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

sorry idk the answer well to you i have a explaination

explanation: a formula which shows the arrangement of atoms in the molecule of a compound

in scientific notation, the value of the  speed of light in a vacuum

  will be written as 2.995 * 10^8. when this value is represented in the form of

  a * 10^b, then, a = 2.995 and b = 8.

the value of the speed of light in a vacuum given above can also be rounded up to approximately 300000000. in this case, the scientific notation will be written as 3 *10^8.