You are working in my lab. I ask you to make 0.250 L of H3PO4 (density is 1.651 g/cm³). I give you solid phosphorus triiodide with water. The other product will be hydrogen iodide gas. I tell you to use 45.0 % excess water and that the reaction will yield 75.0 % H3PO4. How much phosphorus triiodide should be weighed out?

You are working in my lab. I ask you to make 0.250 L of H3PO4 (density is 1.651 g/cm³). I give you solid phosphorus triiodide with water. The other product will be hydrogen iodide gas. I tell you to use 45.0 % excess water and that the reaction will yield 75.0 % H3PO4. How much phosphorus triiodide should be weighed out?

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

How many moles of Al are necessary to form 48.8 g of AlBr₃ from this reaction: 2 Al(s) + 3 Br₂(l) → 2 AlBr₃(s) ?
6
suppose a student reacts 1.57 g Ca with O2 gas. In his/her calculations however S/he mistakenly calculate the theoretical yield with 1.97 g Ca. Will the theoretical yield of CaO be too high, too low, or unaffected?
For the reaction N, + 3H, 2NH, what is the Mole ratio of nitrogen to hydrogen? t. Mole ratio of hydrogen to ammonia?
1.What mass of Cu(IO3)2 can be formed from 0.650 g of CuSO4 · 5H2O?2. What mass of KIO3 is needed to convert the copper in 0.2750 g of CuSO4 · 5H2O to Cu(IO3)2?
1 mole of PCI3 is isolated from the reaction of solid elemental phosphorus, P(s), with excess chlorine gas. Determine the moles of phosphorus required for this reaction if the yield is 25%.
Consider the Haber-Bosch process for the synthesis of ammonia from its elements. Calculate the theoretical yield in moles NH, from the complete reaction of 15.6 grams H, in the presence of excess N, gas according to the following balanced chemical equation: N,(g) + 3 H,(g) → 2 NH,(g)
Silicon tetrachloride (SICI4 ) can be prepared by heating Si in chlorine gas: Si(s) + 2C12(g) -> SiCl2(1) In one reaction, 0.507 mole of SiCI4 is produced. What mass (grams) of molecular chlorine were used in the reaction? Choose the nearest answer. MW SICI4 = 169.9 g/mol; MW CI = 35.453 g/mol (A) 36 grams (B) 72 grams 27 grams D) 63 grams
Potassium chlorate, potassium chloride, and water is produced by passing chlorine gas into a hot solution of potassium hydroxide. Calculate the volume in L of chlorine gas needed to produce 724.25 mL of 4.25 M potassium chlorate. The density of chlorine gas is 3.17 g/L. Atomic Mass: K: 39.098 g/mol Cl: 35.453 g/mol O: 15.999 g/mol H: 1.008 g/mol
First N2(g) + 3H2(g)—2NH3(g) second NH3(g) + 2O2(g)—HNO3(g) + H2O(g). Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and ox
A 235.2-g sample of ground water is analyzed for calcium. The Ca2+ in the sample is first precipitated and filtered-off as NH4CaPO4·7H2O. This precipitate is dried and heated, releasing water and ammonia to yield anhydrous calcium pyrophosphate (Ca2P2O7). The mass of Ca2P2O7 obtained is 0.0234 g.Give the calcium content of the ground water in parts per million (to three significant figures).
Consider the decomposition of aluminum sulfide into aluminum metal and solid S₈ (one of the forms of sulfur). You've determined the compound formed between aluminum and sulfur will be Al₂S₃. This compound decomposes to form solid aluminum and sulfur (as S₈). Write the balanced chemical equation for the reaction.