Question

Nitrogen dioxide is reacted with water according to the following equation. We start with 1.85 x 10 ² g nitrogen dioxide and we have excess water. If 95.0 grams HNO₃ is produced, what is the percent yield?   
3NO₂ + H₂O → 2HNO₃   + NO
Hint: find theoretical yield
Hint: percent yield =(actual yield/ theoretical yield) x 100

When 325 g Al and 812 g Cl2 react according to the following equation, how much AlCl3 can be made, assuming 100 percent yield? 2Al   +   3Cl2    → 2AlCl3   38.0g 11.2 g 1.02 x 10 3 g 96.2 g 13.0 g 48.1 g 916 g 895 g

Answer 1

Given 3 NO₂ + 4₂0 - 2HNO₃ + NO moles of NO₂ = e 1.85010² molar mass of NO. 1.85 X102 46.005 Now, - 4.021 mole. produus 3 moles of NO2 - . 4.6g) mole of N02 x a mole il #NO; (2x4.021 Janole of HNO3 Xlow, ... 4.021 mole of No2 2.68 mole of HNO₃ mole of HNO3 - 63.01 g 2.68 mole of HNO - 63.01x2.68 = 168.92 g. & Theoretical y eilda 168.92g. do yeild = percent actual yeild actual yeild X100 & 95 x 100 Theoretical geild 168-92 =96.23 of

mole of Al= 325 - atomic mase of Al = 12.04 moles 325 26.98 812 812 70.906 - 11.45 moles. Tº = molar mass och produce Here ca is the tiniting rescent. e Giron Equation. 2A + 30. - 2A1C13 Xlow, 3 moles of ch luce a 2 moles of AICI :. 11.45 mole of the produce 3 (2 xl. 4s) = 7-63 moles of Ailly Xlow, linole of Allls - . 13 3.349 . 9.63 mole of Alch - 133.34 x=1-63 = 1017 g 6. Amount of Alch produceda 1.017 X10 = 1.02x103 g e correct option. © 1.02 X1089
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