Question 1: Toluene (C7H8) and nitric acid (HNO3) are used in the production of trinitrotoluene (TNT, C7H5N3O6), an explosive. C7H8 + HNO3 => C7H5N3O6 + H2O (not balanced) (a) what mass in grams of nitric acid is required to react with 454 g C7H8 (b) what mass in grams of TNT can be made from 829 g C7H8 ?
Question 1: Toluene (C7H8) and nitric acid (HNO3) are used in the production of trinitrotoluene (TNT,...
Review Part A What mass in grams of nitric acid is required to react with 712 g CHE? Express your answer with the appropriate units. mass of nitric acid = Value Units Submit Request Answer Part B What mass in grams of TNT can be made from 777 g C H? P Pearson tion Inc. All rights reserved. Terms of Use | Privacy Policy | Permissions
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming of natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia:N2(g)+3H2(g)→2NH3(g)In the second step, ammonia and oxygen react to form nitric acid and water:NH3(g)+2O2(g)→HNO3(g)+H2O(g)Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced.
How many grams of nitric acid, HNO3, are required to neutralize (i.e. completely react with) 3.33 moles of Ca(OH)2 according to the balanced chemical reaction: 2HNO3 + Ca(OH)2 --> 2H2O + Ca(NO3)2
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: NH3(g)+?O2(g)→?NO(g)+?H2O(g) What volume of O2 at 722 mmHg and 27 ∘C is required to synthesize 17.5 mol of NO?
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH3(g)+?O2(g)→?NO(g)+?H2O(g) What volume of O2 at 798 mmHg and 41 ∘C is required to synthesize 12.5 mol of NO? Express your answer to three significant figures and include the appropriate units.
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH3(g)+?O2(g)→?NO(g)+?H2O(g) Part A What volume of O2 at 684 mmHg and 41 ∘C is required to synthesize 19.0 mol of NO? Express your answer to three significant figures and include the appropriate units. volume of O^2=
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH3(g)+?O2(g)→?NO(g)+?H2O(g) What volume of O2 at 912 mmHg and 41 ∘C∘C is required to synthesize 24.5 mol of NO? 750 mmHg = 1 bar R = 0.08314 L bar mol-1 K-1 Express your answer numerically in litres.
6. Calcium oxide reacts with nitric acid to produce calcium nitrate and water. How many grams of calcium oxide are required for complete reaction with 30.0 mL of 0.587 M nitric acid? The molar mass of calcium oxide is 56.077 g/mol. (Hint: start by writing the balanced equation for the reaction.) 7. A sample contains an unknown amount of succinic acid, H2CHO. If 0.3540 g of the sample requires 42.70 mL of 0.1000 M NaOH to neutralize the H2C,H404 completely,...
Copper reacts with nitric acid via the following equation: 3 Cu(s) + 8 HNO3(aq) → 3 Cu(NO3)2(aq) + 2 NO(g) + 4 H2O(ℓ) What mass of NO(g) can be formed when 20.7 g of Cu reacts with 50.0 g HNO3? g NO
Problem 1 - Strontium Hydroxide Acid/Base Question -/1 points A 8.51 mL sample of nitric acid required 13.25 mL of 0.105 M strontium hydroxide for titration. Calculate the molarity of the acid solution. (Hint: It's stoichiometry, you need the balanced equation) Concentration of Nitric Acid M Evaluate Problem 3 - H2Z Molecular Weight -/1 points A solution was made by adding water to 0.22 g of H2Z until the volume totaled 25.00 mL. Subsequent titration required 40.50 mL of 0.11...