Write a balanced equation:
// CaCO3 (s) + 2HCl(aq) ---> CO2(s) + CaCl2(aq) +
H2O(l) // okay with this
A. A flask holds a total of 402.5 g of water at 20.40C. What is the volume of the flask? (density is .9982 g/ml)
///Got .4032 L(is this correct?)///
B. Assuming that the pressure is 758.4 torr and the temperature is 24.60C, calculate the mass of dry air in the flask. (density is 1.185 g)
///Got .4778g - Is this Correct? ///
C. Assuming the mass of the flask filled with dry air is 125.383 g, calculate the mass of the empty flask.
/// 124.905 g? ///
D. Assuming the mass of the flask filled with CO2 is 125.557g , the temperature is 23.20 C, and the pressure is 758.4 torr, calculate the molecular weight of CO2.
/// 39.4 CO2? //
E. Calculate the actual molecular weight of CO2 and determine the percent error.
//90%// Annoying me that it's not cloase to 98-100%...am i doing something wrong?
No all the calcualation you have did is right there must be some mistake in the mass given
all other calculation i have done and getting the same values as you did
except
percent error = (44 g/mol - 39.4 g/mol / 44 g/mol) * 100 % = 10.45 %
Write a balanced equation: // CaCO3 (s) + 2HCl(aq) ---> CO2(s) + CaCl2(aq) + H2O(l) //...
for the following equilibrium: CaCO3 (s) + 2HCl (aq) <----> CaCl2 (aq) + H2O (l) + CO2 (g) a. write the expression for Kc b. write the expression for Kp
Answer the following for the reaction: CaCO3(s)+2HCl(aq)→H2O(l)+CO2(g)+CaCl2(aq) What is the molarity of a HCl solution if the reaction of 215. mL of the HCl solution with excess CaCO3 produces 10.7 LL of CO2 gas at 725 mmHg and 18∘C?
Calcium carbonate (CaCO3) reacts with stomach acid (HCl, hydrochloric acid) according to the following equation: CaCO3(s)+2HCl(aq)⟶CO2(g)+H2O(l)+CaCl2(aq) Tums, an antacid, contains CaCO3. If Tums is added to 10.0 mL of a solution that is 0.400 M in HCl, how many grams of CO2 gas are produced?
Answer the following for the reaction: CaCO3(s)+2HCl(aq)→H2O(l)+CO2(g)+CaCl2(aq) How many milliliters of a 0.240 M HCl solution can react with 9.25 g of CaCO3? Express your answer with the appropriate units.
Data: Mass of flask filled with air - 150.9425 g Mass of flask filled with CO2 Trial 1 - 150.9775 g Mass of flask filled with CO2 Trial 2 - 150.9805 g Average mass flask filled with CO2 - 150.979 g Temperature of CO2 - 296.15 K Barometer reading - 1.0 atm Density of water at room temp - 0.9978g/mL Density of dry air in flask at room temp - 1.201g/L Calculations: Mass of water in flask - 392.85 mL...
Using the equation: Mg(s) + 2HCl(aq)——> H2(g) + MgCl2(aq) complete the prelab. Prelab Questions 1. A student following the procedures in this b i collected the following data mass Mg. 0.0243 initial syringe volume, ml 0.8 final syringe volume, ml barometric pressure, torr temperature, 293.5 Calculate the value of the universal gas constant, R. 26.3 748 2. What would be the volume of hydrogen pas produced by the reaction of 0.100 g of magnesium metal, collected at 750 torr and...
Mass of stoppered flask + air + tape (record all digits from balance) ISLcBS 22 C 151.70es 22 Air temperature 151.Blo4 S1.8744 Mass of stoppered flask and CO2 (gas) + tape 23 °C °C Temperature of CO: (gas) torr Barometric pressure 204 49 mL Volume of water in flask (= Vgas) g/mL Density of air (from CRC Handbook) Mass of air in flask Calculating ngas Mass of EMPTY stoppered flask + tape Mass of CO2 in flask K K Temperature...
Using the equation: Mg(s) + 2HCl(aq) ———> H2(g) + MgCl2(aq), complete the worksheet. Prelab Questions . A student following the procedures in this lab exercise collected the following data: mass Mg, g 0.0243 initial syringe volume, mi 0.8 final syringe volume, ml 26.3 barometric pressure, tor 748 temperature, K 293.5 Calculate the value of the universal gas constant, R. 2. What would be the volume of hydrogen gas produced by the reaction of 0.100 g of magnesium metal, collected at...
According to the equation: Zn(s) + 2HCl(aq) ----> H2(g) + ZnCl(aq), calculate the volume (L) of H2 gas that can be formed at 25 °C and a pressure of 854 mmHg when 25.0 g of Zn is used in the reaction.
inc metal reacts with hydrochloric acid according to the following balanced equation: Zn(s)+2HCl(aq)→ ZnC l 2 (aq)+ H 2 (g) When 0.124 g of Zn(s) is combined with enough HCl to make 52.2 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.5 ∘ C to 24.2 ∘ C . Find ΔHrxn for this reaction as written. (Use 1.00 g/mL for the density of the solution and 4.18 J/(g⋅∘C) as...