Open Question
Complete and balance each combustion reaction equation: a. C(s) + O2(g) → b. C3H8O(l) + O2(g) → c. CS2(s) + O2(g) → d. C4H6(g) + O2(g) →
Ch.4 - Chemical Quantities & Aqueous Reactions
Chapter 4, Problem 25
Consider the unbalanced equation for the combustion of hexane: C6H14(g) + O2(g) → CO2(g) + H2O(g). Balance the equation and determine how many moles of O2 are required to react completely with 7.2 moles of C6H14.
Verified step by step guidance1
Write the unbalanced chemical equation: \( \text{C}_6\text{H}_{14}(g) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(g) \).
Balance the carbon atoms by ensuring the number of \( \text{CO}_2 \) molecules equals the number of carbon atoms in hexane: \( \text{C}_6\text{H}_{14}(g) + \text{O}_2(g) \rightarrow 6\text{CO}_2(g) + \text{H}_2\text{O}(g) \).
Balance the hydrogen atoms by ensuring the number of \( \text{H}_2\text{O} \) molecules equals half the number of hydrogen atoms in hexane: \( \text{C}_6\text{H}_{14}(g) + \text{O}_2(g) \rightarrow 6\text{CO}_2(g) + 7\text{H}_2\text{O}(g) \).
Balance the oxygen atoms by adjusting the \( \text{O}_2 \) molecules: \( \text{C}_6\text{H}_{14}(g) + 19\text{O}_2(g) \rightarrow 6\text{CO}_2(g) + 7\text{H}_2\text{O}(g) \).
Use the balanced equation to determine the moles of \( \text{O}_2 \) needed for 7.2 moles of \( \text{C}_6\text{H}_{14} \) by multiplying the moles of \( \text{C}_6\text{H}_{14} \) by the ratio of \( \text{O}_2 \) to \( \text{C}_6\text{H}_{14} \) from the balanced equation.
Related Practice
Open Question
Consider the balanced equation: 2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g). Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms. Mol N2H4 Mol N2O4 Mol N2 Mol H2O 2 _____ _____ _____ _____ 5 _____ _____ _____ _____ _____ 10 _____ _____ 11.8 _____ 2.5 _____ _____ _____ _____ 4.2 _____ _____
Open Question
We prepare a solution by mixing 0.10 L of 0.12 M sodium chloride with 0.23 L of a 0.18 M MgCl2 solution. What volume of a 0.20 M silver nitrate solution is needed to precipitate all the Cl- ions in the solution as AgCl?
Textbook Question
Consider the unbalanced equation for the neutralization of acetic acid: HC2H3O2(aq) + Ba(OH)2(aq) → H2O(l) + Ba(C2H3O2)2(aq) Balance the equation and determine how many moles of Ba(OH)2 are required to completely neutralize 0.461 mole of HC2H3O2.
1998
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Open Question
Calculate how many moles of NO2 form when each quantity of reactant completely reacts.
Reaction: 2 N2O5(g) → 4 NO2(g) + O2(g)
a. 15.2 g N2O5
b. 6.8 mol N2O5
c. 2.87 kg N2O5
Textbook Question
Calculate how many moles of NO2 form when each quantity of reactant completely reacts. 2 N2O5( g) → 4 NO2(g) + O2(g) a. 2.5 mol N2O5
6124
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