FeadingsedsParagraph5) For the following reaction:L (g) +H. (g) → 2HI (g)If the amount consumed from (L.) according to the above reaction is (50.8g) and theactual yield of HI is (40g) then the percentage yield of (HI) is equal to :a) 78.125%b) 15.625%c) 63.341%d)39.06% .6) The remaining mass of (92g) of HNO, if reacted with (24g) of LiOH accordingto the equation:HNO+LIOH → LINO, + H. Oa) 46b) 29c) 2d) 112) The mass of potassium hydroxide (KOH) to be dissolved in (100 ml) of water to

Given reaction is : H2 (g) + I2 (g) <----------> 2HI (g) Actual yield of HI = 40 g The…

Answered: 5) For the following reaction: L (g) +…

Chemistry: Matter and Change

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Chapter11: Stoichiometry

Section11.4: Percent Yield

Problem 29PP

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Chlorine gas was first prepared in 1774 by C. W. Scheele by oxidizing sodium chloride with manganese(IV) oxide. The reaction is NaCl(aq)+H2SO4(aq)+MnO2(s)Na2SO4(aq)+MnCl2(aq)+H2O(l)+Cl2(g) Balance this equation.
Small quantities of oxygen gas can be generated in the laboratory by the decomposition of hydrogen peroxide. The unbalanced equation for the reaction is H2O2(uz/)-? H2O(/) + O2(g) Calculate the mass of oxygen produced when 10.00 g of hydrogen peroxide decomposes.
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Consider the hypothetical reaction between A2 and AB pictured below. What is the balanced equation? lf 2.50 moles of A2 are reacted with excess AB, what amount (moles) of product will form? If the mass of AB is 30.0 u and the mass of A2 are 40.0 u, what is the mass of the product? If 15.0 g of AB is reacted, what mass of A2 is required to react with all of the AB, and what mass of product is formed?
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5) For the following reaction: L (g) + H. (g) → 2HI (g) If the amount consumed from (I) according to the above reaction is (50.8g) and the actual yield of HI is (40g) then the percentage yield of (HI) is equal to : a) 78.125% b) 15.625% c) 63.341% d)39.06% .