(a) The percent composition of an unknown compound is 40.48% C,
34.66% O, 16.86% N, and 8.01% H. What is its empirical formula?
Show your work.
(b) What mass of H2O(l) will we produce when we do the
combustion of 15.0 g of C4H10(l) with an
excess of O2(g) to produce CO2(g) and
H2O(l)?
b.
Balanced equation for this reaction is ,
2C4H10 + 13O2 ---------> 8CO2 + 10H2O
2 moles of C4H10 gives 10 moles of H2O.
1 mole of C4H10 will give 5 moles of H2O.
Number of moles = Mass/Molar mass
Molar mass of C4H10 = 58.12 g/mol
Moles of C4H10 = 15/58.12
= 0.26 moles
Moles of H2O formed = 0.26 × 5
= 1.30 moles
Molar mass of H2O = 18 g/mol
Mass of H2O formed = 18 g/mol × 1.30 mol
= 23.4 grams of H2O
b.
Balanced equation for this reaction is ,
2C4H10 + 13O2 ---------> 8CO2 + 10H2O
2 moles of C4H10 gives 10 moles of H2O.
1 mole of C4H10 will give 5 moles of H2O.
Number of moles = Mass/Molar mass
Molar mass of C4H10 = 58.12 g/mol
Moles of C4H10 = 15/58.12
= 0.26 moles
Moles of H2O formed = 0.26 × 5
= 1.30 moles
Molar mass of H2O = 18 g/mol
Mass of H2O formed = 18 g/mol × 1.30 mol
= 23.4 grams of H2O
(a) The percent composition of an unknown compound is 40.48% C, 34.66% O, 16.86% N, and...
(a) The percent composition of an unknown compound is 46.23% C, 17.11% O, 26.96% N, and 9.70% H. What is its empirical formula? Show your work. (b) We must do the combustion of what mass of C4H10O(l) to produce a total mass of 73.4 g of product? Combustion is the reaction of a substance with O2(g) to produce CO2(g) and H2O(l).
(a) The percent composition of an unknown compound is 46.23% C, 17.11% O, 26.96% N, and 9.70% H. What is its empirical formula? Show your work. (b) We must do the combustion of what mass of C4H10O(l) to produce a total mass of 75.2 g of product? Combustion is the reaction of a substance with O2(g) to produce CO2(g) and H2O(l).
(a) The centetisimal composition of an unknown compound is 46.23% C, 17.11% O, 26.96% N, and 9.70% H. What is its empirical formula? Show your work. (b) What mass of C4H10O (l) must be burned in order to produce a total mass of 72.3 g of products? Combustion is the reaction of a substance with O2 (g) to produce CO2 (g) and H2O (l).
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