3. Balance the reaction and then answer the following question: NaOH + H2S04 → H20 + Na2S04 a. How many moles of water will be formed if you start with 2.54 moles of NaOH? b. How many grams of Sodium sulfate will be formed if you start with 5.00 moles of Sodium hydroxide? c. How many grams of sulfuric acid are required to make 101 grams of Sodium sulfate? H2SO4 – Sulfuric acid Na2SO4 – Sodium sulfate -

3. Balance the reaction and then answer the following question: NaOH + H2S04 → H20 + Na2S04 a. How many moles of water will be formed if you start with 2.54 moles of NaOH? b. How many grams of Sodium sulfate will be formed if you start with 5.00 moles of Sodium hydroxide? c. How many grams of sulfuric acid are required to make 101 grams of Sodium sulfate? H2SO4 – Sulfuric acid Na2SO4 – Sodium sulfate -

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter6: Chemical Calculations: Formula Masses, Moles, And Chemical Equations

Section: Chapter Questions

Problem 6.61EP: For the chemical reaction Sb2S3+6HCl2SbCl3+3H2S write the conversion factor that would be needed to...

See similar textbooks

Similar questions

Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A tiny portion of the starting mixture is represented by the diagram, where the blue circles represent N and the white circles represent H. Which of these represents the product mixture? For the reaction of the given sample, which of these statements is true? (a) N2 is the limiting reactant. (b) H2 is the limiting reactant. (c) NH, is the limiting reactant. (d) No reactant is limiting: they are present in the correct stoichiometric ratio.
4.9 Sulfur, S8, combines with oxygen at elevated temperatures to form sulfur dioxide. (a) Write a balanced chemical equation for this reaction. (b) If 200 oxygen molecules are used up in this reaction, how many sulfur molecules react? (c) How many sulfur dioxide molecules are formed in part (b)?
4.72 The picture shown depicts the species present at the start of a combustion reaction between methane, CH4 and oxygen, O2 (a) What is the limiting reactant? (b) Draw the resulting state after this set of reactants has reacted as far as possible.
4.110 Write the balanced chemical equation lot the combustion of ethane, C2H6, and answer these questions. (a) How many molecules of oxygen would combine with 14 molecules of ethane in this reaction? (b) If 13.0 mol of oxygen is consumed in a reaction, how many moles of water are produced? (e) How many grams of ethane are burned if 4.201022 molecules of CO2 are produced?
4.30 Copper reacts with nitric acid via the following equation: 3Cu(s)+8HNO3(aq)3Cu( NO3)2(aq)+2NO(g)+4H2O(l) What mass of NO(g) can be formed when 10.0 g of Cu reacts with 115 g of HNO3?
4.70 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) identify the limiting reactant, and explain how the pictures allow you to do so.
4.71 The particulate scale drawing shown depict the products of a reaction between N2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) Identify the limiting reactant, and explain how the pictures allow you to do so.
You have seven closed containers, each with equal masses of chlorine gas (Cl2) . You add 10.0 g of sodium to the first sample, 20.0 g of sodium to the second sample, and so on (adding 70.0 g of sodium to the seventh sample). Sodium and chlorine react to form sodium chloride according to the equation 2Na(s)+Cl22NaCl(s) After each reaction is complete, you collect and measure the amount of sodium chloride formed. A graph of your results is shown below. Answer the following questions: a. Explain the shape of the graph. b. Calculate the mass of NaCl formed when 20.0 g of sodium is used. c. Calculate the mass of Cl2 in each container. d. Calculate the mass of NaCl formed when 50.0 g of sodium is used. e. Identify the leftover reactant, and determine its mass for parts b and d above.
For the chemical reaction Sb2S3+6HCl2SbCl3+3H2S write the conversion factor that would be needed to do each of the following one-step conversions. a. Moles of SbCl3 to moles of H2S b. Moles of Sb2S3 to moles of HCl c. Moles of H2S to moles of HCl d. Moles of Sb2S3 to moles of SbCl3
In a laboratory experiment, the reaction of 3.0 mol of H2 with 2.0 mol of I2 produced 1.0 mol of HI. Determine the theoretical yield in grams and the percent yield for this reaction.
Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.