Detonation of nitroglycerin reaction:
4 C3H5O9N3 (l) ---- > 12CO2(g) + 6N2(g )+ O2 (g) + 10 H2O (g)
Given that 10.0 moles C3H5O9N3
10.0 moles C3H5O9N3*10 mole H2O/4.0 moles C3H5O9N3 = 25 Moles H2O
Part 2
Number of moles = amount in g / molar mass
= 7.0g /207.2 g/ mole
= 0.0338 moles Pb
,moles of Ag can be calculated as follows:
0.0338 moles Pb*2 mole Ag / 1 mole Pb
= 0.0676 moles Ag
Amount in g = number of moles * molar mass
= 0.0676 moles Ag*107.8682 g/ mole
= 7.29189032 g Aag
= 7.3 g
The balanced equation for the detonation of nitroglycerin is shown below. If 10.0 moles of C3H5O9N3 react, how man...
Question 8 3.75 pts The balanced equation for the detonation of nitroglycerin is shown below. If 3.0 mol of C3H5O9N3 react, how many moles of N2 gas should form? 4C3H5O9N3() - 12C02(g) + 6N2(g) + O2(g) + 10H20(g) 0.11 mol N2 4.5 mol N2 6.0 mol N2 2.0 mol N2 No 1.5 mol N2 375 nts
Zinc metal and aqueous silver nitrate react according to the equation: Zn(s) + 2AgNO3 ---> 2Ag (s) + Zn(NO3)2 When an excess of Zn reacts with 25.00 g of AgNO3, (1.30x10^1) grams of silver are produced. What is the percent yield?
molecular equation for the reaction of magnesium metal with aqueous silver nitrate > magnesium + silver nitrate Mg(s) + 2AgNO, (aq) → Mg(NO3)2(aq) + 2Ag(s) copper(11) nitrate silver Cu(NO3)2(aq) Ag(s) silver nitrate AgNO,(aq) Write the molecular equation for the reaction of magnesium metal with aqueous silver nitrate. Include physical states. molecular equation: ABUS Write the net ionic equation for the reaction of magnesium metal with aqueous silver nitrate. Include physical states. net ionic equation:
How many moles of NaCI are produced when 0.5 moles of Na2COs react with excess hydrochloric acid in the acid-base double displacement reaction according to the following equation? Na2COs(s)+2HCl(aq) 2NaCl(aq)+ H20()+ CO2(9) 8.6 g of Na2COs has been neutralised how many grams of NaCI must have been produced? How many moles of Pb(NO3)2 must have reacted with excess KI if 1.5 moles of Pbl2 were produced in the double displacement reaction according to the following equation? Pb(NO3)2(aq) + 2Kl(aq)- Pbl2(s)...
Consider the following balanced equation: 3Li2S(aq) + 2Bi(NO3)3(aq) → 6LiNO3(aq) + Bi2S3(s) If 44.2 moles of Li2S(aq) and 36.2 moles of Bi(NO3)3(aq) are allowed to react to produce 64.6 moles of LiNO3(aq), what is the percent yield of the reaction?
Consider the following balanced equation: 3Li2S(aq) + 2Bi(NO3)3(aq) → 6LiNO3(aq) + Bi2S3(s) If 29.7 moles of Li2S(aq) and 25.4 moles of Bi(NO3)3(aq) are allowed to react to produce 44.2 moles of LiNO3(aq), what is the percent yield of the reaction?
1.) How many moles of calcium metal react with 5.00 mol of hydrochloric acid? ____Ca(s) + HCI(aq)----- _____CaCI2(aq) + _____H2(g) 2.) How many grams of AgCI, silver chloride, are produced from 25.0 mol of AgNO3, silver nitrate? ____AgNO3 + ____BaCI2--------------- _____AgCI + _____Ba(NO3)2
Question 22 From the following balanced equation, 2Ag+(aq)+SO2−4(aq)⟶Ag2SO4(s) how many moles of Ag2SO4 can be formed from 0.50mol Ag+?
Which balanced chemical equation could represent the following result of a precipitation reaction? 0 0 0 400: Select one: • A. K2C1O4(aq) + 2AgNO3(aq) + Ag2 CrO4(s) + 2KNO3(aq) O B. MgSO4(aq) + 2AgNO3(aq) - Ag2SO4(s) + Mg(NO3)2(aq) O C. MgCl2(aq) + 2AgC2H302(aq) + 2AgCl(s) + Mg(C2H302)2(aq) O D. 2K3PO4(aq) + 3Cr2(SO4)3(aq) -- CrPO4(s) + 6KCl(aq) O E. K2S(aq) + Pb(NO3)2(aq) -- PbS(s) + 2KNO3(aq)
a For the following balanced chemical equation, calculate how many moles of products would be produced if 0.666 mol of the first reactant were to react completely CO (9) + 4H2(g) + CH (9) + 2H, 0(1) mol CH mol H2O b For the following balanced chemical equation, calculate how many moles of products would be produced if 0.441 mol of the first reactant were to react completely. BaCl, (aq) + 2AgNO, (aq) + 2ACI(8) + Ba(NO), (aq) mol AgCI...