If 63.8 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and decompose completely via the equation below, what would be the final pressure of carbon dioxide (in atm) assuming it had the full 2.00 L in which to expand? H₂CO₃(aq) → H₂O(l) + CO₂(g)

What volume of carbon dioxide gas (in mL) at 835 mm Hg and 37 °C can be produced when 2.4 g of CaCO3(s) are put into an Erlenmeyer flask containing 108 mL of 0.152 M HCl(aq) ?1 CaCO3(s) + 2 HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)

What is the partial pressure of CO2 if the total pressure is 0.61 atm and the partial pressure of ammonia is 0.26 atm?

A mixture of carbon dioxide and helium gases at a total pressure of 798 mm Hg contains carbon dioxide at a partial pressure of 243 mm Hg. If the gas mixture contains 2.84 grams of carbon dioxide, how many grams of helium are present?   A mixture of methane and krypton gases contains methane at a partial pressure of 658 mm Hg and krypton at a partial pressure of 307 mm Hg. What is the mole fraction of each gas in the mixture?XCH4 = XKr =

4.00 mols of NH3 and 4.00 mols of H2S are placed in an 8.00 L reaction vessel and the mixture is allowed to come to equilibrium. At equilibrium, how many grams of NH4HS (51.11 g/mol) are present? (Assume volume and temperature remain constant.) NH3 (g) + H2S (g) \rightleftarrows⇄ NH4HS (s)       Kc = 400. at 35.0oC

A tank was filled with 18 g of oxygen (O2), 75 g of nitrogen (N2) and 4 g of carbon dioxide(CO2). At 25°C the pressure of the tank was 8.5 atm. If the partial pressure of CO2 in the tank is x atm, what is the value of x?

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Enter your answer in the provided box. A piece of sodium metal reacts completely with water as follows: 2 Na(s)+2H2O(l)->2NaOH(aq)+H2(g)The hydrogen gas generated is collected over water at 23.0\   deg C. The volume of the gas is 291 mL measured at 0.965 atm. Calculate the number of grams of sodium used in the reaction. (The vapor pressure of water at 23.0\deg C=0.027 atm.)

1) An aerosol can with a volume of 0.55 L has a bursting point of 2.6 atm. If the can contains 1.0 g CO₂ (44.01 g/mol) and is heated to 400°C, will it burst? What is the density of the CO(g)

Use the equation that follows for parts (a) and (b) below. Molecular masses are under each salt/molecule. Al2Os (s) + 6 NaOH () + 6 HF (g)→ 2 NasAlF6 (s) + 6 H20 (g) 101.96 40.00 20.01 209.95 18.02 Part a) How many grams of aluminum oxide are needed to react with 3.5 L of HF at 305 K, 4.2 atm pressure in the presence of excess NAOH? Part b) How much energy is released from the reaction of 56.0 g of HF? Assume that 2H for the reaction is -345 kJ.