5. Would you expect the following reactions to be nearly complete? Why or why not? -31 a. N₂(g) + O₂(g) 2NO (g) Kc = 4.6 X 101 b. C₂H4(g) + H₂(g) C₂H6(g) Kc = 1.3 X 10 21

The molecular formula and the empirical formula for this hydrocarbon are a. C5 H10 and CH2 b. C5 H10  and CH3 c. C4H8 and CH2 d. C4H8 and CH3

PLEASE SHOW YOUR WORK (THIS IS NOT A GRADED ASSIGNMENT)

7. Consider the reaction: 2 ZnSe +3 02 )2 Zno s +2 SO,a Which value is closest to the mass of Zno a produced when 50.0 g ZnS is heated in an open vessel until no further weight loss is observed? (molar masses O, [32 g), So, [64 g), Zno [81 g], ZnS [97 g]) a. 25 g b. 40 g c. 50 g d. 60 g (s)

T Ma M PA USN Be * Ma E Ad G ph ph Do E Un O Ac. 6 Pec O Na O Pe Со Bas 3 Pe Stu "app.101edu.co Question 11 of 11 What is the mass in grams of H2 that can be formed from 55.8 grams of NH3 in the following reaction? 2 NH:(g) → 3 H:(g) + N:(g)

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00 %24 4+ dl w/ S' Enter your answer in the provided box. Using the balanced equation for the combustion of ethanol, answer the following question. C2H,O(1) + 3 02(g) – 2 CO2(g) + 3 H,0 (g) ethanol How many grams of H,0 are formed from 1.2 mol of ethanol? OH 8 #3 5. 9. 2 4 0O

Write a balanced chemical equation based on the following description: solid potassium oxide reacts with liquid water to produce aqueous potassium hydroxide

How many grams of oxygen gas (O2) is required for the complete combustion of 25.5 g of benzene (C6H6)? 2C6H6(1) + 1502(g) 12 CO2(g) + 6H2O(g)

2 NaHCO3 (s) → N22CO3 (s) + CO2 (g) + H2O (g) 1. Calculate the moles of NaHCO3 in 3.00 g of NaHCO3. 3,00 84 2. Using your answer to question one, if 1 mole of Na2CO3 is produced for every 2 moles of NaHCO3, how many moles of Na2CO3 would theoretically be produced in the reaction? 3. How many grams of Na2CO3 would theoretically be produced in the reaction? 4. If the actual mass of Na2CO3 produced is 1.25 g, what is the percent yield of Na2CO3? Actual yield (g) Theoretical yield (g) Percent yield = 100% 5. Calculate the theoretical mass of H2O produced from the decomposition of 3.00 g NaHCO3 using similar calculations as above.