Fill in the blanks to complete the balanced formation reaction for the following compound: Notes for filling blanks: • Enter one reactant per blank, in alphabetical order of the element symbols (such as C, CI, H N, O, etc.) • Include stoichiometric coefficients with no space before the element (such as "2N2 (g)"); coefficients of "1" may be omitted; fractional coefficients may be written in parentheses or as decimal values (such as "(1/2)N2 (g)" or "0.5N2 (g)") • Include subscript numbers as standard text (such as "N2 (g)") • Phases must be included, with a space between the element and phase (such as "N2 (g)") • Incorrect capitalization of elements will be marked as incorrect Formation reaction of NiCl₂ (s) (nickel chloride): - NiCl₂ (s)

Fill in the blanks to complete the balanced formation reaction for the following compound: Notes for filling blanks: • Enter one reactant per blank, in alphabetical order of the element symbols (such as C, CI, H N, O, etc.) • Include stoichiometric coefficients with no space before the element (such as "2N2 (g)"); coefficients of "1" may be omitted; fractional coefficients may be written in parentheses or as decimal values (such as "(1/2)N2 (g)" or "0.5N2 (g)") • Include subscript numbers as standard text (such as "N2 (g)") • Phases must be included, with a space between the element and phase (such as "N2 (g)") • Incorrect capitalization of elements will be marked as incorrect Formation reaction of NiCl₂ (s) (nickel chloride): - NiCl₂ (s)

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

need help with this chemistry
6
Tristearin C 57H 11006), obtained from animal fats, was historically used as a household fuel source. The burning of tristearin is depicted as: 0,+0,−CO,+H,0 2 CH 57 110 6 2 When 5.79 kg of tristearin and pure oxygen gas at 9.30% excess were reacted, 11.29 kg of CO2 is recovered. Determine the percent yield of CO2. Type your answer as a percent, 2 decimal places.
E-85 is an alternative fuel for automobiles and light trucks that consists of 85.0% (by volume) ethanol (C2H5OH), and 15.0% gasoline. When ethanol burns completely it produces CO2 and H2O. The balanced equation for the burning of ethanol isC2H5OH+3O2-->2CO2+3H2OThe density of ethanol is 0.790 g/mL. How many moles of carbon dioxide are produced by the complete combustion of the quantity of ethanol in 8.00 gallons of E-85 fuel? _mol CO2
T Ma M PA USN Be * Ma E Ad G ph ph Do E Un O Ac. 6 Pec O Na O Pe Со Bas 3 Pe Stu "app.101edu.co Question 11 of 11 What is the mass in grams of H2 that can be formed from 55.8 grams of NH3 in the following reaction? 2 NH:(g) → 3 H:(g) + N:(g)
7:25 ◄ Search 2- 3c₂²- 1 + Write a balanced chemical equation based on the following description: solid barium carbonate decomposes into solid barium oxide and carbon dioxide gas when heated BaCO3 (s) (s) Be O Question 5 of 20 Reset 2 3 4 5 6 7 8 B (1) Ox Ba Cb (g) C 个 Br Tap here or pull up for additional resources 5G 85 Ca Submit 9 11 (aq) O Cr • x H₂O
Jj.70.
3. Balance the formula equations
00 %24 4+ dl w/ S' Enter your answer in the provided box. Using the balanced equation for the combustion of ethanol, answer the following question. C2H,O(1) + 3 02(g) – 2 CO2(g) + 3 H,0 (g) ethanol How many grams of H,0 are formed from 1.2 mol of ethanol? OH 8 #3 5. 9. 2 4 0O
Enter the coefficients directly from the balanced chemical equation. Do not reduce to lowest terms. For example: If 3 moles H2 react with 3 moles O2, enter "3" for each, not "1". According to the following reaction: СО (g) + H20 (1) — СО, (g) + Hz (g) What would you multiply "grams of carbon monoxide" by to convert to the units "moles of water" ? (number) (unit) (number) (unit) grams CO = moles H20 (number) (unit) (number) (unit)
Nitrogen monoxide reacts with oxygen according to the following reaction: 2NO(g) + O2 (g) ---> 2NO2 (g) If 10 moles of nitrogen monoxide are combined with 4 moles of oxygen, how many moles of NO2 should form?
ookmarks Profiles Tab Window Help G molar r ste X Learnir O Checko R Search M Ryerso E Ryerso Jassignments/389/tasks/103 The Haber-Bosch process involves the combination of nitrogen and hydrogen at high temperatures in the presence of a catalyst to produce ammonia. It is currently the main industrial source of ammonia. N2 (g) + 3 H2 (g) 2 NH3 (g) Assuming that a reaction vessel originally contains 0.400 moles of N, and 0.900 moles of H2 , answer each of the following questions: a) How many moles of NH3 could be produced from these quantities of N, and H2 ? mol NH3 0.600 b) After the reaction is complete, how many moles of N2 would remain? mol N2 0.100 c) After the reaction is complete, how many moles of H2 would remain? moles H2 0.8