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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text:Question 5
Copper(II) nitrate crystallises as a hydrate Cu(NO3)2 ' x H20
In order to determine the number of mole of water in a mole of the hydrate, 2.416 g of the blue, hydrated
crystals was carefully heated to remove the water, 1.876 g of the anhydrous Cu(NO3)2 was left.
(a) Write a balanced equation for the heating of Cu(NO3)2 X H2O.
(b) Use these data to determine the value of x (the number of mole of water per mole of Cu(NO3)2 x H2O.
(x = 3)
%3D
(c) Unfortunately, one student heated the compound too strongly and some of the copper(II) nitrate
decomposed to produce NO2(E) and O2(e)
Balance the equation for the decomposition:
Cu(NO3)2(5)
CuO(s)
NO2(8)
O2(e)
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- Treatment of a 0.3500-g sample of impure potassium chloride with an excess of AgNO3 resulted in the formation of 0.3846 g of AgCl. Calculate the percentage of KCl in the sample.arrow_forward7. Balance the following equation; C+0, → CO,arrow_forwardIf 2.952 g of copper(II) nitrate is reacted with sufficient sodium hydroxide, how much copper (II) hydroxide will be produced?arrow_forward
- Elemental iron is produced according to the following reaction: Fe2O3(s) + Al(s) ---> Al2O3(s) + Fe(s) If 5.34 g Fe2O3 is allowed to react with excess Al, what is the theoretical yield of elemental iron for this reaction? A) 0.934 g B) 1.87 g C) 3.73 g D) 6.82 garrow_forwardWhich of the metals (Fe, Zn, Mg) will react in an aqueous solution of AL(NO3)3 to produce aluminum meatal?arrow_forwardA3) Balance the following equation. You must enter a number in every blank. Fe(s) + O2lg) → Fe3O4(s)arrow_forward
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