reactant) if 0.083 moles SiO2 is reacted with 0.30 moles of HF siO2 + 4HF --> SIF4 + 2H2O *MM: SIO2 = 60.09 g/mol; HF = 20.008 g/mol; SiF4 = 104.09 g/mol; H2O = 18.016 g/mol ) 0.0083 mol of SiO2 remains unreacted (in excess) ) 0.025 mol of HF remains unreacted (in excess) 0.033 mol of HF remains unreacted (in excess) 0.011 mol SiO2 remains unreacted (in excess)

reactant) if 0.083 moles SiO2 is reacted with 0.30 moles of HF siO2 + 4HF --> SIF4 + 2H2O *MM: SIO2 = 60.09 g/mol; HF = 20.008 g/mol; SiF4 = 104.09 g/mol; H2O = 18.016 g/mol ) 0.0083 mol of SiO2 remains unreacted (in excess) ) 0.025 mol of HF remains unreacted (in excess) 0.033 mol of HF remains unreacted (in excess) 0.011 mol SiO2 remains unreacted (in excess)

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

S + 6 HNO3 --> H2SO4 + 6 NO2 + 2 H2O In the above equation how many moles of water can be made when 143 grams of HNO3 are consumed?
Question 3 For the following questions do not include units in the answer. When 5.00 g Al (M.W. = 26.98 g/mole) react with 5.00 g O₂ (M.W. = 31.98 g/mole), 7.83 g of Al2O3 (M.W. = 101.96 g/mole) are recovered. a) What is the limiting reagent? 4 Al(s) + 3 O2(g) = 2 Al₂O3(s) AH = - 1676 kJ 1 mole Al2O3 b) What is the theoretical yield (in grams) of Al2O3? (three sig. figs.) c) What is the percent yield of Al2O3? (three sig. figs.) d) How much excess material is left over (in grams)? (three sig. figs.) e) How much energy (in kJ) is produced during the reaction? (three sig. figs.)
What do you need to do first in this problem: "If 17 g of Al reacted with 13 g 02, how many moles of A1203 are produced?" 4 Al (s) + 3 02 (g) --> 2 A1203 (s) O Write a balanced reaction Determine how many and what the given substances are and what substance is the needed one Multiply by the stoichiometric ratio Calculate the molar mass of A1203 needed to divide the grams by
Can you help me find the theoretical yield and percent yield?
Given the equation: (KCl & KNO3) + AgNO3 ---> AgCl (s) + KNO3 If the mass of (KCl & KNO3)= 1.68 grams If there are 0.35109508 moles of AgCl, how many moles of Cl are there?
A mixture of 6.55 g hydrogen (H2. molecular weight 2.016 g/mol) and 37.5 g oxygen (O2, molecular weight 31.998 g/mol) is prepared in an explosion-proof container, and allowed to react forming liquid water (H2O, 18.016 g/mol). 2 H2(g) + O2(g) ---> 2 H2O(l) This explosive reaction is known to have a nearly 100% yield, so it proceeds until all limiting reagent is used up. Please select the correct amount at the end of the reaction.
Mercury can be isolated from its ore by the reaction: 4 HgS + CaO --> 4 Hg + 3 CaS + CaSO4 a- How many Kilograms of Hg are produced along with 9.75 mol of CaSO4? b- How many Kilograms of CaS are produced along with 9.25 kg of Hg?
Consider this reaction (molecular weights are under each compound): HC=CH + 2 HCI MW = 26 36.5 --> C₂H4Cl2 99 If 4.4 g of HC=CH are reacted with 110 mL of a 2.3 M HCl solution, and 6.0 g of product are actually produced, what is the percent yield?
the following reaction. Na2S2O3 (aq) + Cl₂ (g) + H₂O (1)→ NaHSO4 (aq) + HCI (aq) a) How many moles of Na2S2O3 are needed to completely react with 0.12 moles of Cl₂? b) How many moles of HCI can be produced from 0.12 moles of Cl₂? c) How many moles of H₂O are needed to completely react with 0.36 moles of Cl₂? d) How many moles of Cl₂ would have to react to produce 0.24 moles of HCI?
What is the mass of silver chloride produced if 18.75 g of aluminum chloride react in the following unbalanced reaction? (molar masses: AgNO3 = 169.87 g/mol; AlCl3 = 133.33 g/mol; AgCl = 143.32 g/mol; Al(NO3)3 = 213.00 g/mol) AgNO3 + AlCl3 --> AgCl + Al(NO3)3
3NO2 + H20---> 2HNO3 + NO I need 5.0 grams of HNO3 how many grams of NO2 will i use to produce it?
aqueous sulfuric acid (H_{2}*S*O_{4}) reacts with solid sodium hydroxide ( ) to produce aqueous sodium sulfate (N*a_{2}*S*O_{4}) and liquid water (H_{2}*O). If 0.384 g of sodium sulfate is produced from the reaction of 0.98 g of sulfuric acid and 0.36 g of sodium hydroxide , calculate the percent yield of sodium sulfate Round your answer to 2 significant figures.