When hydrogen sulfide gas is bubbled into a solution of NaOH, the reaction forms sodium sulfide and water according to the following unbalanced reaction. H₂S + 2NaOH → Na₂S + H₂O How many grams of sodium sulfide are formed if 2.75 g of hydrogen sulfide is bubbled into a solution containing 2.75 g of sodium hydroxide. Atomic weights: Na 23.0, O 16.0, H 1.0, S 32.0)

When hydrogen sulfide gas is bubbled into a solution of NaOH, the reaction forms sodium sulfide and water according to the following unbalanced reaction. H₂S + 2NaOH → Na₂S + H₂O How many grams of sodium sulfide are formed if 2.75 g of hydrogen sulfide is bubbled into a solution containing 2.75 g of sodium hydroxide. Atomic weights: Na 23.0, O 16.0, H 1.0, S 32.0)

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

1. Consider the generic reaction: A + 2B→ CHow many moles of C are formed upon the complete reaction of:A. 5.0 moles of AB. 5.0 moles of B 2. For the reaction: 2N2O5 → 4NO2 + O2Calculate how many moles of NO2 form when each amount of the reactant completely reacts.A. 1.3 moles N2O5B. 1.006x10-3 mole N2O5 3. For the reaction: 2S + 3O2 → 2SO3A. Calculate the moles of S needed to completely react with 1.75 moles of O2B. Calculate the moles of product that form when 1.75 moles of O2 completely reacts. Assume thereis more than enough S. 4. For the reaction: 2S + 3O2 → 2SO3A. Calculate the mass of S (32.07 g/mol) needed to completely react with 5.3 g of O2 (32.00 g/mol).B. Calculate the mass of SO3 (80.07 g/mol) that form when 5.3 g of O2 completely reacts. Assumethere is more than enough S. 5. A mixture containing 21 moles of F2 and 8 moles of S is allowed to react according to the reaction:3F2 + S → SF6A. What is the limiting reactant?B. How many moles of the excess reactant remain after…
What is the balanced equation for the experiment hot ice (sodium acetate)? ***For example: The decomposition of the hydrogen peroxide into water and oxygen is catalyzed by the iodide ion. 2 H2O2(aq) → 2 H2O(l) + O2(g) This is what I have but I feel like I am missing something? Na+ [HCO3]- + CH3 - COOH ---> CH3 - COO-NA+ + H2O + CO2
The reaction for producing glucose in plants, called photosynthesis, is 6CO2+6H2O−→−−lightC6H12O6+6O2 6CO2+6H2O→lightC6H12O6+6O2 If a plant produces 5.81 mol C6H12O6,5.81 mol C6H12O6, how many moles of CO2CO2 are needed? moles CO2CO2:
Calculate the mass(in grams) of the product formed when 15.40g of Cl_2(g) completely reacts. Assume that there is more than enough of the other reactant. 2 K(s) + Cl _2(g) --> 2KCl(s)
Classify each chemical reaction: Reaction Cl₂(g) + 2KI (aq) → 2KCl(aq) + 1₂ (s) H₂SO₂ (aq) H₂O(l) + SO₂ (g) PbCl₂ (aq) + FeSO (aq) → FeCl₂ (aq) + PbSO₂ (s) Mg(s) + F₂ (g) → MgF₂ (s) Type choose one choose one choose one choose one X Ś
Solid copper can be produced by passing gaseous ammonia over solid copper (II) oxide at high temperatures, according to the following reaction. NH3 (g) + CuO (s) → N2 (g) + Cu (s) + H2O (g) Balance the reaction.
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: →+P4s 5O2g 2P2O5g In the second step, diphosphorus pentoxide and water react to form phosphoric acid H3PO4 : →+P2O5g 3H2Ol 2H3PO4l Suppose the yield of the first step is 66.% and the yield of the second step is 62.% . Calculate the mass of phosphorus required to make 2.0kg of phosphoric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
17
Consider the general chemical equation 3A+B→2C. Part A. If 1.45 g of A reacts with 1.75 g of B, what is the mass of C? Express your answer with the appropriate units. Part B. If 4.70 g of A reacts to produce 8.95 g of C, what is the mass of B? Express your answer with the appropriate units.
Dibenzalacetone, C₁7H₁40 (molar mass= 234.29 g mol-¹) is a common ingredient in sunscreens that is prepared by the following chemical reaction. 2 C₂H₂O + C3H₁O →→ C17H140 + 2 H₂O 58.08 g In a lab experiment, 4.25 g of C7HÃO (molar mass = 106.12 g mol-¹) and 1.10 g of C3H6O (molar mass = mol-¹) were used to synthesize C₁7H₁40. The target product was produced as a yellow solid with a 81.0% yield. What mass of C₁7H140 was isolated? Choose the closest answer. 4.44 g 4.69 g 3.60 g 2.22 g 2.35 g 7.52 g
7
When HCl(g) and NH3(g) are mixed, a white solid forms. What is the balanced equation for this reaction? The answer is HCl(g) + NH3(g) = NH4Cl(s) Can you please do a step by step to teach me?