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

- "the choice that is not an indicator of a chemical change is "state of matter changes". more common than not, chemical reactions produce energy in the form of light or heat. along with energy, they also produce a new substance called the product that could be in any state of matter (solid, gas, or liquid)."

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