Phosphorus reacts with oxygen to form diphosphorus pentoxide, P2O5P2O5. 4P(s)+5O2(g)⟶2P2O5(s)4P(s)+5O2(g)⟶2P2O5(s) How many grams of P2O5P2O5 are formed when 4.71 g 4.71 g of phosphorus reacts with excess oxygen? Show the unit analysis used for the calculation by placing the correct components into the unit-factor slots. g P2O5g P2O5 4.71 g P×()×()×()=4.71 g P×(1)×(1)×(1)=

Phosphorus reacts with oxygen to form diphosphorus pentoxide, P2O5P2O5. 4P(s)+5O2(g)⟶2P2O5(s)4P(s)+5O2(g)⟶2P2O5(s) How many grams of P2O5P2O5 are formed when 4.71 g 4.71 g of phosphorus reacts with excess oxygen? Show the unit analysis used for the calculation by placing the correct components into the unit-factor slots. g P2O5g P2O5 4.71 g P×()×()×()=4.71 g P×(1)×(1)×(1)=

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 47A

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Phosphorus reacts with oxygen to form diphosphorus pentoxide, P2O5P2O5. 4P(s)+5O2(g)⟶2P2O5(s)4P(s)+5O2(g)⟶2P2O5(s) How many grams of P2O5P2O5 are formed when 1.85 g 1.85 g of phosphorus reacts with excess oxygen? Show the unit analysis used for the calculation by placing the correct components into the unit-factor slots.
The equation for the complete combustion of butane gas (C4H10) is : 2C4H10+ 13O2 8CO2+ 10H2O Measured under the same conditons, how many liters of carbon dioxide are produced when 0.250 liters of butane gas is burned?
A fuel mixture used in the early days of rocketry consisted of two liquids, hydrazine (N2H4) and dinitrogen tetroxide, which ignite on contact to form nitrogen gas and water vapor. How many grams of the excess reactant remain unreacted when 164.8 g of hydrazine react with 150.0 g of nitrogen tetroxide?
How many grams of P2O5P2O5 are formed when 9.51 g 9.51 g of phosphorus reacts with excess oxygen? Show the unit analysis used for the calculation by placing the correct components into the unit-factor slots.
When exposed to air, aluminum metal, AlAl, reacts with oxygen, O2O2, to produce a protective coating of aluminum oxide, Al2O3Al2O3, which prevents the aluminum from rusting underneath. The balanced reaction is shown here: 4Al+3O2→2Al2O3 a) What is the theoretical yield of aluminum oxide if 3.00 molmol of aluminum metal is exposed to 2.55 molmol of oxygen? Express your answer with the appropriate units.
320.4 grams of isomaltitol, C12H24O11, was combusted in a furnace completely in an excess oxygen. The products of this reaction are liquid water and gaseous carbon dioxide. How much water (in kg) do you expect from this reaction assuming that all of the isomaltitol reacts? Enter your numeric answer in the units of kg. Do not enter the unit. Use enough significant digits to prevent rounding errors. Hint: balance the reaction first. Recall that 1 kg = 1000 g.
1. Many metals react with halogens to give metal halides. For example, iron reacts with chlorine to give iron (II) chloride, FeCl2. Fe(s) + Cl2(g) FeCl2(s). Beginning with 10.0 g iron, what mass of Cl2, in grams, is required for complete reaction? What quantity of FeCl2, in moles and in grams, is expected? 2. Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane reacting with excess water yields 270 kg of H2, what is the percentage yield? C3H8(g) + 3 H2O(l) 3 CO(g)+ 7 H2(g). 3. What volume of 0.812 M HCl, in milliliters, is required to titrate 1.45 g of NaOH to the equivalence point? NaOH(aq) + HCl(aq) : H2O(l) + NaCl(aq)
Consider the reaction:Fe(s)+Cl2(g)→FeCl3(s) How many moles of chlorine gas react with 0.300 molmol of metallic iron? Express your answer with the appropriate units.
A side reaction in the manufacture of rayon from wood pulp is 3CS2+6NaOH→2Na2CS3+Na2CO3+3H2O How many grams of Na2CS3 are produced in the reaction of 92.5 mL of liquid CS2 (d = 1.26 g/mL) and 2.61 mol NaOH? Express your answer with the appropriate units.
12. The gaseous hydrocarbon acetylene, C2H2C2H2, used in welders’ torches, burns according to the following equation:2C2H2(g)+5O2(g)→4CO2(g)+2H2O(g) A. What is the theoretical yield, in grams, of CO2CO2, if 26.6 gg of C2H2C2H2 completely reacts? Express your answer with the appropriate units. B. If the actual yield in part a is 64.1 g of CO2CO2, what is the percent yield of CO2CO2 for the reaction? Express your answer with the appropriate units.
The last step in the production of nitric acid is represented by the following equation: 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) Calculate the moles of nitric acid produced when 4.43 mol of nitrogen dioxide react with excess water. Record only your final answer rounded to the correct number of significant digits and include proper units Pure methanol, CH3OH(l), combusts very quickly. 2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(g) If 46.5 mol of methanol undergoes complete combustion, what mass of water, in kilograms, will be produced? Record only your final answer rounded to the correct number of significant digits and include proper units.
Ammonia (NH3) is an important compound since it is used in large amounts for the manufacture of nitrogenous fertilizers, nylon and many other important compounds. It is manufactured industrially by the catalytic reaction between nitrogen between nitrogen and hydrogen, according to the following equation; N2(g) + H2(g) ⇌ NH3(g) When 0.120 mol nitrogen and 1.20 mol hydrogen are mixed together in a closed vessel, 30% of the nitrogen is converted into ammonia. a. Calculate the moles of nitrogen gas that will be present in the vessel? (only 3 decimal places) b. Calculate the moles of hydrogen gas that will be present in the vessel? (only 3 decimal places c. Calculate the moles of ammonia gas that will be present in the vessel? (only 3 decimal places) d. What is the number of moles of nitrogen gas that has reacted? (only 3 decimal places) Blank 4. Fill in the blank, read surrounding text. mol d. What mass of ammonia can be produced from the limiting reactant? (only 3 decimal places