Consider the reaction 2H2(g) + O2(g) +2H2O(l) What is the mass of water, H.O(l). produced when...
Consider the reaction 2H2(g)+O2(g)→2H2O(l) What is the mass of water, H2O(l), produced when 5.20 g of O2(g) reacts with excess H2(g)? PLEASE HELP
Given: 2H2 (g) + O2 (g) --> 2H2O (l) Calculate the mass of water produced if 3.50 L O2 is at 1.25 ATM at 22.0oC reacting with excess H2. 4.55 L sample of CO2 has a pressure of 1.12 ATM. If the pressure is increased to 2.50 ATM what would be the resulting volume? Assume constant temp and no change in moles of gas. B) 4.55 L of He is at 25.0oC in a balloon. If the temp is increased...
Consider the reaction: 2H2O (l) ----> 2h2 (g) + O2 (g) What mass of H2O (MW=18.02) is required to form 1.4 L of O2 at a temperature of 30.0 degrees C and a pressure of 750 torr?
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?
Hydrogen is burned according to the following chemical reaction: 2H2(g) + O2(g) → 2H2O(l) ∆Hrxn = -286 kJ Given 100 g of H2 and excess O2, how much heat is released?
a)What is the mass of heavy water D2O produced when 5.20g of O2 reacts with excess D2? b)What is the mass of water H2O,produced when 5.20g of O2 reacts with excess H2 Consider the reaction 2D2+O2->2D2O Can someone step me through this?
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?
Hydrogen gas reacts with oxygen to form water. 2H2(g)+O2(g)→2H2O(g)ΔH=−483.5kJ2H2(g)+O2(g)→2H2O(g)ΔH=−483.5kJ Determine the minimum mass of hydrogen gas required to produce 233 kJkJ of heat.
consider the following reaction 2H2(g)+O2(g)--> 2H2O (I) delta H= -572KJ A) how much heat is evolved when 1.00 mole of H2O (I) is produced? B) how much heat is evolved when 4.03g H2 are reacted with 40.0g of O2? C) the total volume of hydrogen gas needed to fill the Hindenburg was 2.0*10^8 L at 1.0 atm and 25 degree C. How much HEAT was evolved when the Hidenburg exploded, assuming all of the hydrogen reacted (plenty of oxygen)?
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?