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Determine whether each of the following chemical equations is balanced or not balanced:
a.
b.
c.
d.
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Chapter 7 Solutions
Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: An Introduction to General, Organic, and Biological Chemistry (13th Edition)
- For the following balanced reaction, how many moles of NO are formed from 4.50 moles of NO2 if there is plenty of water present? NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)arrow_forwardWhen N2O5 (g) is heated it dissociates into N2O3 (g) and O2 (g) according to the reaction: N2O5 (g) ↔ N2O3 (g)+ O2 (g) Kc = 7.75 at a given temperature. The N2O3 (g) dissociates to give N2O (g) and O2 (g) according to the reaction: N2O3 (g) ↔ N2O (g) and O2 (g) Kc = 4.00 at the same temperature. 4.00 moles of N2O5 (g) is heated in a 1.00L reaction vessel to this temperature. Find the concentrations of all the other species in the equilibrium system.arrow_forwardWhat is the product in the following equation after it is properly balanced? __Li(s) + __N2(g) --> ?______ (A) 2Li2N(s) (B) 2Li3N(s) (B) Li3N2(s) (D) LiN2(s)arrow_forward
- 3 KOH (aq) + H3PO4 (aq) → K3PO4 (aq) + 3 H2O (l) In this reaction, 25.800 g of KOH reacts with 14.723 g of H3PO4; 4.120 g of H2O are formed. Calculate the theoretical yield (g) and % yield of H2O.arrow_forwardIt takes _______ moles of Ca(OH)2 (aq) to react _______ moles of H3PO4 (aq). Ca(OH)2 (aq) + 2 H3PO4 (aq) → Ca(H2PO4)2 (aq) + 2 H2O (aq) [balanced]arrow_forwardGiven the reaction below, how many moles of Na 2SiO 3 are required to react completely with 0.914 moles of HF? 8HF (aq) + Na 2SiO 3 (s) -> H 2SiF 6 (aq) + 2NaF (aq) + 3H 2O (l) 7.31 moles Na2SiO3 0.171 moles Na2SiO3 1.09 moles Na2SiO3 0.114 moles Na2SiO3arrow_forward
- For the reaction Ti(s) + 2F2(g) --> TiF4(s) compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants. a) 7.0 g Ti, 7.0 g F2 b) 2.6 g Ti, 1.8 g F2 c) 0.239 g Ti, 0.296 g F2arrow_forwardRefer to this equation: 3SCl2 + 4NaF --> SF4 + S2Cl2 + 4NaCl 64.0 grams SCl2 is reacted with excess NaF and 12.5 grams of SF4 is formed. What is percent yield SF4? Hint: find theoretical yieldHint: percent yield =(actual yield/ theoretical yield) x 100arrow_forwardDetermine how many moles of sodium sulfate are needed to react with 2.08 moles of aluminum nitrate. 3Na2SO4(aq) + 2Al(NO3)3(aq) --> 6NaNO3(aq) + Al2(SO4)3(s)arrow_forward
- The reaction of nitric acid with calcium carbonate produces calcium nitrate, carbon dioxide, and water. Determine the correct balanced equation for this reaction. Question 1 options: 2HNO3(aq) + CaCO3(s) → CaNO3(aq) + CO2(g) + H2O(l) HNO3(aq) + CaCO3(s) → Ca(NO3)2(aq) + CO2(g) + H2O(l) 2HNO3(aq) + CaCO3(s) → Ca(NO3)2(aq) + CO2(g) + H2O(l) 2HNO3(aq) + 2CaCO3(s) → 2Ca(NO3)2(aq) + 2CO2(g) + 2H2O(l) HNO3(aq) + CaCO3(s) → CaNO3(aq) + CO2(g) + H2O(l) Question 2 A compound contains only nitrogen and oxygen. Determine the empirical formula of the compound if a sample is found to contain 46.67 % nitrogen by mass. Question 2 options: N22 N2O5 N NO N2O Question 3 Determine the moles of CaCO3 in 275 g of CaCO3. Question 3 options: 0.364 4.57 × 10–22 2.75…arrow_forward1.) For the following chemical reaction: KClO3(s) -----> KCl(s) + O2(g) a. Balance the reaction b. Determine the type of reaction c. Calculate the number of moles of O2 produced from 3.50 moles of KClO3 d. Calculate the number of moles of KCl produced from 3.50 moles of KClO32. For the following chemical reaction: N2(g) + H2(g) -------> NH3(g) a. Balance the reaction: b. Name the type of reaction: c. Determine the limiting reagent from 42.0g of N2 and 8.00g H2: d. Calculate the theoretical yield: e. Calculate the percent yield if the actual yield of NH3 in the reaction was 38.8arrow_forwardWhich of the following reaction is not balanced? a. BaO + 2 HCl → BaCl2 + H2O b. 2 SO2 + O2 → 2 SO3 c. 2 C2H6 + 7 O2 → 4 CO2 + 6 H2O d. Ca + 2 H2O → Ca(OH)2 + 2 H2arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
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