Question

Verizon 8:58 PM 1%D * Question 6 of 10 Submit Determine the number of molecules of Cr2O3 that form when 1.34 x 103 g of oxygen completely reacts according to the following equation: 4 Cr(s) + 3 02(g) → 2 Cr2O3(s) STARTING AMOUNT ADD FACTOR ANSWER RESET - 1.34 x 103 4.24 x 103 g Cr 52.00 2.52 x 1025 mol Cr N| دی 32.00 3.78 x 1025 g 02 152.00 mol O2 6.022 x 1023 1.68 x 1025 g Cr2O,

Answer 1

4 Cr(s) + 3O2(g) ---------------- 2Cr2O3(s)

                3 mole                      2 mole

mass of O2= 1.34x10^3 grams

molar mass of O2 = 32.0 gram/mol

number of moles of O2 = mass/molar mass = 1.34 x10^3 / 32.0 = 41.875 moles

number of moles ofO2= 41.875 moles

according to equation

3 moles of O2 = 2 moles of Cr2O3

41.875 moles of O2 = ?

                                  = 41.875 x 2 / 3 = 27.92 moles of Cr2O3

number of moles of Cr2O3 formed = 27.92 moles

number of molecules present in one mole of Cr2O3 = 6.022x10^23 molecules

number of molecules present in 27.92 moles of Cr2O3 = ?

                                                                                      = 27.92 x 6.022 x10^23 = 168.16 x 10^23 molecules

number of molecules of Cr2O3 formed = 168.16 x 10^23 molecules. = 1.68 x10^25 molecules.

Answer 2

wrong answer