Question

If the rate of appaerance of O2 in the reaction: 2O3 (g)-->3O2(g) is .250 M/s over...

If the rate of appaerance of O2 in the reaction: 2O3 (g)-->3O2(g) is .250 M/s over the first 5.50 , how much oxygen will form during this time. Please explain!

Homework Answers

Answer #1

rate = 0.250 M / s

time = 5.50 sec

cocentration of O2 produced = rate x time

                                              = 0.250 x 5.50

                                             = 1.375 M

O2 produced = 1.38 M

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Find ΔHrxn for the following reaction: 3S(s,rhombic)+2O3(g)→3SO2(g) Use the following reactions with known ΔH values: S(s,rhombic)+O2(g)3O2(g)→→SO2(g)2O3(g)ΔH=−296.8...
Find ΔHrxn for the following reaction: 3S(s,rhombic)+2O3(g)→3SO2(g) Use the following reactions with known ΔH values: S(s,rhombic)+O2(g)3O2(g)→→SO2(g)2O3(g)ΔH=−296.8 kJΔH=+285.4 kJ Express the energy to one decimal place and include the appropriate units.
Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4Fe(s)+3O2(g)⟶2Fe2O3(s)4Fe(s)+3O2(g)⟶2Fe2O3(s) Suppose 12.3 g12.3 g...
Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4Fe(s)+3O2(g)⟶2Fe2O3(s)4Fe(s)+3O2(g)⟶2Fe2O3(s) Suppose 12.3 g12.3 g of iron (Fe)(Fe) is reacted with 21.0 g21.0 g of oxygen (O2).(O2). Select the limiting reagent. FeFe Fe2O3Fe2O3 O2O2 Calculate the theoretical yield of iron(III) oxide (Fe2O3Fe2O3). theoretical yield = g The reaction produces 5.63 g5.63 g of Fe2O3.Fe2O3. What is the percent yield of the reaction? percent yield =
Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s) What volume of O2...
Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s) What volume of O2 gas (in L), measured at 783 mmHg and 33 ∘C, is required to completely react with 52.1 g of Al?
Given the following chemical reaction 4Al(s) + 3O2(g)=2Al2O3(s). If 10.0grams of Al and 19.0gram of O2...
Given the following chemical reaction 4Al(s) + 3O2(g)=2Al2O3(s). If 10.0grams of Al and 19.0gram of O2 are mixed together how many moles of each reactants you have. b) how many moles of the product you will form c) which of these two reactant is the limiting reactant d) what is the theoritical yield of this reaction (in gram) e) If 15.0grams of Al2O3 was obtained, what is the percent yield of this reaction.
1) Elemental S reacts with O2 to form SO3 according to the reaction 2S+3O2→2SO3 A) How...
1) Elemental S reacts with O2 to form SO3 according to the reaction 2S+3O2→2SO3 A) How many O2 molecules are needed to react with 3.25 g of S? B) What is the theoretical yield of SO3 produced by the quantities described in Part A? 2) 1.05 g H2 is allowed to react with 9.71 g N2, producing 1.15 g NH3. A) What is the theoretical yield in grams for this reaction under the given conditions? Express your answer to three...
Elemental S reacts with O2 to form SO3 according to the reaction 2S+3O2→2SO3 Part A: How...
Elemental S reacts with O2 to form SO3 according to the reaction 2S+3O2→2SO3 Part A: How many O2 molecules are needed to react with 8.03 g of S? Express your answer numerically in units of molecules Part B: What is the theoretical yield of SO3 produced by the quantities described in Part A? Express your answer numerically in grams.
Question 2 options: Consider this reaction: 2S(s) + 3O2(g) à 2SO3(g) You begin the reaction with...
Question 2 options: Consider this reaction: 2S(s) + 3O2(g) à 2SO3(g) You begin the reaction with 7 moles of S and 9 moles of O2. Fill in each blank with a whole number (including 0) to make the statements true. The theoretical yield is ________ moles of SO3. After the theoretical yield is achieved, there will be________ moles of S left over and ______ moles of O2 left over.
Consider the following reaction: 2 N2O(g) → 2 N2(g)+O2(g) In the first 10.0 s of the...
Consider the following reaction: 2 N2O(g) → 2 N2(g)+O2(g) In the first 10.0 s of the reaction, 1.7×10−2 mol of O2 is produced in a reaction vessel with a volume of 0.430 L . What is the average rate of the reaction over this time interval?
Catalysts Catalysts are substances that increase the rate of reaction but can be recovered unchanged at...
Catalysts Catalysts are substances that increase the rate of reaction but can be recovered unchanged at the end of the reaction. Catalysts can be classified as either homogeneous (same state as reactants) or heterogeneous (different state than reactants). Part A Platinum is used to catalyze the hydrogenation of ethylene: H2(g)+CH2CH2(g)−⟶Pt(s)CH3CH3(g) Chlorofluorocarbons (CFCs) catalyze the conversion of ozone (O3) to oxygen gas (O2): 2O3(g)−⟶CFC(g)3O2(g) Magnesium catalyzes the disproportionation of hydrogen peroxide to produce water and oxygen: 2H2O2(aq)−⟶Mg(s)2H2O(l)+O2(g) What type of catalysts...
use the following equilibria to calculate kc for the reaction. S(s)+O2(g) ><SO2(g)K'c=4.2×10^-52 2S(s)+3O2(g)><2SO2(g)Kc=9.8×10^128 calcuate kc for...
use the following equilibria to calculate kc for the reaction. S(s)+O2(g) ><SO2(g)K'c=4.2×10^-52 2S(s)+3O2(g)><2SO2(g)Kc=9.8×10^128 calcuate kc for the reation 2SO2(g)+O2><2SO3(g)