12:13 .ll LTE Question 5 of 14 Submit Determine the number of molecules of Cr2O3 that form when 1.34 x 103g of oxygen completely reacts according to the following equation: 4 Cr(s) + O2(g) → 2 Cr203(s) х STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 3 4 mol O2 mol Cr 1.34 × 103 1.68 x 1025 g Cr2O3 32.00 3.78 x 1025 mol Cr2O3 2.52 x 1025 152.00 g O2 52.00 g Cr 4.24 x 103 molecules Cr2O3 6.022 x 1023 Tap here or pull up for additional resources

Remaining Time! 02:29:4. Consider the balanced chemical equations shown below. When a 6.00 g sample of a mixture of iron (Fe) and aluminum (Al) is treated with excess HCl(aq), 0.177 moles of H2 are obtained. What is the mass percentage of Fe in the original mixture? Choose the closest answer. Fe(s) + 2 HCI(aq) FeCl2(aq) - + H2(g) 2 Al(s) +6 HC((aq) 2 AICI3(aq) + 3 H2(g) 96 % 69 % 47 % 33 % 17 % Rack Question Menu - O O

11:11 AM Sun Oct 22 < Question 16 of 34 13% % Submit If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 5.0 mol of NO₂ were collected, then what is the percent yield for the reaction? 2 NO (g) + O₂(g) → 2 NO2 (g)

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