A 50.0 g of solid CO2 (dry ice) is added at -100°C to an evacuated (all of the gas removed) container with a volume of 5.0 L. if the container is sealed and allowed to warm to room temperature (25°C) so that the
entire solid CO2 is converted to gas, what is the pressure inside the container?

The Pressure  inside the container 5.56 atm

Explanation:

Given that:

the mass of CO2 = 50.0g

molar mass of CO2= 44 g/mol

So; the number of moles of CO2 = mass/molar mass

= 50.0 g/44 g/mol

= 1.1364 mol

Volume of the container = 5.0 L

Temperature = 25°C = ( 25+273.15)K = 298.15 K

universal gas constant R  = 0.08206 L atm mol⁻¹ K⁻¹

Using Ideal Gas Equation PV = nRT

P = nRT/V

P = (1.1364 × 0.08206  ×  298.15) / 5.0

P =  27.80337718/ 5.0

P = 5.560675436 atm

P ≅ 5.56 atm

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.