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)
Based on the following chemical equation: 4HCN + 5O2 -> 2N2 + 4CO2 + 2H2O Identify...
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...
For the following reaction: 4HCN(l)+5O2(g)⟶2H2O(g)+4CO2(g)+2N2(g) What is the change in free energy in kJmol? The relevant standard free energies of formation are: ΔG∘f,HCN=120.1kJmolΔG∘f,O2=0kJmolΔG∘f,H2O=-228.4kJmolΔG∘f,CO2=-394.6kJmolΔG∘f,N2=0kJmol Your answer should includ
for problems 3-6, refer to the following balanced equation: 2C2H2(g) + 5O2(g) + 4CO2(g) + 2H2O(0) 3. How many moles of CO2 are produced when 18 moles of O2 reacts? 4. How many grams of water (H20) are produced from 8.4 moles of CH2?! 5. How many grams of O2 react with 7.32 g of CzHz? During an experiment, 5.19 g of oxygen (O2) reacted with excess C2Hz to produce 4.38 g of CO2. Determine the percent yield of CO2...
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?
N2(g)3H2(g)2NH3(g) Answer Consider the following balanced chemical equation 4KO2(s)2H20(I)302(8) +4KOH(s) Determine the mass (in g) of (a) KOH formed if 10.0 g of KO2 reacts with 10.0 g of H2O. Identify the limiting reactant. Determine the mass (in g) of KOH formed when 20.0 g of (b) KO2 reacts with 10.0 g of H20. Identify the limiting reactant. Determine the mass (in g) of (c) O2 formed when 25.0 g of KO2 reacts with 5.00 g of H20. Identify the...
Consider this balanced chemical equation: Ca + 2H2O -> Ca(OH)2 + H2 The limiting reactant when 3.00 moles of calcium are reacted with 8.00 moles of water in the above equation is ____________________. If you carried out the above reaction with these molar amounts, what will be the theoretical yield of hydrogen gas. _______________________g. A student carried out the reaction above and collected 2.15 g of hydrogen gas product. What is the % yield for the reaction? _______________________. (3...
Use the set of three reactions shown below to answer the questions that follow. 2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ 2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJ N2(g) + O2(g) → 2NO(g) ΔH = +183 kJ If 27.9 g of NO g is reacted with excess oxygen, how much heat energy is produced? What mass of liquid water will be consumed during the production of 33900 J of energy assuming that there is...
The combustion of propane can be represented by the following equation: __ C3H8 (g) + __O2(g) → __CO2(g) + __H2O(g) Balance the equation and answer the next three questions. If 257. g of C3H8 and 951. g O2 react, which reactant is used up first? (enter propane or oxygen) What is the mass of carbon dioxide produced? (Give your answer to 3 sig figs.) What is the mass of water produced?(Give your answer to 3 sig figs.) grams
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.
1. Moles of Reactant to Mass of Reactant: Identify the iodide ions and ozone in the balanced chemical equation. Use mole ratio, then convert to grams. A method used by the EPA for determining the ozone concentration in the air is to pass an air sample through a bubbler containing iodide ions. The iodide ions remove the ozone according to the following reaction: O3(g) + 2 I-(aq) + H2O(l) → O2(g) + I2(aq) + 2 OH-(aq) How many grams of ozone...