In the carbon cycle, combustion reactions produce atmospheric oxygen.
True
False
The empirical formulas for H2O, H2O2, NH3, N2H4, C12H22O11, and Al2Cl6 are H2O, HO, NH3, NH2, C12H22O11, and AlCl3, respectively.
True
False
The combustion reaction of hydrocarbons, in the presence of excess oxygen, will produce carbon monoxide and water.
True
False
Stoichiometry of a chemical reaction refers to the quantitative relationships between the amounts of reactants and products involved in the reaction.
True
False
The percent composition of a substance is the number of moles of each element in the compound divided by the number of moles of the compound.
True
False
The actual yield (experimentally determined) of a chemical reaction is almost always larger than the theoretical yield because of side reactions, incomplete reactions, and loss during purification steps. The percent yields for most reactions are less than 100%.
True
False
In the carbon cycle, combustion reactions produce atmospheric oxygen.
In photosynthesis to produced oxygen
True >>>>answer
The empirical formulas for H2O, H2O2, NH3, N2H4, C12H22O11, and Al2Cl6 are H2O, HO, NH3, NH2, C12H22O11, and AlCl3, respectively.
True >>>>answer
The combustion of hydrocarbons in presence of excess of oxygen to produce CO2 , H2O
The combustion reaction of hydrocarbons, in the presence of excess oxygen, will produce carbon monoxide and water.
False >>>answer
Stoichiometry state the mass -mass, volume-volume, mass-volume relation ship between reactant and products.
Stoichiometry of a chemical reaction refers to the quantitative relationships between the amounts of reactants and products involved in the reaction.
True >>>>answer
The percent composition of a substance is the number of moles of each element in the compound divided by the number of moles of the compound.
True >>>>answer
percent yield = actual yield*100/theoretical yield
actual yield always less than the theoretical yield .
False >>>answer
In the carbon cycle, combustion reactions produce atmospheric oxygen. True False The empirical formulas for H2O,...
Not yet answered Graded out of 1.00 Flag question Question text In the process of photosynthesis, water and carbon dioxide are produced. Select one: True False Question 2 Not yet answered Graded out of 1.00 Flag question Question text In the carbon cycle, combustion produces atmospheric oxygen. Select one: True False Question 3 Not yet answered Graded out of 1.00 Flag question Question text In a balanced chemical equation, the number of each type of atom in the reactants must...
12. Combustion reactions take place between a fuel and oxygen and produce carbon dioxide and water. Balance the following combustion reaction. DC2H6O + CO2 CO2 + H2O
yield of chemical reactions Liquid hexane (cr, (CH2),CH) reacts with gaseous oxygen gas (02) to produce gaseous carbon dioxide (CO) and gaseous water (H2O) If 27.9 g of water is produced from the reaction of 28.44 g of hexane and 134.4 g of oxygen gas, calculate the percent yield of water Round your answer to 3 significant figures.
a) 0.07. Short Answer Questions (True (a) or False (b)) 14. The numbers preceding the formulas for a compound in chemical equations are referred to as the moles 15. The actual yield of a chemical reaction is calculated by multiplying its limiting reagent by the molecular weight of the product. 16. The pH of purified water (or of a neutral solution) is 7.80. 17. The reaction of 2.75 g N; with excess Hz produces 1.77g NHs. The percent yield of...
Liquid hexane CH3CH24CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . If 13.8g of water is produced from the reaction of 77.56g of hexane and 104.0g of oxygen gas, calculate the percent yield of water. Round your answer to 3 significant figures.
22) Given that 4 NH3 +50,-- 4 NO:6 HO.if 3.00 mol NHy were made to react with excess of oxygen gas, the amount of H2O formed would be: A) 4.50 mol B) 2.00 mol. C) 6.00 mol. D) 3.00 mol. E) none of the above 23) Which of the following statements is FALSE? A) The actual yield is the amount of product actually produced by a chemical reaction. B) The percent yield - Actual Yield Theoretical Yield"100 C) The limiting...
cal 22) Given that 4 NH3 5 O2-4 NO+6 HyO, if 3.00 mol NH3 were made to react with excess of 22) Oxygen gas, the amount of H2O formed would be A) 4.50 mol. B) 2.00 mol. C) 6.00 mol. D) 3.00 mol. E) none of the above 23) Which of the following statements is FALSE? A) The actual yield is the amount of product actually produced by a chemical reaction. B) The percent yield- 23) Actual Yield Theoretical Yield...
Gaseous ethane CH3CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O If 8.38g of water is produced from the reaction of 9.32g of ethane and 45.5g of oxygen gas, calculate the percent yield of water. Be sure your answer has the correct number of significant digits in it.
Question 1 0.5 When table sugar is burned in presence of oxygen, carbon dioxide and water vapor are produced according to the unbalanced chemical equation: C12H22011(s) + 02(9) - CO2(g) + H2O(g) How many moles of oxygen are required to react completely with 2.70 mol of sugar? 47 O 32.4 - 65 2.70 O None of these Question 2 0.5 pts Consider the reaction of magnesium metal with hydrochloric acid to produce magnesium chloride and hydrogen gas. If 3.65 mol...
A. Classify each of the following reactions as decomposition, combination, combustion, 2CH3OH(l)+3O2(g)→2CO2(g)+4H2O(g) 2KClO3(s)→2KCl(s)+3O2(g) S(s)+3F2(g)→SF6(g) CaO(s)+H2O(l)→Ca(OH)2(aq) 2Cu(NO3)2(s)→2CuO(s)+4NO2(g)+O2(g) B. Solid aluminum metal and diatomic chlorine gas react spontaneously to form a solid product. Give the balanced chemical equation (including phases) that describes this reaction. Indicate the phases using abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively. Express your answer as a chemical equation. C. When heated, solid copper(II) carbonate decomposes to solid copper(II) oxide and carbon dioxide gas. Give...