Consider the reaction 2H2(g)+O2(g)→2H2O(l) What is the mass of water, H2O(L), produced when 5.20g of O2(g) reacts with excess H2(g)?
I am not sure how to proceed. I don't have a lot of sleep. working and going to school both full time. The 2nd part of this is..... Molar masses of isotopes The molar mass (in grams per mole) of any isotope can be approximated by its mass number. For example, the molar mass of H (also symbolized as 1H) is very close to its mass number of 1. Similarly, the molar mass of D (also symbolized as 2H) can be approximated by its mass number of 2. Part C Consider the reaction 2D2(g)+O2(g)→2D2O(l) What is the mass of heavy water, D2O(l), produced when 5.20g of O2(g) reacts with excess D2(g)?
Consider the reaction 2H2(g) + O2(g)<==> 2H2O(g) at some equilibrium position.using the following choices?
C. No change At equilibrium there's a balance. The size of the vessel won't affect the equilibrium. There will be greater pressure, but that will not affect the equilibrium.
Consider the following reaction 2H2(g) +O2(g) →2H2O(l) ΔH=-572 KJ?
a. How much heat is evolved for the production of 1.00 mol H2O(l) ? b. How much heat is evolved when 4.03 g hydrogen is reacted with excess oxygen? c. How much heat is evolved when 186 g oxygen is reacted with excess hydrogen d. The total volume of hydrogen gas needed to fill the Hindenburg was 2.0x 108L at 1.0 atm and 25 °C. How much heat was evolved when the Hindenburg exploded, assuming all of the hydrogen reacted?
Consider the reaction 2H2(g)+O2(g)→2H2O(g)?
If this reaction were done at STP, what volume in liters of H2 gas would be required to react completely with 22.4 L of O2 gas? What volume in liters of H2O(g) would be produced?
Consider the following reaction: 2H2 + O2 ---> 2H2O delta(rxn)H=-483.6kJ/mol?
a) reaction is exothermic , energy is getting released ( evolved ) . b) it is -483.6 x 6 / 2 = -1450.8 kJ / mole . c) it is -483.6 x 3.5 / 4 = -423.15 kJ / mole .
Consider the following reaction. 2H2 + O2 ---> 2H2O. Change of H(rxn) = -484kJ.?
Which answer best describes the transfer heat that occurs when 1.5o mol of H2 reacts? a. 726 kJ absorbed b. 363 kJ absorbed c. 484 kJ absorbed d. 726 kJ released e. 363 kJ released f. 484 kJ released g.
Consider the following reaction: 2H2O2(aq)→2H2O(l)+O2(g) Use the graph to calculate the following.?
The instantaneous rate of formation of O2 at 50s. 2. If the initial volume of the H2O2 solution is 1.6 L , what total amount of O2 (in moles) is formed in the first 50 s of reaction?
Consider the following reaction 2H2+O2 gives 2H2O. What gram of H2 is formed if 2G of H2 reacts with 1G of O2?
moles of O2 are :- 1gm/16moles of H2 are :- 2gm/1Now, according to the reaction,1 mole of O2 gives 2 mole of H2OTherefore, 1/16 moles will give (1/16)x2 moles.Taking H2 case,2 moles of H2 will give 2 moles of H20,But 1 mole per result mole is more than what O2 has which is (1/16)th of a mole.Thus, O2 will stop the reaction long before H2 finished and thus, becoming the limiting reagent.Thus, the mass of H20 = (1/16)*2*18Where 18 is the molar mass of H2O…..
94) Consider the reaction: 2H2 + O2------>2H2O...Identify the limiting reagent in each of the reaction...?
In this reaction you need: 2molecules of H2 and 1molecule of O2: a) OK 50:25 = 2:1 = no limiting reactant b) Ratio = 1:1 H2 is short so is limiting reactant c) 0.8mol :0.75mol Not enough H2 - should be 1.5mol:0.75mol . H2 limiting reactant.