Carbon monoxide reacts with oxygen to form carbon dioxide.

2 co(g) + o2(g) → 2c02(8)

in a 1.00 l flask, 3.40 atm of co reacts with 2.60 atm of o2. assuming that the temperature remains constant, what is the final pressure in the flask?

4.30 atm

2.60 atm

3.40 atm

6.00 atm

The total pressure in the flask =  4.30 atm

Explanation:

Step 1: Data given

Volume of the flask = 1.00 L

Pressure of CO = 3.40 atm

Pressure of O2 = 2.60 atm

Step 2: The balanced equation

2 CO(g) + O2(g) → 2C02

Step 3: Calculate the final pressure

3.40 atm of CO reacts with 1.70 atm of O2

There will remain 2.60 - 1.70 = 0.90 atm O2

There will be produced 3.40 atm of CO2

The total pressure in the flask = 0.90 atm + 3.40 atm = 4.30 atm

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-

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the atomic number of carbon is six, which means that a carbon atom has six protons. carbon has three naturally occurring isotopes: carbon-12, carbon-13, and carbon-14. which of these statements are true about carbon and its isotopes? select all that appl