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Report (any type)/Brief report
22/09/2021
The volume at STP is 882 mL. The volume at 25 °C and 1.01 atm is 941 mL.
Step 1. Convert grams of ##”CaC”_2## to moles of ##”CaC”_2##.
##2.49 cancel(“g CaC₂”) × (“1 mol CaC”_2)/(64.10 cancel(“g CaC₂”)) = “0.038 85 mol CaC”_2##
Step 2. Use the molar ratio from the balanced equation to convert moles of ##”CaC”_2″## to moles of ##”C”_2″H”_2##.
##”CaC”_2 + “2H”_2″O” → “Ca(OH)”_2 + “C”_2″H”_2″##
##0.038 85 cancel(“mol CaC₂”) × (“1 mol C”_2″H”_2)/(1 cancel(“mol CaC₂”)) = “0.038 85 mol C”_2″H”_2##
Step 3. Use the Ideal Gas Law to calculate the volume of ##”C”_2″H”_2## at STP.
STP is defined as a pressure of 100 kPa and a temperature of 273.15 K.
##PV = nRT##
##V = (nRT)/P = (0.038 85 cancel(“mol”) × 8.314 cancel(“kPa”)”·L·”cancel(“K⁻¹mol⁻¹”) × 273.15cancel(“K”))/(100 cancel(“kPa”)) = “0.882 L” = “882 mL”##
The volume at STP is 882 mL.
Step 4. Use the Ideal Gas Law to calculate the volume at 25 °C and 1.01 atm.
##V = (nRT)/P = (0.038 85 cancel(“mol”) × 0.082 06 “L·”cancel(“atm·K⁻¹mol⁻¹”) × 298.15cancel(“K”))/(1.01 cancel(“atm”)) = “0.941 L” = “941 mL”##
The volume at 25 °C and 1.01 atm is 941 mL.
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I want to thank your team (Jeff) for finding a new writer when you were unable to reach my existing writer to revise my paper. I appreciate your professionalism and efforts. Thanks
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