1. A mass of 3.462 g of a metal carbonate, MCO3, is heated to drive off...
A 5.37 g mixture of sodium chloride and sodium carbonate is heated to decompose the sodium carbonate into sodium oxide and carbon dioxide according to the following chemical equation. Na2CO3 → Na2O + CO2 The sodium chloride will not decompose. If the final mixture has a mass of 4.03 g, what was the percent sodium carbonate in the original mixture? Hint: Consider the Law of Conservation of Matter - the mass of reactants must equal the mass of products. However,...
15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate? Name the hydrate
A.) When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO3(s)→CaO(s)+CO2(g) What is the mass of calcium carbonate needed to produce 25.0 L of carbon dioxide at STP? B.) Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00 atm and 23 ∘C, what is the volume of carbon dioxide formed by the combustion...
A carbonate salt with an unknown metal MCO3 reacts with sulfuric acid to produce MSO4, carbon dioxide gas and water and hydrogen gas. MCO3 (s) + H2SO4 (aq) ---> MSO4(s)+ CO2(g) + H20 (1) a) If 11.75 mL of a 0.1000 mol/L solution of sulfuric acid is reacted with 0.231 g of the MCO3. What is the molar mass and identity of the metal in the carbonate salt? b) What volume (in mL) of carbon dioxide gas is produced at...
A carbonate salt with an unknown metal MCO3 reacts with sulfuric acid to produce MSO4, carbon dioxide gas and water and hydrogen gas. MCO3 (s) + H2SO4 (aq) ---> MSO4 (s)+ CO2 (g) + H2O (l) a) If 11.75 mL of a 0.1000 mol/L solution of sulfuric acidis reacted with 0.231 g of the MCO3. What is the molar mass and identity of the metal in the carbonate salt? b) What volume (in mL) of carbon dioxide gas is produced...
Strontium carbonate decomposes into strontium oxide and carbon dioxide gas when heated, as shown below. What mass of strontium carbonate would be required to produce 1.349 g of strontium oxide, assuming the reaction went at 100% yield? 2. SrCOs(s)->SrO(s)+ CO2 (g) What volume of oxygen, in mlL, would be produced at STP (0 °C and 1.00 atm) by the decomposition of 3.428 g of sodium chlorate, according to the equation below? 3. 2 NACIO,(s)->2 NaCl (s) + 3 O2(g) If...
If 1.3000 g of alum is heated in a cricible to drive off the water and the remaining solid has a mass of 0,7600 g, how many moles of water were removed from the solid? Show calculation and correct number of sig figs
When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO3 ---> CaO + CO2 How many grams of calcium carbonate are needed to produce 73.0 of carbon dioxide at STP?
Gasses a) What is the molar mass of a gas if 5.50 g of the gas fills a 50.0 L container with a pressure of 1590 torr at 30°C? b) 100.0 g of calcium carbonate (CaCO3 ) in a 25.0 L container is heated to 600°C, producing calcium oxide (CaO) and carbon dioxide (CO2). What is the pressure generated in the container when all of the CaCO3 is consumed? after it is allowed to cool down to 20°C? CaCO3 (s)...
CaCO3(s) = Cao (s)+CO2 (g) When heated strongly, solid calcium carbonate decomposes to produce solid calcium oxide and carbon dioxide gas, as represented by the equation above. A 2.0 mol sample of CaCO3(s) is placed in a rigid 100. L reaction vessel from which all the air has been evacuated. The vessel is heated to 898°C at which time the pressure of CO2(g) in the vessel is constant at 1.00 atm, while some CaCO3(s) remains in the vessel. a. Calculate...