Using the following balanced synthesis reaction for silveroxide, how many grams of oxygen are needed tocompletely react with 85.0 grams of silver?4 Ag (s) + O2 (g) ----> 2 Ag2O (s)1 mol Ag107.87 g Ag4 mol 02 6.022 x 1023 , 021 mol Ag"85 g Ag x1 тol O2O 85 g Ag x1 mol Ag107.87 g Ag4 mol 02 22.4 g O21 mol Ag“ 1 mol 02O 85 g Ag x1 mol Ag107.87 g Ag1 тol Op16.00 g О24 mol Ag 1 тol Oz1 mol Ag107.87 g Ag1 mol 02 32.00 g O24 mol Ag" 1 mol 0285 g Ag x

Given: mass of Ag = 85g The given eqn is: We know that, The molar mass of Ag = 107.87 g Molar mass…

Using the following balanced synthesis reaction for silver oxide, how many grams of oxygen are needed to completely react with 85.0 grams of silver? 4 Ag (s) + O2 (g) ----> 2 Ag20 (s) 1 mol Ag 107.87 g Ag * 1 mol Ag 4 mol 02 6.022 z 1023g O2 1 тol Oz 85 g Ag x 1 mol Ag O 85 g Ag x 107.87 g Ag 1 mol Agº 1 mol 02 4 mol 02 22.4 g O2 1 mol Ag 85 g Ag x 107.87 g Ag 4 mol Ag 1 mol 02 1 mol 02 16.00 g O2 1 mol Ag O 85 g Ag x 107.87 g Ag 4 mol Ag™ 1 mol 02 1 mol 02 32.00 g O2

Using the following balanced synthesis reaction for silver oxide, how many grams of oxygen are needed to completely react with 85.0 grams of silver? 4 Ag (s) + O2 (g) ----> 2 Ag20 (s) 1 mol Ag 107.87 g Ag * 1 mol Ag 4 mol 02 6.022 z 1023g O2 1 тol Oz 85 g Ag x 1 mol Ag O 85 g Ag x 107.87 g Ag 1 mol Agº 1 mol 02 4 mol 02 22.4 g O2 1 mol Ag 85 g Ag x 107.87 g Ag 4 mol Ag 1 mol 02 1 mol 02 16.00 g O2 1 mol Ag O 85 g Ag x 107.87 g Ag 4 mol Ag™ 1 mol 02 1 mol 02 32.00 g O2

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

To balance the Chemical equation: X1 Ca3(PO4)2+ x2 H3PO4→X3 Ca(H,PO)2, the equation for the Oxygen O is: 8x1 +4x2=8x3 %3D X1 +8 x2= 2x3 %3D 4x, +4x2= 4X3 8x1 +4 x2= 2x3
3 Cu + 8HNO3 --> 3 Cu(NO3)2 + 2 NO + 4 H2O In the above equation how many moles of water can be made when 178.7 grams of HNO3 are consumed?
What type of chemical reaction is shown in the chemical equation below? * Na PO4+3 KOH → 3 NaOH + KPO4 Synthesis Decomposition Single Displacement Double Displacement Combustion
2 HgO(s) → 2 Hg(ℓ) + O₂(g) 4.00 grams of HgO was used in this reaction. How many moles of HgO were used?
4 NH3 + 5 O 2 -----> 4 NO + 6 H2O HOW MANY MOLES OF OXYGEN (O2) ARE NEEDED TO REACT WITH 51.12 GRAMS OF AMMONIA(NH3) BY THIS REACTION ? NH3 MOLAR MASS = 17.04g/mol 2 C4H10+13 O2 --------------> 8 CO2+ 10H2O HOW MANY GRAMS OF WATER (H2O) ARE PRODUCED IF 100.0 MOLES OF C4H10 ARE USED? H2O MOLAR MASS = 18.02 G /MOL
Balance the chemical equation. What is the coefficient in front of O₂? C3H8(1) + ? O2(g) →→→ CO2(g) + H₂O(g) 02 3 O4 05 none of these
The reaction of a 4.35-g K sample with excess oxygen (O2) yielded 4.82-g K20. What is the percent yield of this reaction? 4 K(s) + O2(g) – 2 K20(s) K 39.10 g/mol 02 32.00 g/mol K20 94.20 g/mol
Which of the following is a balanced chemical reaction(s)? a) H₂SO4 + B(OH)3 → B2(SO4)3 + H₂O b) C12H22O11 + H₂O → 2 C₂H5OH + 2 CO2 c) Sg +8 028 SO₂ d) Fe + AgNO3 → Fe(NO3)2 + Ag
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 g
In the following reaction, how many grams of lead(II) nitrate, Pb(NO3)2, will be needed to react with 60.7 g of potassium iodide, KI? 2KI+Pb(NO3)2 -----> PbI2+2KNO3
Fernando is doing his pre-lab homework for Chemistry. He is asked to predict how many grams of CO, are produced if 2.09 mol of HCl are reacted according to this balanced chemical equation shown. CaCO3+2HCI→ CaCl2 + CO2+ H2O He performs the following calculation. 1 mol-EO, 44.019CO, 2 motHCT 1malEo, 2.09 motHCT x = 46.0 g CO, X- from the coefficients of the balanced equation On the day of the lab his group obtains 40.9 grams of CO2 as their experimental result. What is their percent yield? round your answer to the tenths place, i.e. one decimal place
A sample of 0.75 g of hydrogen gas was obtained by reacting 32.5 g hydrochloric acid with 18.0 g magnesium. Mg(s) + 2 HCI (aq) --> MgCl₂ (aq) + H₂(g) What is the percent yield for this reaction? 100% 83% 41% 50%