Question 2 (2 points) 4) Listen How many grams of carbon dioxide gas are in a 1.0-L balloon at STP? 0.045 g 2.08 22.4 Question 3(2 points)

## Step 1:At Standard Temperature and Pressure (STP), 1 mole of any gas occupies 22.4 Liters.### **n = \frac{V}{22.4}**Here, we first need to find out how many moles of CO2 would occupy 1.0L volume at STP. The number of moles ( ) can be calculated by the formula , where is the volume.## Step 2:Substitute the given volume into the formula:### **n = \frac{1.0L}{22.4L/mol} = 0.0446 mol**So, we have 0.0446 moles of CO2.## Step 3:Since we know the molar mass of CO2 (1mol of C = 12.01 g, and 2mol of O = 2*16.00 g = 32.00 g. So the molar mass of CO2 = 12.01 g + 32.00 g = 44.01 g), we can now calculate the mass of these moles of CO2.### **m = n \times \text{Molar mass}**## Step 4:Substitute the number of moles and the molar mass into the formula:### **m = 0.0446 mol \times 44.01 g/mol = 1.96 grams**So, the mass of CO2 that would occupy a 1.0 L balloon at STP is 1.96 grams.#