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 following balanced equation: 2H2 + O2 --------> 2H2O If you start with 8.133 g...
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
From the following balanced equation, 2H2(g)+O2(g)⟶2H2O(g) how many molecules of H2O can be formed from 5.58mol H2?
Using the equation 2H2(g) + O2(g) --> 2H2O(g), what formula would I use to find the mass of H2O produced from 13.5 g O2 and 1.5 g H2? A. 1.5 g H2 x 1 mol H2 x 2 mol H2O x 18 g H2O 1 2 g H2 2 mol H2 1 mol H2O B. 13.44 g O2 x 1 mol O2 x 2 mol H2O x 18 g H2O 1 32 g O2 1 mol O2 1 mol H2O...
Consider the reaction 2H2(g) + O2(g) +2H2O(l) What is the mass of water, H.O(l). produced when 6.25 g of O2(g) reacts with excess H2(g)?
Based on the following chemical equation: 4HCN + 5O2 -> 2N2 + 4CO2 + 2H2O Identify the limiting reactant and the mass of N2 produced when 100.0 g of HCN react with 100.0 g of O2. Enter the chemical formula of the limiting reactant. The reactant that is present in excess will be (enter the chemical formula): The mass of N2 produced will be g. (3 sig figs will be sufficient) QUESTION 17 Based on the following chemical equation: 4HCN 502...
Based on the following chemical equation: 4HCN + 5O2 -> 2N2 + 4CO2 + 2H2O Identify the limiting reactant and the mass of N2 produced when 100.0 g of HCN reacts with 100.0 g of O2. Enter the chemical formula of the limiting reactant _________________________________. The reactant that is present in excess will be (enter the chemical formula): ____________________________. The mass of N2 produced will be _____________________________ g. (3 sig figs will be sufficient)
6)Using the balanced equation: SiO2 + 6HF → H2SiF6 + 2H2O, if 40.0 g SiO2 and 40.0 g HF react, determine: a) how many grams of H2SiF6 are produced, b) the limiting reactant, c) the excess reactant, d) the left over mass of your excess reactant e) the percent yield if 45.8 g H2SiF6 was produced in lab.
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?
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
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...