Question

1.) Imagine that you have a 7.00 L gas tank and a 4.00 L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 155 atm , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases. Express your answer with the appropriate units.

2.) Part 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? Express your answer with the appropriate units. Part 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 of 4.00 g of butane? Express your answer with the appropriate units. 3.) One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 atm and a temperature of 273 K. The temperature is then increased to 301 K , but the container does not expand. What will the new pressure be? Part A The most appropriate formula for solving this problem includes only which variables? Enter the required variables, separated by commas (e.g., P,V,T). View Available Hint(s)

Answer 1

1) In order for both gases to exit at the same time, they must have the same pressure, that is 155 atm.

2) Part A: The moles of CO2 are calculated:

n CO2 = P * V / R * T = 1 atm * 25 L / 0.082 * 273 K = 1.12 mol

The mass of CaCO3 is calculated:

m CaCO3 = 1.12 mol CO2 * (1 mol CaCO3 / 1 mol CO2) * (100 g CaCO3 / 1 mol) = 112 g

Part B: I) The moles of CO2 formed are calculated:

n CO2 = 4 g butane * (1 mol / 58.12 g) * (8 mol CO2 / 2 mol butane) = 0.275 mol

The volume is calculated:

V = n * R * T / P = 0.275 * 0.082 * 296 K / 1 atm = 6.7 L

3) The final pressure is calculated:

P2 = P1 * T2 / T1 = 1 atm * 301 K / 273 K = 1.10 atm

If you liked the answer, please rate it in a positive way, you would help me a lot, thank you.