Water of Hydration Record the mass empty evaporating dish ( or crucible). Record the mass of dish before heating the hydrate 29.00g 31.11g Measure the mass of the dish and the anhydrous material here. 30.75g Determine the chemical formula of the original hydrate. Show your calculation here: Anhydrate: Cu3(PO4)2 Mass of anhydrate menm Moles of the anhydrate - Mass of water Moles of H20

Water of Hydration Record the mass empty evaporating dish ( or crucible). Record the mass of dish before heating the hydrate 29.00g 31.11g Measure the mass of the dish and the anhydrous material here. 30.75g Determine the chemical formula of the original hydrate. Show your calculation here: Anhydrate: Cu3(PO4)2 Mass of anhydrate menm Moles of the anhydrate - Mass of water Moles of H20

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter10: Gases And Their Properties

Section: Chapter Questions

Problem 25PS: A gaseous organofluorine compound has a density of 0.355 g/L at 17 C and 189 mm Hg. What is the...

See similar textbooks

Similar questions

/ext/map/index.html?_con%3Dcon&external_browser%3D08launchUrl%=https%253/ Chapter 6 HW # 2 Saved 3 attempts left Check my work Be sure to answer all parts. 1 A mercury mirror forms inside a test tube as a result of the thermal decomposition of mercury(II) points oxide: 2 HgO(s) →2 Hg(!) + O2(g) AH = 181.6 kJ References (a) How much heat is needed to decompose 513 g of the oxide? kJ (b) If 607 kJ of heat is absorbed, how many grams of Hg form? x 100 g Hg (Enter your answer in scientific notation.) Mc Graw Hill < Prev 3 of 15
There are 20 kg of exhaust gas formed per kg of fuel oil burned in the combustion of diesoline C16H32. What is the excess air percent.
WhalefossilsfoundintheSaharaDesertprovetheregionwasoncecoveredin water. Remnants of that water, called “fossil water,” still exist today in the Nubian Sandstone Aquifer System (NSAS). The NSAS is the world’s largest body of fossil water, containing an estimated 1.65 x 1014 tons. Given the density of water as 1.00 g/mL, what is the NSAS’s volume? Is the NSAS bigger or smaller than Lake Michigan (estimated at 5.0 x 1018 cm3)? (1 ton=2000 pounds exactly) (1 pound=0.454 kg)
CUSO4 (aq) + Zn(s) → Cu(s) + ZnSO4(aq) The single-replacement reaction above produces 140.0 g of copper and an unknown concentration of zinc sulfate. With excess CuS04, what mass of Zn was used? Molar mass of Cu: 63.55 g/mol Molar mass of Zn: 65.38 g/mol Answer: g of zinc (Use 4 sig figs)
04/22/ 2021 ot art e b NAME Kouri KulRu DATE SECTION POSTLABORATORY ASSIGNMENT 1. Calculate the theoretical percentage of water for the following hydrates. (a) manganese(II) monohydrate, MnSO4 • H2O (b) manganese(II) tetrahydrate, MNSO4 • 4H2O 2. An unknown hydrate, AC• XH»O, has a mass of 1 .00 g before heating, and 0.738 g atter heating. What is the experimental percentage of water in the hydrate? ombvl lo slmo noihesilla logataW If the anhydrous compound (AC) has a molar mass of 101 g/mol, what is the water of crystallization (X) and the formula for the hydrate (AC XH,O)?ouphut suf (snoilgo) ai sh Formula of hydrate AC H20 Water of crystallization
Silicon tetrachloride (SiC14 ) can be prepared by heating Si in chlorine gas: Si(s) + 2C12(g) -> SiClą(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 %3D g/mol; MW CI = 35.453 g/mol
O • + 88 www-awu.aleks.com ALEKS - Anniston Stovall Answered: Wine goes bad soon after opening... | bartleby O CHEMICAL REACTIONS Anniston Solving for a reactant using a chemical equation 2/5 Ammonia (NH,) chemically reacts with oxygen gas (0,) to produce nitric oxide (NO) and water (H,0). What mass of nitric oxide is produced by the reaction of 9.4 g of ammonia? Be sure your answer has the correct number of significant digits. olo x10 18 Ar Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
What volume (in mL) of 3.20 M HNO3(aq) needs to be added to excess Na,CO3(s) to generate 4.85 L CO2(g) at standard temperature and pressure (STP)? Provide your answer in decimal notation rounded to the appropriate number of significant figures.
3. 1986 B Three volatile compounds X, Y, and Z each contain element Q. The percent by weight of element Q in each compound was determined. Some of the data obtained are given below. Percent by Weight of Element Q Compound Molecular Weight 64.8% Y 73.0% 104. Z 59.3% 64.0 The vapor density of compound X at 27°C and 750. mm Hg was determined to be 3.53 grams per litre. Calculate the molecular weight of compound X. Determine the mass of element Q contained in 1.00 mole of each of the three compounds. Calculate the most probable value of the atomic weight of element Q. Compound Z contains carbon, hydrogen, and element Q. When 1.00 gram of compound Z is oxidized and all of the carbon and hydrogen are converted to oxides, 1.37 grams of CO, and 0.281 gram of water are produced. Determine the most probable molecular formula of compound Z. а. b. с. d.
Oxyacetylene torches rely on a precise mixture of fuel (C2H2(g)) to oxygen to optimize the welding process. CH,(g) + _0,(g) → _co,(g) + _H,0(g) Calculate the volume (in L) of 02(g) required to react completely with 15.3 L of acetylene. Assume both substances are at SATP. Hint: Balance the combustion reaction first. Do not show your work in the space provided. Record only your final answer with the correct number of significant digits and the proper units. Answer: |
A gaseous compound of phosphorus (P) and fluorine (F) was found to have a density of 3.50 g L' at a temperature of 25.0 °C and a pressurc of 740 tor. It was also found to consist of 35.2% P and 64.8% F in a volume of 1 L. Assume that the mass of the sample is 100.0 g. Determine a) (i) its empirical formula (ii) its molecular mass using its empirical formula stated in part (i) (iii) its molecular mass using ideal gas law (iv) its molecular formula. Explain why the molecular formula is same as empirical formula. Given that the molecular mass of P is 30.97 g mol'; the molecular mass of F is 19 g mol'; 1 atm = 760 torr
11. Calculate the mass of salt present in 1m³ of seawater with a density of 1,030 kgm-³. (a) 300.0 kg (b) 40.0 kg (c) 30.0 kg (d) 38.6 kg