3 Cu + 8HNO3 → 3 Cu(NO3)2 + 2 NO + 4 H₂O In the above equation, how many grams of water can be made when 7.9 moles of HNO3 are consumed? Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0 Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.: Molar Element Mass Hydrogen 1 Nitrogen 14 Copper 63.5 Oxygen 16

3 Cu + 8HNO3 → 3 Cu(NO3)2 + 2 NO + 4 H₂O In the above equation, how many grams of water can be made when 7.9 moles of HNO3 are consumed? Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0 Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.: Molar Element Mass Hydrogen 1 Nitrogen 14 Copper 63.5 Oxygen 16

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...

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Aluminum nitrate reacts with sodium hydroxide according the the equation below. When 10.99 grams of aluminum nitrate is added to an excess amount sodium hydroxide, how many moles of aluminum hydroxide will be produced by the time the reaction is 29% complete? Report your answer with three significant figures. Al(NO3)3 (s) + 3 NaOH (aq) → Al(OH)3 (s) + 3 NaNO3 (aq)
3 Cu + 8HNO3 → 3 Cu(NO3)2 + 2 NO + 4 H2O In the above equation, how many grams of water can be made when 16.8 moles of HNO3 are consumed?
What is the formula (solve for x) for the original hydrated sample of copper (II) sulphate? You weigh a sample of CuSO4 · XH2O. After you heat the sample, you find that the mass of the anhydrous salt is 1.47g. What is the value of x? CONTEXT Mass of just anhydrous compound = mass of anhydrous compound rod mass of beaker and 108.34g - 106.87g = 1.47g %3D %3D = original compound mass - anhydrous compound mass = 3.00g - 1.47g = 1.53g Mass of just water
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Is H₂O₂ being created or destroyed by the chemical reaction? If H₂O2 is being created or destroyed, what is the rate at which it is being created or destroyed 1000 seconds after the reaction starts? Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. If H₂O₂ is being created or destroyed, what is the average rate at which it is being created or destroyed during the first 1000 seconds of the reaction? Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. ооо created destroyed neither created nor destroyed 0 x10 00 X Ś 0
Aluminum nitrate reacts with sodium hydroxide according the the equation below. When 19.39 grams of aluminum nitrate is added to an excess amount sodium hydroxide, how many moles of aluminum hydroxide will be produced by the time the reaction is 62% complete? Report your answer with three significant figures. AINO3)3 (s)+3 NaOH (aq) - A(OH)3 (s) + 3 NANO3 (aq)
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.
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Mercury can be obtained by reacting mercury(II) sulfide (show below) with calcium oxide. If you began with 136.6 grams of mercury(II) sulfide and mixed it with excess amounts of calcium oxide, how many moles of calcium sulfide will you make? 4 HgS (s) +4 CaO (s)--> 4 Hg (1)+3 CaS (s) +1 CaSO4 (s) round your answer using appropriate sig fig rules
An experiment using the reaction below produces 36.51 grams of chlorine gas (Cl2). What mass of HF is produced by this experiment? Round your answer to the nearest 0.01 and remember to include units and substance! HCl + F2 -- > HF + Cl2
Carbogenum (a mixture of gases 7% CO2 and 93% O2). It is used in surgicalpractice to stimulate breathing during anesthesia. Calculate the amount of oxygen (in mols) in 150 liters (STP) of carbogen.
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