The formula of the hydrate of magnesium sulfate was determined (M9SO4.×H20 ) and the following data was obtained. Mass of crucible + lid + unknown 6.0236 g Mass of crucible + lid 4.0002 g Mass of unknown hydrate Mass of crucible + lid + residue: after 1 st heating 5.0842 g after 2 nd heating 5.0426g after 3 rdheating 5.0339g Mass of water lost Mass of anhydrous salt Percent Water in unknown hydrate_ Moles of water in hydrate sample Moles of anhydrous salt in hydrate sample Calculated Mole ratio(H2O: salt) Complete formula of the hydrate

The formula of the hydrate of magnesium sulfate was determined (M9SO4.×H20 ) and the following data was obtained. Mass of crucible + lid + unknown 6.0236 g Mass of crucible + lid 4.0002 g Mass of unknown hydrate Mass of crucible + lid + residue: after 1 st heating 5.0842 g after 2 nd heating 5.0426g after 3 rdheating 5.0339g Mass of water lost Mass of anhydrous salt Percent Water in unknown hydrate_ Moles of water in hydrate sample Moles of anhydrous salt in hydrate sample Calculated Mole ratio(H2O: salt) Complete formula of the hydrate

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

Acetylene can be produced by forcing calcium carbide to react with water, producing calcium hydroxide as a by-product. What mass of acetylene will be produced if 32.05 g of calcium carbide are used in the reaction? Balance the chemical reaction equation and show all work.
1. Balance the following Chemical Reactions: CH3CI+ 02= CO2+ H2O+! Cl2 CH:0+ CO=> CizH2On+! C12H22O11+ H2O+! O2
Please help me fill in the blanks to find out theoretical yield
Balance the following chemical equation (if necessary): C,H(g) + O,(g) –→ H̟O(g) + CO,(g) 04- 3. D2+ 3+ O4+ 1 4 6. 8. 9. 9. (s) (1) (g) (aq) CH0 CO, H̟O Reset • x H,O Delete 5
Give handwritten answer
5. a. What is % w/w when 15.5 grams of C6H12O6 dissolves in enough water to make 251 grams of solution? b. Determine mass of the solvent. 6.A What is % w/v when 15.5 ml of C₂H5OH (density = 0.785 g/ml) dissolves in 251 grams of water? B What is % w/w when 15.5 ml of C₂H5OH (density = 0.785 g/ml) dissolves in 251g of solution? CWhat is the molarity of solution, when 15.5 grams of C₂H5OH dissolves in enough water to make up 251 mL of solution? DCalculate ppb and ppm of the above solution 10. Show your calculation for preparation of 230.0 mL of 0.265 M sodium hydroxide solution from 0.850M sodium hydroxide.
Riccardo states that for the process of iron reacting with sulfur to produce iron(Il) sulfide according to 16FE +35 8Fe, Sy, 16.00 g of iron will react with 3.00 g of sulfur in the reaction. Do you agree or disagree with this statement? Explain.
The iron, tin, and titanium in a sample were jointly precipitated as hydroxides, which were washed and ignited to produce Fe₂O3, SnO₂, and TiO₂. This mxture of oxides, which amounted to 0.3768 g, was dssolved after fusion with potassium pyrosulfate. Analys s showed that 0.0322 g of Ti was present. The ron was determined separately as an oxide: 0.1837 g FeO was found. What was the weight (mass) of tin in the sample?
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
If the empirical formula of a compound is found to be CH2, which of the following value is a plausible molecular mass for the compound? The answer is 70.15. How did you get that?
Chlorine is used by textile manufacturers to bleach cloth. Excess chlorine is destroyed by its reaction with sodium thiosulfate, Na2S2O3, as follows:Na2S2O3(aq) + 4Cl2(g) + 5H2O 2NaHSO4(aq) + 8HCl(aq) Using the concepts established in the previous parts, answer the following questions about the following reaction:The octane in gasoline burns according to the following equation:2C8H18 + 25O2 → 16CO2 + 18H2O(a) How many moles of O2 are needed to react fully with 6.84 mol of octane? (b) How many moles of CO2 can form from 0.511 mol of octane? (c) How many moles of water are produced by the combustion of 8.20 mol of octane? (d) If this reaction is used to synthesize 6.00 mol of CO2, how many moles of oxygen are needed? How many moles of octane are needed? ? mol O2 ? mol C8H18 Thanks.
Be sure to answer all parts. Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures: Hint oints Solution 5Ca + V,05- 5CAO + 2V eBook Guided Solution Print In one process, 1.540 x 10° g of V,O5 react with 2.120 × 10³ g Ca. References (a) Calculate the theoretical yield of V. (b) Calculate the percent yield if 815.0 g of V are obtained. Report your answers to the correct number of significant figures. Next > Mc Graw Hill Prev 4 of 45 31°C Mostly sunny P Type here to search 1080 Jade Pa F12 Prt Sc F11 F10 NumLk F8 F9 F7 F6 E5