Imagine that you have a 6.50 L gas tank and a 3.00 L gas tank. You need to fill
ID: 1008535 • Letter: I
Question
Imagine that you have a 6.50 L gas tank and a 3.00 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. When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO_3 (s) rightarrow CaO (s) + CO_2 (g) What is the mass of calcium carbonate needed to produce 67.0 L of carbon dioxide at STP? Express your answer with the appropriate units. Butane, C_4H_10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C_4H_10 (g) + 13O_2 (g) rightarrow 8CO_2 (g) + 10H_2O(l) At 1.00 atm and 23 degree 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. Rank the following gases in order of decreasing rate of effusion. Rank from the highest to lowest effusion rate. To rank items as equivalent, overlap them. How is the partial pressure exerted by N_2 gas affected when some O_2 is introduced into a container if the temperature and volume remain constant? The partial pressure of N_2 will increase. The partial pressure of N_2 will decrease. The partial pressure of N_2 will not change. How is the total pressure affected? The total pressure will increase. The total pressure will decrease. The total pressure will not change. An ideal gas differs from a real gas in that the molecules of an ideal gas have an average molecular mass have no attraction for one another have appreciable molecular volumes have no kinetic energy have a molecular weight of zero Of the following gases. will have the greatest rate of effusion at a given temperature. HBr NH_3 CH_4 Ar HCl The kinetic-molecular theory predicts that pressure rises as the temperature of a gas increases because the average kinetic energy of the gas molecules decreases the gas molecules collide more frequently with the wall the gas molecules collide less frequently with the wall the gas molecules collide more energetically with the wall both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wallExplanation / Answer
2) Part A
Mass of CaCO3 to produce 67L of CO2
1 mole of CaCO3 gives 1 mole of CO2
PV = nRT (R = 0.0821Latmmol-1K-1 , T= 273K, P=1 atm)
n = 2.989 moles of CO2
Therefore mass of 2.989 moles of CaCO3 is 298.9 gm
B) 2 moles of butane gives 8 moles of CO2
116 gms of butane gives 352 gms of CO2
Therefore 4 gms of butane gives 12.138 gms of CO2
12.138 gms of CO2 is 0.2758 moles
PV = nRT (P = 1 atm, T =23 C, R = 0.0821, n= 0.2758 moles)
V = 6.7 L
3) The rate of effusion for a gas is inversely proportional to the square-root of its molecular mass (Graham's Law). The gas with the lowest molecular weight will effuse the fastest.
Molecular weight of:
F2 = 38 , H2 = 2, He = 4, C4H10 = 58, NO = 30
Therefore Effusion rate of H2 > He > NO > F2 > C4H10
6) CH4 will have the greatest effusion rate because amongst the given options the molecular weight of CH4 is the least.