First, capitalization matters in chemistry.
The proper formula for nitrogen monoxide (nitric oxide) is NO. No is the symbol for the element nobelium.
The balanced equation is 2NO + O2 --> 2NO2
To determine the mass of NO2 formed when NO reacts with O2, we need to write and balance the chemical equation for the reaction. The balanced equation is 2NO + O2 -> 2NO2. From the equation, we see that 2 moles of NO will react with 1 mole of O2 to produce 2 moles of NO2. Next, we need to calculate the number of moles of O2 present in 384g using its molar mass. Finally, we can use the mole ratio from the balanced equation to find the mass of NO2 formed.
To determine the grams of oxygen needed to produce 4.50 moles of NO2, use the coefficients in the balanced equation. In this case, 7 moles of O2 are required to produce 4 moles of NO2. Calculate: (4.50 moles of NO2) * (7 moles of O2 / 4 moles of NO2) = 7.88 moles of O2. Finally, convert moles to grams using the molar mass of O2 (32.00 g/mol): 7.88 moles * 32.00 g/mol = 252.16 grams of O2.
The chemical equation provided is unbalanced. To balance the equation, you would need to ensure that the number of each type of atom is the same on both sides of the equation. Once balanced, the equation will show the reactants C7H10NO2 (organic compound) reacting with O2 to produce CO2, H2O, and NO2.
1/2 N2(g) + O2(g) + 33.1 kJ NO2(g)
The balanced equation for this reaction is: 2NO(g) + O2(g) ⇌ 2NO2(g) At equilibrium, the equilibrium constant, Kc, would be equal to [NO2]^2 / ([NO]^2 * [O2]).
The balanced equation for the reaction between nitrogen (N2) and oxygen (O2) to form nitrogen dioxide (NO2) is: 2N2 + 4O2 -> 4NO2
This reaction is:S + 6 HNO3 = H2SO4 + 2 H2O + 6 NO2
Balanced Equation: 2Mg(NO3)2 = 2MgO + 4NO2 + O2
The reactions are:N2 + O2 = 2 NO2 NO + O2 = 2 NO2
To determine the mass of NO2 formed when NO reacts with O2, we need to write and balance the chemical equation for the reaction. The balanced equation is 2NO + O2 -> 2NO2. From the equation, we see that 2 moles of NO will react with 1 mole of O2 to produce 2 moles of NO2. Next, we need to calculate the number of moles of O2 present in 384g using its molar mass. Finally, we can use the mole ratio from the balanced equation to find the mass of NO2 formed.
To determine the grams of oxygen needed to produce 4.50 moles of NO2, use the coefficients in the balanced equation. In this case, 7 moles of O2 are required to produce 4 moles of NO2. Calculate: (4.50 moles of NO2) * (7 moles of O2 / 4 moles of NO2) = 7.88 moles of O2. Finally, convert moles to grams using the molar mass of O2 (32.00 g/mol): 7.88 moles * 32.00 g/mol = 252.16 grams of O2.
C3h8 + 5o2 --> 3co2 + 4h2o
2h2 + o2 -> 2h2o stupid wiki is not allowing capitalization again!! Know that all the letters are capitals.
This equation is not balanced as given. To balance it, you need to change the coefficients of the reactants and products. The balanced equation is 4Al + 3O2 -> 2Al2O3.
The product of N plus O2 to form NO2 is a chemical reaction where nitrogen and oxygen gas combine to form nitrogen dioxide gas. This reaction occurs when nitrogen and oxygen molecules react under specific conditions to produce the NO2 molecule.
NO. There is no chlorine on the reactant side, so it cannot be balanced.
First, balance the equation: 2NO + O2 -> 2NO2 Calculate the molar mass of NO2 using the periodic table. Calculate the number of moles of NO involved using the given mass. Use the stoichiometry of the balanced equation to find the theoretical yield of NO2 in grams.