Silicon tetrachloride (SİCI4 ) can be prepared by heating Si in chlorine gas: Si(s) + 2CI2(g) -> SİCI,(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 27 grams 63 grams D) 72 grams

Silicon tetrachloride (SİCI4 ) can be prepared by heating Si in chlorine gas: Si(s) + 2CI2(g) -> SİCI,(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 27 grams 63 grams D) 72 grams

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...

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Silicon tetrachloride (siCI4 ) can be prepared by heating Si in chlorine gas: Si(s) + 2C12(8) -> SİCI4() 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 Cl = 35.453 g/mol (A) 36 grams B 72 grams (c) 27 grams D) 63 grams
Phosphoric acid, a mild acid used among other things as a rust inhibitor, food additive, and etching agent for cavity repair by dentists, can be made from elemental phosphorus in a two step process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P4(s) + 5O2(g) -> 2P2O5(g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid H3PO4: P2O5(g) + 3H2O(l) -> 2H3PO4(l) Suppose the yield of the first step is 69.% and the yield of the second step is 82.%. Calculate the mass of phosphorus required to make 1.0kg of phosphoric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
A compound has the composition: carbon 37.21%; hydrogen 7.83%; and chlorine 54.96%. If its MW is 385 g/mol, determine (a) the empirical formula (b) the molecular formula.
Silicon tetrachloride (SiCl4 ) can be prepared by heating Si in chlorine gas: Si(s) + 2Cl2(g) -> SiCl4(l) In one reaction, 0.507 mole of SiCl4 is produced. What mass (grams) of molecular chlorine were used in the reaction? Choose the nearest answer. MW SiCl4 = 169.9 g/mol; MW Cl = 35.453 g/mol 63 grams 27 grams 72 grams 36 grams
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4) Zinc oxide can be produced by the following reaction: 2 Zn (s) + O2(g) 2 ZnO (s) - There are many uses for ZnO, but one is a heat- reflective coating on windows (thus lowering cooling demands in hot climates). This coating requires a thin layer (approximately 40-50 µm thick) of zinc oxide. Assume that this thin film uses 1.9x1020 Zn atoms per cm² of surface. How many grams of ZnO are added to a window that has an area of 5500 cm²? g Zno
6. Consider the following chemical reaction: 2 Cr(OH)3(aq) >Cr₂O3(s) + 3H₂0(1) 12.00 moles of chromium (III) hydroxide is decomposed. Calculate moles of the water produced. O 18.00 moles O 1.500 moles O 4.00 moles O 12.00 moles
Name: 14. The following reaction occurs and 9.81 x 1025 CO, molecules are produced. C6H12O6 (s) + O₂(g) → CO₂(g) + H₂O(1) How many kilograms of O₂ is required? © 2021 F'21/S'22 NetID: Chemistry I A: 5.21 WORKSH 83
Q 3 Hydrogen cyanide, HCN, is prepared from ammonia, air, and natural gas (CH4) by the following process: Pt 2NH3(g) + 302(8) + 2CH4(g) 2HCN(g) + 6H20(g) -> Hydrogen cyanide is used to prepare sodium cyanide, which is used in part to obtain gold from gold-containing rock. If a reaction vessel contains 11.5 g NH3, 12.0 g 02, and 10.5 g CH4, what is the maximum mass in grams of hydrogen cyanide that could be made, assuming the reaction goes to completion as written?
Ammonia (NH3) is an important compountd is used in large amounts for the manufacture of nitrogenous fertilizers, nylon and many other important compounds. It is manufactured by the catalytic reaction between nitrogen between nitrogen and hydrogen, according to the following equation; N2(g) +H2(g) = NH;(g) When 1.20 mol nitrogen and 1.20 mol hydrogen are mixed together in a closed vessel, 30% of the nitrogen is converted into ammonia. a. Calculate the moles of nitrogen gas that will be present in the vessel? (only 3 decimal places) mol b. Calculate the moles of hydrogen gas that will be present in the vessel? (only 3 decimal places) mol c. Calculate the moles of ammonia gas that will be present in the vessel? (only 3 decimal places) Activate W mol d. What is the number of moles of nitrogen gas that has reacted? (only 3 decimal places) 10:09 Links 18°C 1O 23-Nov-21
4. A common experiment at Science Fairs is the demonstration of a volcano using a mixture of baking soda, NaHCO3(s), and vinegar, CH₂COOH(aq), with the reaction: NaHCO3(s) + CH3COOH(aq)- CO2(g) + H₂O(l) + Nat(aq) + CH3COO(aq) where the heavier CO2 gas displaces the liquid mixture to the top of the container to simulate lava overflowing. If the volume of the reaction vessel is 0.500 L and the pressure is 0.997 atm and 298 K. given 50.5 ml of 0.351 M CH3COOH() in water, what mass of NaHCO3(s) is required to fill the bottle with CO2 gas?
Calcium hydride reacts with water to produce hydrogen gas according to the following reaction: CaH2(s) + 2 H2O(l) ----> 2H2(g) + Ca(OH)2(aq) This reaction is used to generate hydrogen gas to inflate air bags in cars and life rafts on boats and for similar uses where a simple compact means of hydrogen generation is necessary. Assuming complete reaction with water, how many grams of calcium hydride are required to fill a raft to a total pressure of 2.0 atm at 25oC if the volume of the raft is 1,000 L?