Answer:
1) A. 0.0515 L
2) B. 35.504 L
3) B. 422.446 g
Explanation:
At STP, you have 0.101 g of carbon dioxide gas. What is the volume of this gas?
Step 1: Data given
Mass of CO2 gas = 0.101 grams
Molar mass of CO2 = 44.01 g/mol
STP = 1 atm and 273K
Step 2: Calculate moles CO2
Moles CO2 = mass CO2 / molar mass CO2
Moles CO2 = 0.101 grams / 44.01 g/mol
Moles CO2 = 0.0023 moles
Step 3: Calculate the volume
For 1 mol at STP we have 22.4L
0.0023 moles we have 22.4L * 0.0023 = 0.0515 L
<u>Option A is correct</u>
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You have 27g of ammonia (nitrogen trihydride) at STP. What is the volume? Hint...you will first need to convert mass of ammonia to moles!
Step 1: Data given
Molar mass of NH3 = 17.03 g/mol
Mass of NH3 = 27.00 grams
STP = 1 atm and 273K
Step 2: Calculate moles NH3
Moles NH3 = 27.00 grams / 17.02 g/mol
Moles NH3 = 1.585 moles
Step 3: Calculate volume
For 1 mol at STP we have 22.4 L
For 1.585 moles we have 22.4 * 1.585 = 35.504 L
<u>Option B is correct</u>
<u />
Which of the following represents the MASS of 215 L of dinitrogen monoxide at STP? Hint...find the # of moles of this gas and then use the molar mass to go from moles to mass!
Step 1: Data given
Volume = 215 L
STP = 1 atm and 273 K
Molar mass of N2O = 44.01 g/mol
Step 2: Calulate moles N2O
22.4L = 1 mol at STP
215 L = 215 / 22.4 = 9.60 moles
Step 3: Calculate mass N2O
Mass N2O = moles N2O * molar mass N2O
Mass N2O = 9.60 moles* 44.01 g/mol
Mass N2O = 422.446 g
<u>Option B is correct</u>
