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Using the equation in Sample 6.8, calculate the grams of
Chapter 6, Problem 8SC(choose chapter or problem)
Using the equation in Sample 6.8, calculate the grams of CO2 that can be produced when 25.0 g of O2 reacts.Sample 6.8When acetylene, C2H2, burns in oxygen, high temperatures are produced that are used for welding metals. How many grams of CO2 are produced when 54.6 g of C2H2 is burned?Solution Step 1 State the given and needed quantities.Analyze the 2 Write a plan to convert the given to the needed quantity (mole or grams).grams of C2H2 Step 3 Use coefficients to write mole?mole factors; write molar mass factors if needed.
Questions & Answers
QUESTION:
Using the equation in Sample 6.8, calculate the grams of CO2 that can be produced when 25.0 g of O2 reacts.Sample 6.8When acetylene, C2H2, burns in oxygen, high temperatures are produced that are used for welding metals. How many grams of CO2 are produced when 54.6 g of C2H2 is burned?Solution Step 1 State the given and needed quantities.Analyze the 2 Write a plan to convert the given to the needed quantity (mole or grams).grams of C2H2 Step 3 Use coefficients to write mole?mole factors; write molar mass factors if needed.
ANSWER:Solution 8SCStep 1 of 2:Here, we are asked to calculate the grams of CO2 that can be produced when 25.0 g of O2 reacts, using the equation in Sample Problem 6.8.Equation: Given:Mass of O2 = 25.0 gMass of CO2 =Molar mass of O2 = 31.998 g/molAccording to the equation given, 1 mole of O2 = 31.998 g of O2. So, the mole-mass factor will be: and 5 moles of O2 = 4 moles of CO2. So, the mole-mole factor will be: and And, 1 mole of CO2 = 44.01 g of CO2. So, the mole-mass factor will be: and ________________