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
Equation needed to balanced: H2 + O2 ----> H2O
#Option A : H2 + O2 ----> H2O2
This is an incorrect option. As the reaction says there should be H2O on the right side but here it is H2O2.
#Option B : 2H2 + O2 ----> 2 H2O
As the number of hydrogen and oxygen is the same on both sides, so this is the correct option.
#Option C: H2 + O2 ----> H2O
As here the no. of oxygen on the left side is 2 and on right side, it is one, so this is unbalanced. This is an incorrect option.
#Option D: H2 + 2O2 ----> 4H2O
As here the no. of hydrogen on the left side is 2 and on the right side, it is 8, so this is unbalanced. This is an incorrect option.
Option B is correct.
The equation H2+O2 arrow to the right H2O be balanced by changing it to: A. H2+O2...
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
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?
When 5.58g H2 react by the following balanced equation, 32.8 g H2O are formed. What is the percent yield of the reaction? 2H2(g)+O2(g)?2H2O(g) Select the correct answer below: 17.0 % 65.7 % 11.7 % 38.9 %
From the following balanced equation, 2H2(g)+O2(g)⟶2H2O(g) how many molecules of H2O can be formed from 5.58mol H2?
If 1.97g of H2 reacts with 2.77g of O2 according to the balanced reaction below, calculate the theoretical yield of H2O. 2H2(g) + O2(g) ⟶ 2H2O(g)
9. C3H8 + 5O2 ---> The reactants of a chemical equation are given above. In a balanced chemical equation, the products could be a. 4CO2 + 3H2O b. 3CO2 + 4H2O c. 2CO2 + 3H2O d. 3CO + 4H2O 10. Mg + 2HCl ---> MgCl2 + H2 If 24.31g of Mg react completely with 72.92g of HCl, according to the reaction above, how many total grams of product should be formed? a. 24.31g b. 72.92g c. 97.23g d. The reaction...
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
For the reaction 2H2O(g)−⇀↽−2H2(g)+O2(g)2H2O(g)↽−−⇀2H2(g)+O2(g) the equilibrium concentrations were found to be [H2O]=0.250 M,[H2O]=0.250 M, [H2]=0.490 M,[H2]=0.490 M, and [O2]=0.750 M.[O2]=0.750 M. What is the equilibrium constant for this reaction?
The elementary reaction 2H2O(g)−⇀↽−2H2(g)+O2(g)2H2O(g)↽−−⇀2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H2O,H2O, H2,H2, and O2O2 reach 0.0200 atm,0.0200 atm, 0.00550 atm,0.00550 atm, and 0.00700 atm,0.00700 atm, respectively. What is the value of the equilibrium constant at this temperature? kp= ?
Given the thermochemical equation for the formation of H2O by burning H2 and O2: H2(g) + 402 (8) → H2O (8) ΔH° = -241.8 kJ Calculate the ΔH for the following reaction: 2H2O (g) → 2 H2(g) + O2 (g)