A 2.337 g sample of magnesium carbonate (MgCO3) was dissolved in hydrochloric acid. The following reaction occurred at 27.1oC and a pressure of 784 mmHg:
MgCO3(s) + 2HCl(aq) --> CO2(g) + H2O(l) + MgCl2(aq)
Calculate the volume (in mL) of CO2 produced.
Give your answer to the correct number of significant figures and in units of mL.
Data: 1 atm = 760 mmHg, 0oC = 273 K, PV = nRT, R = 0.0821 L.atm.mol-1.K-1, Molar mass (g/mol) of Mg = 24.31, C = 12.01 O = 16.00.
A 2.337 g sample of magnesium carbonate (MgCO3) was dissolved in hydrochloric acid. The following reaction...
If 5.49 kg of propane gas (C3H8) is stored in a 86.8 L container at 15.9oC, what pressure (in atm) will be exerted on the storage tank? Give your answer to the correct number of significant figures and in units of atm. Data: 1 atm = 760 mmHg, 0oC = 273 K, PV = nRT, R = 0.0821 L.atm.mol-1.K-1, Molar mass (g/mol) of C = 12.01 H = 1.008.
A 1.75 L volume of helium gas stored at 0.873 atm will have a temperature of 46.9oC. If the helium is compressed down to a volume of 523 mL while allowing the pressure to settle at 1,662 mmHg, what will the temperature of the helium gas now be, in oC? Give your answer to one decimal place, and in units of oC. Data: 1 atm = 760 mmHg, 0oC = 273 K, PV = nRT, R = 0.0821 L.atm.mol-1.K-1.
If 3.95 kg of propane gas (C3H8) is stored in a 68.5 L container at 19.1°C, what pressure (in atm) will be exerted on the storage tank? Give your answer to the correct number of significant figures and in units of atm. Data: 1 atm = 760 mmHg, 0°C = 273 K, PV = nRT, R = 0.0821 L.atm.mol-1.K-1, Molar mass (g/mol) of C = 12.01 H = 1.008.
Hydrogen gas can be produced in the laboratory through the reaction of magnesium metal with hydrochloric acid: Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g) What is the volume, in liters, of H2 gas produced at 22 ∘C and 840 mmHg from the reaction of 32.0 g of Mg?
14. The reaction of magnesium metal with hydrochloric acid produces hydrogen gas as a product. I would like to collect 125 mL of hydrogen gas from the experiment. The temperature of the lab is 23.5°C and the pressure is 762 mmHg. How many grams of magnesium metal should I use if the hydrochloric acid is kept in excess? Mg(s) + 2 HCl(aq) MgCl2(aq) + H2(g)
Question 16 In the reaction of magnesium metal with hydrochloric acid: Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g) How many moles of hydrogen are produced if 10 moles of HCI react?
Assignment/takeCovalentActivity.do locator assignment take (References) An 18.6 mL volume of hydrochloric acid reacts completely with a solid sample of MgCO,. The reaction is 2HCl(aq) + MgCO3(s) + CO2(g) + H20(1) + MgCl, (aq) The volume of CO2 formed is 135 mL at 23°C and 731 mmHg. What is the molarity of the HCl solution? Molarity = Submit Answer Try Another Version 3 item attempts remaining
Calcium carbonate, CaCO3, reacts with stomach acid, (HCI, hydrochloric acid) according to the following equation: CaCO3(s) + 2HCl(aq)-CO2(g) + H2O(1) +CaCl2(aq) Tums, an antacid, contains CaCO3. If Tums is added to 20.0 mL of a 0.400 M HCl solution, how many grams of CO2 gas are produced?
Aqueous hydrochloric acid reacts with magnesium to produce hydrogen gas according to the balanced equation below 2HCl (aq) + Mg (s) = MgCl2 (aq) + H2 (g) If 250.0 mL of 3.00 M HCl is combined with 9.92 g Mg, what volume of hydrogen gas can be produced? Assume the temperature and pressure of the gas are 25oC and 0.988 atm, respectively. ( R=0.08206 )
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?