Consider the Harber-Basch process for the synthesis of ammonia from its elements. Calculate the theoretical yield in moles NH3 from the complete reaction of 59.8 grams N2 in the presence of excess H2 gas according to the following balanced equation N2(g)+3H2(g)->2NH3(g)

How many moles of NO₂ would be required to produce 3.01 moles of HNO₃ in the presence of excess water in the following chemical reaction? 3 NO₂(g) + H₂O (l) → 2 HNO₃(g) + NO(g)

An alloy of a metal containing Al, Cu and Ge is to be produced as follows: 10g of Cu is mixed with 100 cm3 of Al. How many grams of Ge must be added to achieve 0.2 atom percent of Ge in the alloy?

What is the maximum amount (in grams) of sulfur dioxide that can be produced by the reaction of 440 g of dihydrogen sulfide with 1860 g of oxygen according to the balanced equation below?2 H2S(g) + 3 O2(g) → 2 H2O(g) + 2 SO2(g)

How many moles of HNO₃ will be produced from the reaction of 33.5 g of NO₂ with excess water in the following chemical reaction? 3 NO₂(g) + H₂O (l) → 2 HNO₃(g) + NO(g)

Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients, Ca, (PO),(s) + SiO₂ (s) + C(s) + CaSiO₂ (s) + P (s) + CO(g) X x 5 Ś ?

If MgCl2·H2O is the limiting reagent with a mole amount of 0.00189 mole. What is the theoretical yield of Mg(OH)2 (58.319 g mol-1) precipitate which will be formed?

5a) Calculate the mass, in grams, of the product produced when 10.0 g of aluminum reacts with 10.0 g of oxygen. b) What was the percent yield from this reaction if 7.80g of product were produced. c) Calculate the mass of the excess reagent that is remains unused.

Chlorine gas can be produced in the laboratory by adding concentrated hydrochloric acid, HCl, to manganese(IV) oxide according to the following reaction: MnO2 (s)   +   4 HCl (aq)   →   MnCl2 (aq)   +   2 H2O (l)   +   Cl2 (g) What mass of MnO2 is required to produce 48.4 g Cl2 by the following reaction? Be sure to enter a unit with your answer.

What mass of Silver Chromate is produced Silver nitrate ? from 4.65 mol 2 AgNO3 + Na₂ CrO4 → Ag₂ Cr Oy + 2NaNO3 Of