1. Moles of H2O = mass / molar mass = 25 / 18 = 1.39 moles
Moles of NO2 = mass / molar mass = 25 / 46 = 0.544 moles
We see that NO2 is the limiting reagent
Moles of HNO3 = moles of NO2 * 2 /3 = 0.544 * 2 / 3 = 0.363 moles
Mass = moles * molar mass = 0.363 * 159 = 57.72 g
2. Moles of ethanol = mass / molar mass = 25 / 46 = 0.544 moles
Moles of O2 = mass / molar mass = 25 / 32 = 0.781 moles
We se that O2 is the limiting reagent
Moles of CO2 = moles of ethanol * 2 = 0.544 * 2 = 1.09 moles
Mass of CO2 = moles * molar mass = 47.96 g
Part E Determine the limiting reactant, given 250 g of each reactant, in the following: 3NO2(g)...
i just need the answer . thank Part E Instructors View all hidden pane Determine the limiting reactant, given 25.0 g of each reactant, in the follow ANSWER: 3NO2(g) + H2O(1) + 2HNO3(aq) + NO(g) HNO3 Ο NO HO NO2 Part F Calculate the grams of HNO3 that would be produced. Express your answer with the appropriate units. ANSWER: m(HNO3) = Part G Determine the limiting reactant, given 25.0 g of each reactant, in the following: CyH60(1) + 302 (8)...
Part 6 Determine the limiting reactant aivan 250 g of each reactant in the following C,H(1) + 302(g) 2002(g) + 3H20() ANSWER: CO2 CHO H2O 02 Part 1 Calculate the grams of CO, that would be produced. Express your answer with the appropriate units. ANSWER: m(CO2) =
29.0 g Part E Determine the limiting reactant. CH, OH(1) + 302(g) +2C02(g) + 3H2O(g) Express your answer as a chemical formula. 02 Submit Previous Answers ✓ Correct Part F Calculate the grams of product in parentheses that would be produced. (H2O) Express your answer with the appropriate units. ? THE Å Value 0 a Units m(H,0) = Type here to search O E A
For each of the following reactions, 15.0 g of each reactant is present initially. A. 4Al(s)+3O2(g)→2Al2O3(s) Calculate the grams of product in parentheses that would be produced. (Al2O3) Express your answer with the appropriate units. B. 3NO2(g)+H2O(l)→2HNO3(aq)+NO(g) Calculate the grams of product in parentheses that would be produced. (NO) Express your answer with the appropriate units. C. C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g) Calculate the grams of product in parentheses that would be produced. (CO2) Express your answer with the appropriate units.
Part B How many moles of CO are produced when 2.2 moles C reacts? ication Express your answer using two significant figures. к" ANSWER pr moles Part C How many moles of SO2 are required to produce 0.55 mole CS2? Express your answer using two significant figures. ANSWER moles Part D How many moles of CS2 are produced when 3.0 moles C reacts? Express your answer using two significant figures. ANSWER moles Problem 7.76 - Enhanced - with Feedback You...
for each of the following reaction 29.0 g of reactant Part B Calculate the grams of product in parentheses that would be produced. (C1,03) Express your answer with the appropriate units. °H MAR 0 2 ? m(Cr2O3) = 92 cra Submit Previous Answers Request Answer X Incorrect; Try Again; 2 attempts remaining For each of the following reactions, 29.0 g of each reactant is present initially. Part A Determine the limiting reactant 4Cr(s) + 302(g) +2Cr2O3(s) Express your answer as...
Problem 7.77 ® 13 of 20 ~ For each of the following reactions, 15.0 g of each reactant is present initially. Part A Determine the limiting reactant. 2Al(s) + 3Cl2(g)+2AlCl3 (s) Express your answer as a chemical formula. = A ¢ A o 2 ? Submit Request Answer Part B Calculate the grams of product in parentheses that would be produced. (AIC13) Express your answer with the appropriate units. MÅ A 0 2 ? m(AlCl3 ) = Value Units Submit...
For each of the following reactions, 32.0 g of each reactant is present initially. A. 1. Determine the limiting reactant. 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) 2. Calculate the grams of product in parentheses that would be produced. (H2O) B. For each of the following reactions, 32.0 g of each reactant is present initially. 1. Determine the limiting reactant. CS2(g)+3O2(g)→CO2(g)+2SO2(g) 2. Calculate the grams of product in parentheses that would be produced. (CO2)
For 3NO2(g)+H2O(l)→2HNO3(aq)+NO(g), the first part of the question asks me to find the mass of HNO3 made from 293 g of NO2 (found to be 267.55). How do i find the volume of NO gas formed in the reaction with those 293 grams? Air temp is 284.5K and pressure is 714/760atm
background info: So I have the balanced equation = 2C8H18(g)+25O2(g)→16CO2(g)+18H2O(g) and oxygen is the limiting reactant of 0.180 mol of octane is allowed to react with 0.880 mol of oxygen. Part C How many moles of water are produced in this reaction? Express your answer with the appropriate units. View Available Hint(s) : HÅR O 2 ? H2O produced = H,0 produced = Value Units Submit Part D After the reaction, how much octane is left? Express your answer with...