Nitrogen dioxide (NO,) gas and liquid water (H,0) react to form aqueous nitric acid (HNO3) and nitrogen monoxide (NO) gas. Suppose you have 9.0 mol of NO, and 13.0 mol of H,O in a reactor. Calculate the largest amount of HNO, that could be produced. Round your answer to the nearest 0.1 mol. 3. I mol x10

SS a. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.255 mol of the first reactant were to react completely. CO₂(g) + 4H₂(g) → CH4 (g) + 2H₂O (1) mol CH₂ mol H₂O b. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.790 mol of the first reactant were to react completely. BaCl₂ (aq) + 2AgNO3(aq) → 2AgCl(s) + Ba(NO3)2 (aq) mol AgCl mol Ba(NO3)2 c. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.815 mol of the first reactant were to react completely. C3H8 (9)+502(g) → 4H₂O(1) + 3CO2(g) mol H₂O mol CO2 Submit Answer Retry Entire Group Show Hint 9 more group attempts remaining 19 Previous Next

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Fernando is doing his pre-lab homework for Chemistry. He is asked to predict how many grams of CO, are produced if 2.09 mol of HCl are reacted according to this balanced chemical equation shown. CaCO3 +2 HCI → CaCl2 + CO2 + H20 He performs the following calculation. 1molEo, 2 metHCT 2.09 motHCI x 44.01 g CO. = 46.0 g CO, 1molEo, of the balanced On the day of the lab his group obtains 31.21 grams of CO2 as their experimental result. What is their percent yield in standard notation?