The compound H2O can be decomposed to form H2 and O2. This can be represented at the atomic level by a chemical equation: 2H2O 2H2 + O2 According to the law of conservation of mass, if 26.8 grams of H2O decomposes and 3.0 grams of H2 is formed, how many grams of O2 must simultaneously be formed?
_____grams O2
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The compound H2O can be decomposed to form H2 and O2. This can be represented at...
The compound NH, NO, can be decomposed to form N, and H.O. This can be represented at the atomic level by a chemical equation NH NON + 2H1,0 According to the law of conservation of mass, if 28.3 grams of NH NO, decomposes and 12.4 grams of N, is formed, how many grams of H.O must simultaneously be formed? grams H2O The compound NH, can be formed by combining N2 and H. This can be represented at the atomic level...
How many grams of H2O will be formed when 31.78 mol H2 is mixed with 2.64 mol of O2 and allowed to react to form water according to the reaction below? 2H2 + O2 -----> 2H2O (Note: Determine the limiting reagent first)
QUESTION 14 Balance this equation: H2 + O2 -> H2O 3H2 + O2 + 5H2O 2H2 + 202 + 4H2O 2H2 + O2 + 2H2O H2 + 402 - 3H2O Click Save and Submit to saue and submit. Click Save All Answers to sau. . 99+ AS
How many grams of H2O will be formed when 31.78 mol H2 is mixed with 2.64 mol of O2 and allowed to react to form water according to the reaction below? 2H2 + O2 -----> 2H2O (Note: Determine the limiting reagent first) 7.3 g 286 g 23.6 g 94.6 g 144 g
The equation H2+O2 arrow to the right H2O be balanced by changing it to: A. H2+O2 arrow to the right H2O2 B. 2H2+O2 arrow to the right 2H2O C. Nothing needs to be done; it is already balanced D. H2+2O2 arrow to the right 4H2O
Consider the following balanced equation: 2H2 + O2 --------> 2H2O If you start with 8.133 g of H2 and 3.425 g of O2, find the following: a) With excess O2, what mass (grams) of H2O would be produced by the H2? b) With excess H2, what mass (grams) of H2O would be produced by the O2? c) What is the chemical formula for the limiting reactant?
The following thermochemical equation is for the reaction of hydrogen(g) with oxygen(g) to form H2O(g). 2H2(g) + O2(g) 2H2O(g) AH=-484 kJ How many grams of H2(g) would have to react to produce 61.5 kJ of energy? grams
From the following balanced equation, 2H2(g)+O2(g)⟶2H2O(g) how many molecules of H2O can be formed from 5.58mol H2?
Water can be decomposed into O2 and H2 gas by applying electricity in a process called electrolysis. Calculate the mole fractions and partial pressures of O2 and H2 if 125.0 g of H2O is completely decomposed. Assume the reaction is done in a 10.0 L container at 20 celcius.
Consider the following chemical reaction. 2H2O(l)→2H2(g)+O2(g) What mass of H2O is required to form 1.3 L of O2 at a temperature of 310 K and a pressure of 0.948 atm ? Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00 atm and 23 ∘C, how many liters of carbon dioxide are formed by the combustion of 4.00 g of butane?