How many grams of Ni are formed from 51.7 g of Ni2O3? 2Ni2O3(s)⟶4Ni(s)+3O2(g) Ⓒ Macmillan Learninggrams Ni₂03Incorrect51.7 g Ni₂03 xgrams N₁₂03Incorrectmoles O,165.38 g Ni₂O3Answer Bank1 mole 0₂grams O₂moles NiStep 2: Show the conversions required to solve this problem and calculate the grams of Ni.moles Ni₂033 moles 0₂grams Ni1 mole Ni₂03Answer Bank→grams Ni58.69 g Ni2 moles Ni₂O31 mole Ni= g Ni32.00 g 0₂4 moles Ni

Nickel(III) oxide decomposes into nickel metal and oxygen gas. The equation for the balanced…

Macmillan Learning grams Ni₂O3 → Incorrect 51.7 g Ni₂03 X grams Ni₂03 Incorrect moles 0₂ 165.38 g Ni₂0₂ Answer Bank 1 mole 0₂ grams 0₂ moles Ni Step 2: Show the conversions required to solve this problem and calculate the grams of Ni. X moles Ni₂0₂ 3 moles 0₂ grams Ni 1 mole Ni₂03 Answer Bank grams Ni 58.69 g Ni 2 moles Ni₂0₂ 1 mole Ni = g Ni 32.00 g 0₂ 4 moles Ni

Macmillan Learning grams Ni₂O3 → Incorrect 51.7 g Ni₂03 X grams Ni₂03 Incorrect moles 0₂ 165.38 g Ni₂0₂ Answer Bank 1 mole 0₂ grams 0₂ moles Ni Step 2: Show the conversions required to solve this problem and calculate the grams of Ni. X moles Ni₂0₂ 3 moles 0₂ grams Ni 1 mole Ni₂03 Answer Bank grams Ni 58.69 g Ni 2 moles Ni₂0₂ 1 mole Ni = g Ni 32.00 g 0₂ 4 moles Ni

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter8: Chemical Composition

Section: Chapter Questions

Problem 128CP: itamin B12 , cyancobalamin, is essential for human nutrition. Its molecular formula is...

See similar textbooks

Similar questions

1. A student collected the following data during Lab: Mass of MgCO3 hydrate = 0.9987 g. Constant mass of anhydrous MgCO3 = 0.4831 g How many moles of water were in the MgCO3 hydrate? 2. A student uses gravimetric determination to find the water of hydration of a hydrated sample of cobalt (II) sulfate. The student’s sample contained 0.0098459 moles of anhydrous cobalt(II) sulfate (CoSO4) and 0.068921 moles of water (H2O). What is the formula of the cobalt(II) sulfate hydrate? 3. A student has a sample of CaSO4 hydrate and it weighs 0.4813 grams. He heats it strongly to drive off the water of hydration, and after subsequent heatings, the student finds the anhydrous compound has a constant mass of 0.3750 grams. Find the formula of the hydrate.
Na2CO3(aq) + CaCl2⋅2H2O → CaCO3(s) + 2NaCl(aq) + 2H2O(aq) A. how many moles of CaCl2•2H2O are present in 1.50 g of CaCl2•2H2O and then calculate how many moles of pure CaCl2 are present in the 1.50 g of CaCl2•2H2O. B. determine how many moles of Na2CO3 are necessary to reach stoichiometric quantities. From that calculation, determine how many grams of Na2CO3 are necessary to reach stoichiometric quantities
Convert 7.61 mol NaCl to moles of CaCl2, using the equation given below. Round to the nearest 0.01, and remember to include units (properly abbreviated) and substance in your answer! Na3PO4 + CaCl2 --> Ca3(PO4)2 + NaCl
Sodium hydroxide reacts with carbon dioxide as follows: 2NaOH(s)+CO2(g)→Na2CO3(s)+H2O(l) How many moles of Na2CO3Na2CO3 can be produced? Express your answer in moles to two decimal places.
When the following equations are balanced using smallest integers, what is the coefficient O2 or H2? a) C8H18(l) + O2(g) → CO2(g) + H2O(g) Coefficient of O2 = b) CH3OH(l) + O2(g) → CO2(g) + H2O(g) Coefficient of O2 = c) NH3(l) + O2(g) → NO(g) + H2O(g) Coefficient of O2 = d) Fe(s) + HCl(aq) → FeCl3(aq) + H2(g) Coefficient of H2 =
2Al(s) + 3I2(s) > 2AlI3 If 7.5 moles of AlI3 is consumed, then how many moles of I2 is needed? *Use conversion factor
#1 a.) If 60.0 grams of CaCO3 are heated, how many grams of CaO will be produced if the ratio is 1 mole CaCO3: 1-mole CaO. Hint, you will need to convert the grams to moles first. Report your answer to 3 significant figures. b.) The amount you calculated is the actual yield. True or False? Provide an explanation for your answer in the rationale.
Calculate the moles of 1.00 ft3 lead (II) sulfide with a density of 7.46 g/cm3. Group of answer choices 15.9 moles 883 moles 0.950 moles 0.838 moles 779 moles
A halothane- oxygen mixture (C2HBrCIF3 + O2) can be used as an anesthetic. Assume that a tank containing such a mixture has the following particles P(halothane)= 1.70x102torr P Oxygen=5.70x102torr If the tank contains 160 gramns of O2, how many grams of C2HBrCIF3 are present
Use stoichiometry (Ch 13) to calculate how many grams of PbSO4(s) would be produced if 5.50 grams of LiNO3 were produced. It will be helpful to do this on paper first. Li2SO4(aq) + Pb(NO3)2(aq) ⟶2 LiNO3(aq) + PbSO4(s) a. Select the value for the molar mass of LiNO3, with the correct value, significant figures, and units. b. Select the value for the molar mass of PbSO4, with the correct value, significant figures, and units. c. Select the mole ratio that will be used, with the correct values and units. d. Select the first operation and conversion factor used to cancel the given unit and substance. e. Lastly, select the calculated answer, expressed with the appropriate significant figures and unit.
Acetic acid (CHaCOOH) can be produced based onthe reaction: CHgCOOC2H5+ H20+CH COOH+C2H5OH. If there are 344.5 g of CHgCOOC2H5 and165.8 g of H20a. How many moles of acetic acid will be produced?3.910 b. Calculate the percent yield if 125 g of acetic acidwas produced (express your answer in 1 decimal placeonly).53 2
KSCN(aq) + Ag+(aq) → AgSCN(aq) + K+(aq) By calculation she determines the buret delivered: 6.52108 moles of KSCN. The moles of Ag+ which were present in her sample was: