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Answer :
Final Answer:
When balloon is filled with 88 g of CO₂ at 15°C then the pressure in kPa is: c) 258.9 kPa
Explanation:
To find the pressure in the balloon, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. First, convert the given volume from liters to cubic meters. 23.8 L is equal to 0.0238 m³.
Next, convert the temperature from Celsius to Kelvin by adding 273.15. 15°C is equal to 288.15 K. Now, rearrange the ideal gas law equation to solve for pressure: P = nRT/V.
Calculate the number of moles (n) using the given mass of CO₂ (88 g) and the molar mass of CO₂ (44.01 g/mol). n = mass/molar mass. Plug in the values for n (moles), R (8.31 J/(mol·K)), T (temperature in Kelvin), and V (volume in cubic meters) into the rearranged equation.
Solve for pressure (P) in Pascals.
Convert the pressure from Pascals to kilopascals by dividing by 1000.
The final answer is c) 258.9 kPa
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