Chemistry help? Easy 10ts.?
When the following equation is balanced with lowest ratio whole number coefficients, the coefficient of CaO is CaO + P4O10 ---- Ca3(PO4)2 a. 3 b. 4 c. 5 d. 6 e. 7
CHEMISTRY HELP!!!!!!!!!!!!! EASY 10 PTS?
balanced equation .. 1 Zn + 2 HBr ---> 1 ZnBr2 + 1 H2 if Zn is the limiting reagent, this much H2 is formed .. 5.00g Zn * (1 mol Zn / 65.68g Zn) * (1 mol H2 / 1 mol Zn) = 0.07648 mol H2 but if HBr is the LR, then this much H2 is formed .. 35.0mL HBr * (1L / 1000mL) * (4.00 mol HBr / L HBr) * (1 mol H2 / 2 mol HBr) = 0.07000 mol H2 since HBr gave less H2, it must be the LR and 0.07000 mol H2 is formed then .. PV = nRT .. P = nRT/V = (0.07000mol H2) * (0.08206 Latm/molK) * (298K) / (1.50L) = 1.14 atm
Chemistry Help: Easy 10 Points?
1. mole of C7H6O3= 185000g/138(Mr of salicylic acid) =1340.57971moles 2. mole of C4H6O3= 189000g/102(Mr of C4H6O3) =1852.941176moles From eqn, it shows, 1 mole of C7H6O3 reacts with 1 mole of C4H6O3 therefore... C7H6O3,salicylic acid is the limiting reagent. 1 mole of mole of C7H6O3,salicylic acid = 1 mole of C9H8O4,aspirin 1340.57971moles of C7H6O3 =1340.57971moles of C9H8O4 Theoretical mass of C9H8O4=1340.57971moles X (9(12)+8+4(16)) =241304.3478g Answer=241.30kg(5 sig fig) % yield of aspirin= 159/241.30 X 100% =65.9%(3 sig fig) ______________________________________... What do you mean by 10-5? is it 10 divided by 5? i don't know about this, so i don't think i can do. sorry ______________________________________... 1. moles of NH3= 3.10/17(Mr of NH3) = 0.182352941 moles From eqn, 4 moles of NH3=4 moles of NO therefore, 0.182352941 moles of NH3= 0.182352941 moles of NO Mass of NO formed=0.182352941 moles X (14+16) =5.471g(4sf) 2. Moles of O2= 4.77g/16(Ar of oxygen) =0.298125moles From eqn, 4 moles of NH3 reacts with 5 moles of O2 0.182352941 moles of NH3=0.227941176 moles of O2 however, the actual moles of O2 present= 0.298125moles This is more than the needed, hence, O2 is the excess reagent. Moles of excess reagent left after reaction= 0.298125moles minus 0.227941176moles = 0.070183823 moles Massof excess reagent left in grams=0.070183823 moles X 16 = 1.123g(4sf) of Oxygen gas left Hope it helps! :D i hope the numbers are all correct.
CHEMISTRY HELP!! EASY 10 Points?
How many grams of silver chloride can be prepared by the reaction of 108.5 mL of 0.21 M silver nitrate with 108.5 mL of 0.14 M calcium chloride? Calculate the concentrations of each ion remaining in solution after precipitation is complete. Ag+ NO 3- Ca 2+ Cl-
Chemistry Help!!!!! Easy 10 points?
Too bad this wasn't already answered on Google, but at least it's there. =( To find C: 14.22g * (12gc/44g CO2) = 3.87 divide that by the total g burned, which is 4.8, to get your % 3.87/4.8=80.625% dvd by the MM of C 80.625/12=6.7 H: 1.66* (2g H/18gH2O) = .184 .184/4.8=3.84% 3.84/1=3.84 Subtract your percents from 100, and you should get 15.535% left over, hence the % O you have. 15.535/16=.97 Since .97 is your lowest limiting factor, divide each factor by .97 C: 6.7/.97=6.9 H: 3.84/.97=3.95 O: .97/.97=1 Round up, C7H4Ois your empirical formula. MM = (m*k*i)/(deltaT *kg) they give you 1.5 mols, multiply that by 104 (MM of C7H4O), and you should get 156g. DeltaT is the change in temperature, which in this case is 66C, and keep it in C. 20.8g is your solvent. convert that to kg and you get .0208 kg. to get K, add 14.7 psi and 13.8 psi, convert to atms, and get 1.94 atms (Don't ask why, but it works in the end). i can be left out. MM= (156*1.94)/(66*.0208)=220.45 Divide 220 by 104, and you should get 2.12. Round up to 2 (your mole ratio), multiply the empirical formula by 2. In the end, you should get C14H8O2 (according to Wikipedia, that's the actual molecular formular) Best of luck, foo.
Chemistry help easy 10 points?
please explain i think i get it but theres somethin im doing wrong Balance the following chemical equations. 1. _____C2H6(g) + _____O2(g) ---> _____H2O(g) + _____CO2(g) 2. _____O2 + _____C6H12O6 ---> _____H2O + _____CO2 3. ___Br2(g) + ___H2O(l) + ___SO2(g) ---> ___HBr(aq) + ___H2SO4(aq) 4. _____KOH + _____H3PO4 ---> _____K3PO4 + _____H2O Balance the following chemical equations. 1. _____Mg + _____N2 ---> _____Mg3N2 2. _____KNO3(s) ---> _____KNO2(s) + _____O2(g) 3. _____Fe + _____H2SO4 ---> _____Fe2(SO4)3 + _____H2 4. _____MgCO3(s) ---> _____MgO(s) + _____CO2(g) Identify the following chemical equations by type. 1. C4H8 + 6O2 ---> 4CO2 + 4H2O 2. HCl + NaOH ---> H2O + NaCl 3. 2KNO3(s) ---> 2KNO2(s) + O2(g) 4. AgNO3 + NaCl ---> NaNO3 + AgCl 5. 2Mg + O2 ---> 2MgO 6. 2Ag + S ---> Ag2S 7. MgCO3(s) ---> MgO(s) + CO2(g)
10 points easy...chemistry help..please!!?
*** 1 *** M1V1 = M2V2 M2= M1V1/V2 = 0.821 M x 25.0 mL / 500 mL = 0.0411 M *** 2 *** 1.9 M means 1.9 moles / L 4.65 moles HCl x (1 L / 1.9 moles HCl) = 2.45 L *** 3 *** 205 g Mg(NO3)2 x (1 mole Mg(NO3)2 / 148.3 g Mg(NO3)2 ) = 1.382 moles Mg(NO3)2 1 mole Mg(NO3)2 has 2 moles NO3- so.,,, 1.382 moles Mg(NO3)2 x (2 moles NO3- / 1 mole Mg(NO3)2 ) = 2.764 moles OH- so molarity of OH- = 2.764 moles OH- / 0.500 L = 5.53 moles OH- / L = 5.53 M OH- finally 0.100 L x (5.53 moles OH- / L) = 0.553 moles OH-
1 chemistry question that i need help with (easy)?
WHOOOPS SOO SORRY FOR MY FIRST ANSWER. I WAS CONSIDERING OXYGEN (16), AND I DIDN'T NOTICE YOU HAD OXYGEN (18) THE ISOTOPE in ionic reactions you never touch the nucleus which contains number of protons and neutrons other wise you will change the atom) so you only modify the number of electrons O18 has 2 more NEUTRONS THAN OXYGEN 16 In oxygen Z = number of protons = number of electrons In Oxide number of electrons = Z+2 = 10 SO THE ANSWER IS B, the others are correct
Help with chemistry homework [stoichiometry] EASY 10 POINTS!!?
this question has me stumped. a 0.7549 g sample of the compound burns in O2(g) to produce 1.9061 g of CO2(g) and 0.3370 g H20(g) 1.calculate the individual masses of C, H, and O in the .7549 g sample 2. determine the empirical fromula for the compound.