_8H_{10}}$

Thus, since we already know the enthalpy of combustion of the fuel, for carbon and water we have -393.5 and -241.8 kJ/mol respectively, thereby, the enthalpy of combustion turns out:

$H_{comb}=8*(-393.5kJ/mol)+5(-241.8kJ/mol)-49.0kJ/mol\\\\H_{comb}=-4406kJ/mol$