True or False ?? 2H2 + O2 → 2H2O indicates that 2grams of H2 react with one gram of O2
It indicates that 2 moles of hydrogen reacts with one mole of oxygen
Or 2 Litres of hydrogen reacts with 1 litre of hydrogen
So the correct option is false
True or False ?? 2H2 + O2 → 2H2O indicates that 2grams of H2 react with...
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= ?
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?
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
For the reaction 2H2O(g)−⇀↽−2H2(g)+O2(g) the equilibrium concentrations were found to be [H2O]=0.250 M, [H2]=0.340 M, and [O2]=0.750 M. What is the equilibrium constant for this reaction?
The elementary reaction 2H2O(g)−⇀↽−2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H2O, H2, and O2 reach 0.0750 atm, 0.00850 atm, and 0.00650 atm, respectively. What is the value of the equilibrium constant at this temperature?
A chemist knows that the
kJ for the reaction 2H2(g) + O2
(g) ---> 2H2O (g) ,and that
kJ
for the reaction H2 (g) + F2 (g) ---> 2HF
(g).
With this information he calculated the
for the reaction 2H2O (g) + 2F2
(g) ---> 4HF(g) + O2 (g) and
predicted whether
was positive or negative. How?
A Ho- 485
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?
Consider the reaction 2H2(g) + O2(g) +2H2O(g) Using standard thermodynamic data at 298, calculate the entropy change for the surroundings when 1.75 moles of H2(e) react at standard conditions. surroundings JK AS Submit Answer Retry Entire Group 9 more group attempts remaining
Using the equation 2H2(g) + O2(g) --> 2H2O(g), what formula would I use to find the mass needed of H2 to react with 13.5 g O2? A. 13.5 g O2 x 1 mol O2 x 1 mol H2 x 2 g H2 1 32 g O2 2 mol O2 1 mol H2 B. 13.5 g O2 x 32 g O2 x 2 mol H2 x 2 g H2 1 1 mol O2 1 mol O2 1 mol H2 C. 13.5 g O2...
Given the equilibrium constants for the following reactions: 2H2(g) + O2(g) → 2H2O(g) K1 = 3.74 x 1026 H2(g) + Cl2(g) → 2HCl(g) K2 = 9.73 x 1012 calculate the equilibrium constant for the reaction below. 4HCl(g) + O2(g) → 2Cl2(g) + 2H2O(g)