Nitrogen monoxide and oxygen react to form nitrogen dioxide.Consider the mixture of NO and O2 shown in the accompanyingdiagram. The blue spheres represent N, and the red onesrepresent O. (a) How many molecules of NO2 can be formed,assuming the reaction goes to completion? (b) What is the limitingreactant? (c) If the actual yield of the reaction was 75%instead of 100%, how many molecules of each kind would bepresent after the reaction was over?

Consider the haber-bosch process for the synthesis of ammonia from its elements. Calculate the theoretical yield in moles NH3 from the complete reaction of 15.6 grams H2 in the presence of excess N2 gas according to the following balanced chemical equation. N2(g) + 3H2(g) -> 2NH3(g)

How many grams of P2O5P2O5 are formed when 9.51 g 9.51 g  of phosphorus reacts with excess oxygen? Show the unit analysis used for the calculation by placing the correct components into the unit-factor slots.

Home-Grown Example: Calculation of Mass-Related Concentrations (a) A solution is made by dissolving 1.675 mg of sucrose (C₁2H22011) in 0.01091 g of water. What is the mass percentage of each component of the solution? (b) A 1762-kg sample of groundwater was found to contain 2.443 µg of Fe²+. What is the concentration of Fe²+ in parts per billion?

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In a reaction to produce NaF, 3.50 g of HF and 1.26 of Na2SiO3 are reacted according to the following: Na2SiO3 (s) + HF (aq) →H2SiF6 (aq) + NaF (aq) + H2O (l) (a) Balance the equation.   (b) Calculate the theoretical yield of NaF.   (c) If 0.792 g of NaF is formed, calculate the percent yield.

A chemist invents a new combustion analysis instrument that uses less O2(g) which saves money on each analysis. The improvement is that instead of CO2(g) being formed and trapped, CO(g) is formed and trapped. H2O (g) is also formed and trapped when substances that contain hydrogen are analyzed.(a) The chemist places 2.184 g of an unknown compound of carbon and hydrogen in the new analyzer. 4.627 g of CO (g) and 1.795 g of H2O (g) are produced. Find the empirical formula for the compound.(Molar masses (g/mol): CO = 28.0104, H2O = 18.015) (b) Despite the best efforts of the chemist, the molar mass of the compound cannot be determined (using this method). Clearly explain why this prevents the determination of the molecular formula

In an industrial process, hydrogen chloride, HCl, is prepared by burning hydrogen gas, H2, in anatmosphere of chlorine, Cl2. Write the chemical equation for the reaction. Below the equation, give themolecular molar and mass interpretations.

Glucose, C6H1206, can be represented by the molecular model shown below. If 1.00 mol of glucoseis submitted to combustion analysis, how many moles of CO2 and how many moles of H2O wouldbe formed?

balance the following equation