A sample of 45.7 g of tetraphosphorous decoxide (P,O10) reacts with 79.1 g of water to produce phosphoric acid (H, PO,) according to the following balanced equation. P,O10 + 6 H,0 → 4 H,PO, Determine the limiting reactant for the reaction. O P,010 H,O O H, PO, Calculate the mass of H, PO, produced in the reaction. mass of H, PO: Calculate the percent yield of H, PO, if 35.0 g of H, PO, is isolated after carrying out the reaction. percent yield:

A sample of 45.7 g of tetraphosphorous decoxide (P,O10) reacts with 79.1 g of water to produce phosphoric acid (H, PO,) according to the following balanced equation. P,O10 + 6 H,0 → 4 H,PO, Determine the limiting reactant for the reaction. O P,010 H,O O H, PO, Calculate the mass of H, PO, produced in the reaction. mass of H, PO: Calculate the percent yield of H, PO, if 35.0 g of H, PO, is isolated after carrying out the reaction. percent yield:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

For the following reaction,23.1 grams of carbon disulfide are allowed to react with 89.2 grams ofchlorine gas .carbon disulfide(s) +chlorine(g) carbon tetrachloride(l) + sulfur dichloride(s)What is the maximum amount of carbon tetrachloride that can be formed? grams What is theFORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams
what mass of calcium hydroxide in grams is needed to produce 5.11 mol of water?
The Haber process is used to industrially produce ammonia ( NH3 ) . Ammonia is the active ingredient in a variety of household cleaners . The data table below summarizes the experimental quantities of reactants and products collected from a specific batch. If the company chemist calculated that 12,163 g of NH3 should be produced, what is the percent yield
When sodium azide is activated in an automobile airbag, nitrogen gas and sodium areproduced according to the equation2 NaN3(s) −→ 2 Na(s) + 3 N2(g). If 0.37 mol of NaN3 reacts, what mass ofnitrogen would result? Answer in units of g.
For the following reaction, 0.343 moles of sulfuric acid are mixed with 0.223 moles of calcium hydroxide. sulfuric acid (aq) + calcium hydroxide(s) → calcium sulfate(s) + water(l) What is the formula for the limiting reagent? Limiting reagent: What is the maximum amount of calcium sulfate that can be produced? Amount = moles
Aqueous hydrochloric acid HCl will react with solid sodium hydroxide NaOH to produce aqueous sodium chloride NaCl and liquid water H2O Suppose 1.82 g of hydrochloric acid is mixed with 3.7 g of sodium hydroxide. Calculate the maximum mass of water that could be produced by the chemical reaction.
Write and balance the chemical equation and then determine which reactant is the limiting reagent based on the amounts of reagents given. Finally, determine how much water is produced in grams 2.0moles of nitric acid reacts with 2.1 moles of aqueous sodium hydroxide
For the following reaction, 4.20 grams of chlorine gas are mixed with excess carbon disulfide. The reaction yields 1.98 grams of carbon tetrachloride. carbon disulfide (s) + chlorine (g) →carbon tetrachloride (1) + sulfur dichloride (s) What is the theoretical yield of carbon tetrachloride ? What is the percent yield of carbon tetrachloride ? grams %
Write a balanced chemical equation based on the following description: butane gas reacts with oxygen gas to produce carbon dioxide gas and water vapor C4H10(g)+O2(g)_
Be clear/specific/detailed
16.5 ML of 0.228 M NaOH what is required to neutralize 15 ML of an unknown H2SO4 Solution. What is the molarity of theH2SO4
For the following reaction, 37.3 grams of sulfuric acid are allowed to react with 42.5 grams of zinc hydroxide. sulfuric acid (aq) + zinc hydroxide(s) → zinc sulfate (aq) + water (1) What is the maximum amount of zinc sulfate that can be formed? Mass= What is the formula for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? Mass= g.