CH4(g) + H2O(g) CO(g) + 3 H2(g) If 622 g CHs react with excess H20 at 332 K and
ID: 1089124 • Letter: C
Question
CH4(g) + H2O(g) CO(g) + 3 H2(g) If 622 g CHs react with excess H20 at 332 K and 0.890 atm, what volume of H2 gas will form? Question 4 21 9947 X3 10. At a given temperature, nitrogen gas effuses 1.813 times faster than the gas X, what is the molar mass of X? Question 5 10. Tungsten hexafluoride is one of the heaviest gases known, with a molar mass of 297.9 g/mol. At a given temperature, how long will it take WFs to cover the distance H2 can travel in 58 metuken (t) Question 6 10. You wish to measure the changes in pressures of gases during the course of a reaction using a closed-end mercury manometer. Suppose 805 mmHg N204 is allowed to react to form NO2 according to the reaction, N204(g) 2 NO2(g). The total pressure you measure, as the reaction proceeds, is the sum of the pressures of N204 and NO2 present. When the total pressure is 1250 mmHg, what is the pressure of N2O4? (mmHg) ntiat vrosu sos turouero,un 125 Cus Question 7 10. The diffusion rate of H2 in a lecture hall was found to be 23.0 m/sec at 25°C. How long will it take poisonous HCN gas to diffuse 13 m in the same room? (s) 13%6 Question 8 10. During the decomposition of CaCO,(s) into Ca0(s) and CO2(8), 97.0 mL of gas is collected isplacement of water in a flask at 18°C with an atmospheric pressure of 757 mmHg. The 2Explanation / Answer
Question 4)
It is based on Graham's law of diffusion(effusion).
the rate of diffusion of a gas is inversely proportional to square root of its molar mass.
Thus for two gases effusing
rate of gas1/ rate of gas 2 = Square root of [ molar mass 2 / molar mass1]
1.813/1 = square root of [ M2/28]
Thus molar mass of gas X (M2) =92.035 g/mol