Al(OH),(s) + HCI(aq) - AICI, (aq) + H,0(1) C. Calculate the number of grams of AICI, and the number of grams of H,O formed when 0.500g of Al(OH), b. Calculate the number of grams of HCI that can react with 0.500g of Al(OH), 4. Several brands of antacids use Al(OH), to react with stomach acid, mostly HCI. +] a. Balance this equation. reacts.

Al(OH),(s) + HCI(aq) - AICI, (aq) + H,0(1) C. Calculate the number of grams of AICI, and the number of grams of H,O formed when 0.500g of Al(OH), b. Calculate the number of grams of HCI that can react with 0.500g of Al(OH), 4. Several brands of antacids use Al(OH), to react with stomach acid, mostly HCI. +] a. Balance this equation. reacts.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter3: Mass Relations In Chemistry; Stoichiometry

Section: Chapter Questions

Problem 53QAP: Cyanogen gas, C2N2, has been found in the gases of outer space. It can react with fluorine to form...

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Cyanogen gas, C2N2, has been found in the gases of outer space. It can react with fluorine to form carbon tetrafluoride and nitrogen trifluoride. C2N2(g)+7F2(g)2CF4(g)+2NF3(g)(a) How many moles of fluorine react with 1.37 mol of cyanogen? (b) How many moles of CF4 are obtained from 13.75 mol of fluorine? (c) How many moles of cyanogen are required to produce 0.8974 mol of NF3? (d) How many moles of fluorine will yield 4.981 mol of nitrogen trifluoride?
4. ) 58.12 g/mol 32.00 g/mol 44.01 g/mol 18.02 g/mol 2C4H1ogy + O2ig) CO2(gi + H2Oigi a. Calculate the mass of carbon dioxide (in grams) that can be produced from 23.00 grams of butane liquid. b. Calculate the percent yield if a student uses 23 grams of butane but obtains 56.25 grams of carbon dioxide.
In the equation: NAOH • H,SO, -→ Na,S0. + H,0 25.0 g of NaOH (40 g/mo) reacts with 50.0 g of H,SO. (98g/mo) which resulted to the production of Na,SO, and water. 20. How much Na,So, is produced when all limiting reactant is consumed? A. 34. 50 g of Na.so. C. 72.45 g of NaSO. D. 88.75 g of NaSO.
Be sure to answer all parts. Ammonia is a colorless gas with a pungent, characteristic odor. It is prepared by the reaction between hydrogen and nitrogen: 3H,(g) + N2g) – 2NH,(g) In a particular reaction, 7.6 moles of NH, were produced. How many moles of H, and how many moles of N2 were consumed to produce this amount of NH,? moles H2 moles N2=
If 3.5 moles of calcium carbide (CaC,) react with an excess of water, how many moles of acetylene (C,H,) will be produced? CaC, + H,O I Ca(OH), + CH, How many grams of propane (C,H,) are needed to produce 5.0 moles of Co,? CH.+ 0,0 CO, + H,0 How many moles of ammonia (NH,) will be produced when 7.5 grams of N, react with excess hydrogen? N + H, O NH,
8. Use the following equation for the following: ni 916 2siuosiom ynsm woll Mg3N2 + H₂O → Mg(OH)2 + NH3 20000.0 6 a. Balance the equation. IX IX. b. How many moles of NH3 are produced when 0.0425 moles of Mg3N2 are reacted? c. How many grams of H₂O are needed to form 6.31 x 10-5 moles of Mg(OH)2 ? d. How many molecules of H₂O are needed to react with 0.525 lbs Mg3N₂? e. How many kilograms of Mg(OH)2 are produced when 7.23 x 1027 molecules of NH3 are also produced? f. How many grams of Mg3N2 are needed to make 4.18 lb Mg(OH)2 ?
1.) The combustion of propane (C3H8) produces CO2 and H2O: C3H8(g) + 5O2 (g) ---> 3CO2 (g) + 4H2O (g) The reaction of 2.5 mol of O2 with 4.6 mol of propane will produce _______ mol of H2O.
3. Acetic acid (CH;COOH) can be produced based from the reaction: CH;COOC2H5 + H2O → CH;COOH + C2H5OH If there are 344.5 g of CH3COOC2H5 and 165.8 g of H20 How many moles of acetic acid will be produced? b. Calculate the percent yield if 125 g of acetic acid was produced а.
aqueous sulfuric acid (H_{2}*S*O_{4}) reacts with solid sodium hydroxide ( ) to produce aqueous sodium sulfate (N*a_{2}*S*O_{4}) and liquid water (H_{2}*O). If 0.384 g of sodium sulfate is produced from the reaction of 0.98 g of sulfuric acid and 0.36 g of sodium hydroxide , calculate the percent yield of sodium sulfate Round your answer to 2 significant figures.
Consider the following reaction.Na2S2O3 (aq) + Cl2 (g) + H2O (l) → NaHSO4 (aq) + HCl (aq)a) How many moles of Na2S2O3 are needed to completely react with 0.12 moles of Cl2?b) How many moles of HCl can be produced from 0.12 moles of Cl2?c) How many moles of H2O are needed to completely react with 0.36 moles of Cl2?d) How many moles of Cl2 would have to react to produce 0.24 moles of HCl?
Consider the reaction between HCl and O2: 4 HCI + O2 -> 2 H20 + 2 Cl2 Calculate the theoretical yield of H20 when 64 grams of HCI react with 19 grams of 02. O A) 16 g H2O O B) 21 g H2O O C) 32 g H20 O D) 43 g H2O Question 8 (Mandatory) (2 points) Consider the following chemical reaction: 4 Al + 3 O2 --> 2 Al2O3 If 12.85 g of Al reacts completely with oxygen and 18.42 g of aluminum oxide is obtained, what is the percent yield of the reaction? 49°F
8. In the reaction 2 Na + 2 H2O → 2 NaOH + H2(g), the number of moles of H2 produced when 20.0 g of NaOH is formed is 1) 1: 2) 0.25; 3) 0.5; 4) 10