In image, 5 molecules of O2 and 8 molecules of NO are present.
According to the reaction,
1 molecule O2 require 2 molecules of NO
5 molecule of O2 require 10 molecules of NO
Since we have only 8 molecules of NO. Thus , NO is limiting reagent and O2 is in excess.
Third image represent the mixture after reaction completed because 1 molecule of O2 remain left.
Question 13 of 15 > O, reacts with NO to form NO, according to the following...
D Question 9 1 pts Nitrogen and hydrogen gas react to form ammonia (NH3) according to the reaction: N2 (s) +3 H2 (s)- 2 NH3 (s). If a flask contains a mixture of reactants as shown below Н2 which image best represents the mixture N2 in the flask after the reactants have reacted as completely as possible? NH3 Hа N2 (a) (b) (c) Which is the limiting reactant? NH3 На N2 (a) (b) (c) Which is the limiting reactant? Which...
1. Aluminum reacts with oxygen according to the following reaction: 4 Al(s) + 3 O2(g) -> 2 Al2O3 If 8.00 moles of oxygen are reacted with 8.00 moles of aluminum to completion, which is the excess reactant?
chemistry
limiting reactant
question 3 Nitrogen monoxide reacts with chlorine to form nitrosyl chloride according to the following Unbalanced reaction, Nog)+ Cl2(g) → Nocle) 1 If we start with 12.56 of nitrogen monoxide and 17,8 g of chlorine. how many grams of the excess reactant are leftover after the reaction is complete?
If 20 g of Na2SO4 is reacted with 20 g of Al(NO3)3 according to the following equation: 3 Na2SO4 + 2 Al(NO3)3 --> Al2(SO4)3 + 6 NaNO3 How many grams of the excess reactant will remain after the reaction, assuming that all of the limiting reactant reacts to form the products?
Question 3 of 3 > Ammonia, NH), reacts with oxygen to form nitrogen gas and water. 4NH, (aq) + 30,(E) — 2N,(s) + 6H20(1) If 3.45 g of NH, reacts with 5.18 g of O, and produces 0.450 L of N, at 295 K and 1.00 atm, which reactant is limiting? - NH (0) 0,(8) What is the percent yield of the reaction? percent yield: 29.14
H2 and O, react to form H,O according to the equation: 2H,(g)+02(8) 2H,0(8). If 2.00 g of hydrogen gas and 20.0 g of oxygen gas are placed in a 100.0 L container at 37.0°C, a) What is the total pressure of the mixture of gases at the end of the reaction? (hint identify your limiting reactant, identify the gases in the mixture at the end of the reaction) b) If the temperature was raised to 47°C, what would the new...
< Question 3 of 3 > Ammonia, NH, reacts with oxygen to form nitrogen gas and water. 4NH, (aq) + 30,(g) + 2N (8) + 6 H,0(1) If 2.45 g of NH, reacts with 3.68 g of O, and produces 0.850 L of N, at 295 K and 1.00 atm, which reactant is limiting? O NH3(aq) O 02(8) What is the percent yield of the reaction? percent yield: 55.7
15. (10 pts.) Hydrazine (N2H) is commonly used as rocket fuel. It reacts with oxygen according to the balanced chemical equation: N2H4(g) + 302(g) + 2N02(g) + 2H20(1) Compound Molecular Weight (g/mol) 70.5 g of Hydrazine (N2Ha) is reacted with 195.3 g of Oz to test | N₂H4 32.06 the thermodynamics of the reaction. 02 32.00 MAKE SURE TO SHOW ALL OF YOUR WORK 46.01 NO a. Identify the limiting reactant:
Cl2 + 3F2 → 2CIF: Chlorine reacts with fluorine to form gaseous chlorine trifluoride. You start with 500g of chlorine and 95.0g of fluorine. a) What is the limiting reagent? b) What is the theoretical yield of chlorine trifluoride in grams? c) How many grams of excess reactant remain un-reacted? 2C2H2 + 50, 400, + 2H2O Oxyacetylene torches used in welding and cutting steel reach temperatures near 2000'C. The reaction involved is the complete combustion of acetylene (CH2). Starting with...
Question 13 of 13 > A precipitation reaction occurs when 745 mL of 0.648 M Pb(NO), reacts with 459 mL of 0.851 M KI, as shown by the following equation. Pb(NO3)2(aq) + 2 Kl(aq) — Pl_(s) + 2 KNO, (aq) Identify the limiting reactant. OKI O KNO, Pb(NO) Pol, Calculate the theoretical yield of Pbl, from the reaction. mass of Pbl : on 13 O 15 Identify the limiting reactant. OKI O KNO, Pb(NO3)2 OPhl Calculate the theoretical yield of...