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how to find the percent mass of NaHCo3? mass of solution:30.997 g volume of solution:0.25 L...
A 10.0 g solid sample contains 14.0% NaHCO3 by mass; the rest is NaHSO4. Find the mass of CO2 gas it will produce if treated with an excess of hydrochloric acid. Molar masses: M(NaHCO3) = 84.007 g/mol, M(CO2) = 44.01 g/mol. The gas-evolution reaction: NaHCO3(s) + HCl(aq) = NaCl(aq) + H2O(l) + CO2(g). (A) 0.733 g (B) 1.47 g (C) 2.67 g (D) 4.51 g (E) 5.24 g
1. Consider the reaction: NaHCO3(aq) + HCl(aq) → NaCl(aq) + CO2(g) + H2O(l) Question: 0.056 moles of NaHCO3 are reacted with excess HCl. 2.267 g of CO2 were produced. What is the percent yield of CO2?
Data: Mass of crucible and cover (g): 30.1500g Mass of crucible, cover, and mixture (g): 30.6208 Mass of crucible, cover, and residue after reaction with HCl (g): 1st weighing: 30.1371g 2nd weighing: 30.1372g Mass of unknown sample: .4708g Mass of NaCl formed: .01285g A. Solve the two equations and calculate the mass of NaHCO3 and the mass of Na2CO3- NaHCO3+HCl--->NaCl+CO2+H2O NaCO3+2HCl--->2NaCl+CO2+H2O B. Calculate the percent NaHCO3 in the mixture. C. Calculate the average percent by mass of other elements in...
1. Calculate the molar mass of NaHCO3: of NaHCO: 0 84.01, 2. Write the balance chemical equation for the reaction of sodium bicarbonate with hydrochloric acid: NaHCO3 (s) +_ HCI (aq) → 3. Calculate the volume of CO2 (in mL) of 0.005 moles of CO2 (Remember the gas equation, PV = nRT, where R -0.082 L-atm-mol''.K. Room temperature, T = 20.0°C and Pco2 = 738.5 mm Hg; 1 atm = 760 mm Hg). 4. Calculate the volume of CO2 that...
The reaction of NaHCO3 and HCl produces NaCl, H2O and CO2. The balanced equation is: NaHCO3 + HCl = NaCl + H2O + CO2 You combine 5.0 g of NaHCO3 and 5.0 g of HCl. Determine the limiting reagent. Determine the amount of NaCl formed in the reaction based on these quantities of reactants. How much of the excess reactant remains? Thank you in advance!
Baking soda (NaHCO3) (84.01 g/mol) is often used as an antacid. It neutralizes hydrochloric acid (HCl) (36.46 g/mol) secreted by the stomach according to the balanced equation below. What is the maximum mass of CO2 (44.01 g/mol) that can be produced from a mixture of 2.00 x 103 g NaHCO3 and 5.00 x 102 g HCl? NaHCO3 (s) + HCl (aq) → NaCl (aq) + H2O (l) + CO2 (g) Group of answer choices
A mixture of Na2CO3 and NaHCO3 has a mass of 22 gram. Treatment with excess HCL solution liberates 6 litre of CO2 at 25 degree Celsius and 0.947 atm pressure. Determine the percent of Na2CO3 in the mixture?
Please provide the formulas or steps to solve the four short problems considering the following data: DATA Atmospheric Pressure: 752mmHg Temperature of H2O: 21 deg. C Vapor Pressure of H2O at this temp: 18.7torr Pressure of CO2 in system: 733mmHg Balanced reaction: NaHCO3(aq) + HCl(aq) --> CO2(g) + H2O(l) Mass of Sample: 0.2008g Vol initial: 16.60mL Vol final: 35.10mL Vol total: 20.50mL PROBLEMS 1.) Mols of CO2 2.) Moles of NaHCO3 3.) Mass of NaHCO3 in sample (in grams) 4.)...
Use mass-to-mass stoichiometry, calculate the theoretical yield of NaCl in reaction NaHCO3+HCl —> NaCl+ H2O+CO2 obtained mass of NaHCO3 0.372 grams mass of NaCl got from the reaction 0.148 grams
Given: 2H2 (g) + O2 (g) --> 2H2O (l) Calculate the mass of water produced if 3.50 L O2 is at 1.25 ATM at 22.0oC reacting with excess H2. 4.55 L sample of CO2 has a pressure of 1.12 ATM. If the pressure is increased to 2.50 ATM what would be the resulting volume? Assume constant temp and no change in moles of gas. B) 4.55 L of He is at 25.0oC in a balloon. If the temp is increased...