What pressure in kPa is exerted by 94.60 g CO2 at 57.00 ℃ in 0.7500 L?

7,859.9829 kPa

Explanation:

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables where R is the molar constant of the gases:

P * V = n * R * T

Then the pressure can be calculated as:

Equation (A)

In this case R is a known constant and the volume and temperature are given as data. The number of moles n can be calculated from the molar mass. You know:

Then the molar mass of CO₂ is:

CO₂= 12 g/mole + 2*16 g/mole=  44 g/mole

Now you can apply the following rule of three: if 44 g are contained in 1 mole of CO₂, 94.6 g in how many moles are they?

moles= 2.15

Then you know the following data:

Replacing in Equation (A):

Solving:

P= 77.572 atm

Knowing that 1 atm is equal to 101.325 kPa, then 77.572 atm is 7,859.9829 kPa

b..

is the correct one

explanation:

covalent bonds form as valence electrons are shared between two atoms. lewis structures and structural formulas are common ways of showing the covalent bonding in organic molecules. formal charge describes the changes in the number of valence electrons as an atom becomes bonded into a molecule.