When nitrogen dioxide from car exhaust combines with water in the air, it forms nitric acid...
When nitrogen dioxide from car exhaust combines with water in the air, it forms nitric acid (HNO3) which causes acid rain and nitrogen monoxide. a.Write a balanced chemical equation for the reaction above. b.How many moles of each product are produced from 0.250 moles of water? c.How many grams of nitrogen dioxide are needed to form 75.0 g of nitric acid?
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When nitrogen dioxide from car exhaust combines with water in
the air, it forms nitric acid...
When nitrogen dioxide (NO2) from car exhaust combines with water in the air, it forms nitric...
When nitrogen dioxide (NO2) from car exhaust combines with water in the air, it forms nitric acid (HNO3), which causes acid rain, and nitrogen oxide. 3NO2(g)+H2O(l)→2HNO3(aq)+NO(g) A. How many moles of HNO3 are produced from 0.196 mole of H2O? B.How many moles of NO are produced from 0.196 mole of H2O? C.How many grams of HNO3 are produced when 90.5 g of NO2 completely reacts? D.How many grams of NO2 are needed to form 64.5 g of HNO3? Gasohol is...
NewOVI 10. When nitrogen dioxide (NO2) gas from car exhaust combines with water vapor in the...
NewOVI 10. When nitrogen dioxide (NO2) gas from car exhaust combines with water vapor in the air, it forms aqueous nitric acid (HNO3), which causes acid rain, and nitrogen oxide gas. a. Write the balanced chemical equation. b. How many moles of each product are produced from 0.250 mole of H20?! C. How many grams of HNO3 are produced when 60.0 g of NO2 completely reacts? d. How many grams of NO2 are needed to form 75.0 g of HNO3?
Acid rain results from the reaction of nitrogen dioxide with water in the air. Unbalanced equation:...
Acid rain results from the reaction of nitrogen dioxide with water in the air. Unbalanced equation: NO2(g) + H2O(l) --> HNO3(aq) + NO(g) A water spray is sometimes used in exhaust stacks at coal fired power plants to help prevent acid rain. Given the following parameters, calculate the concentration of the nitric acid in 8L of wastewater (assume no evaporation ... I know this is not reality but let's make the calculation a bit easier!). 1000L/min vented through the exhaust...
Calculating an equilibrium constant from a heterogeneou... Nitrogen dioxide and water react to form nitric acid...
Calculating an equilibrium constant from a heterogeneou... Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO2(9)+H2O(1)-2 HNO3(aq)+NO(9) At a certain temperature, a chemist finds that a 9.3 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO 24.18 HO 247.2 g HNO, 7.4 g NO 17.6 Calculate the value of the equilibrium constant for this reaction. Round your answer...
Nitrogen dioxide (NO) gas and liquid water (H20) react to form aqueous nitric acid (HNO3) and...
Nitrogen dioxide (NO) gas and liquid water (H20) react to form aqueous nitric acid (HNO3) and nitrogen monoxide (NO) gas. Suppose you have 2.0 mol of NO, and 7.0 mol of H2O in a reactor. What would be the limiting reactant? Enter its chemical formula below.
Concentrated nitric acid (HNO3) can oxidise elemental sulfur (S) to give sulfur dioxide, nitrogen dioxide and...
Concentrated nitric acid (HNO3) can oxidise elemental sulfur (S) to give sulfur dioxide, nitrogen dioxide and water, write a balanced chemical equation for this process.
Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation:...
Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3NO2(g)+H2O(l)→2HNO3(l)+NO(g) Part A Suppose that 4.8 mol NO2 and 1.0 mol H2O combine and react completely. Which reactant is in excess? Part B How many moles of the reactant in excess are present after the reaction has completed?
Chemistry limiting reactant how many of grams? Chemistry Q1 Nitrogen occording dioxide to the reacts with...
Chemistry
limiting reactant
how many of grams?
Chemistry Q1 Nitrogen occording dioxide to the reacts with water to form nitric acid and nitrogen monoxide following unbalanced reaction: NO₂ g) + H₂O 4 HNO3 cag) + No (g) If we start with 11.69 of nitrogen dioxide and 25.8 g of water, how many groms of the excess reactant are leftover after the reaction is complete?
9. Nitrogen dioxide (NO2) can react with water to form aqueous nitric acid according to the...
9. Nitrogen dioxide (NO2) can react with water to form aqueous nitric acid according to the following reaction. This is one way that acid rain forms in the atmosphere. Also listed are the standard free energies of formation for the species involved in the reaction. 3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) Compound AG, (kJ/mol) NO2(g) 51.3 H2O(0) -237.1 HNO3(aq) -110.9 NO(g) 87.6 a. Calculate AGºrx (6 points) b. Is the reaction spontaneous at standard conditions? Circle one and explain...
Aqueous glucose (C6H12O6) combines with oxygen gas during metabolism, producing carbon dioxide gas and liquid water....
Aqueous glucose (C6H12O6) combines with oxygen gas during metabolism, producing carbon dioxide gas and liquid water. A. Write a balanced chemical equation (including physical states) for the reaction described above. B. If 0.125 moles of glucose are metabolized, how many moles of carbon dioxide are formed? C. If 0.125 moles of glucose are metabolized, how many moles of water are formed? Zinc reacts with aqueous sulfuric acid, in a single displacement reaction. 1. Write a balanced chemical equation (including physical...
NewOVI 10. When nitrogen dioxide (NO2) gas from car exhaust combines with water vapor in the air, it forms aqueous nitric acid (HNO3), which causes acid rain, and nitrogen oxide gas. a. Write the balanced chemical equation. b. How many moles of each product are produced from 0.250 mole of H20?! C. How many grams of HNO3 are produced when 60.0 g of NO2 completely reacts? d. How many grams of NO2 are needed to form 75.0 g of HNO3?
Calculating an equilibrium constant from a heterogeneou... Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO2(9)+H2O(1)-2 HNO3(aq)+NO(9) At a certain temperature, a chemist finds that a 9.3 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO 24.18 HO 247.2 g HNO, 7.4 g NO 17.6 Calculate the value of the equilibrium constant for this reaction. Round your answer...
Nitrogen dioxide (NO) gas and liquid water (H20) react to form aqueous nitric acid (HNO3) and nitrogen monoxide (NO) gas. Suppose you have 2.0 mol of NO, and 7.0 mol of H2O in a reactor. What would be the limiting reactant? Enter its chemical formula below.
Chemistry
limiting reactant
how many of grams?
Chemistry Q1 Nitrogen occording dioxide to the reacts with water to form nitric acid and nitrogen monoxide following unbalanced reaction: NO₂ g) + H₂O 4 HNO3 cag) + No (g) If we start with 11.69 of nitrogen dioxide and 25.8 g of water, how many groms of the excess reactant are leftover after the reaction is complete?
9. Nitrogen dioxide (NO2) can react with water to form aqueous nitric acid according to the following reaction. This is one way that acid rain forms in the atmosphere. Also listed are the standard free energies of formation for the species involved in the reaction. 3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) Compound AG, (kJ/mol) NO2(g) 51.3 H2O(0) -237.1 HNO3(aq) -110.9 NO(g) 87.6 a. Calculate AGºrx (6 points) b. Is the reaction spontaneous at standard conditions? Circle one and explain...
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