A 0.554 gram sample of a metal, M, reacts completely with sulfuric acid accordin
ID: 923720 • Letter: A
Question
A 0.554 gram sample of a metal, M, reacts completely with sulfuric acid according to: M(s) + H_2SO_4(aq) rightarrow MSO_4(aq)+H_2(g) A volume of 215 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr and the temperature is 25 degree C. Calculate the molar mass of the metal. At 1 atm, how much energy is required to heat 83.0 g of H2O(s) at -10.0 degree C to H_2O(g) at 175.0 degree C? 741 cal of heat is added to 5.00 g ice at - 20.0 degree C. What is the final temperature of the water? Calculate the heat energy released when 11.8 g of liquid mercury at 25.00 degree C is converted to solid mercury at its melting point.Explanation / Answer
1. M(s) + H2SO4(aq) ---> MSO4(aq) + H2(g)
No of mol of H2 = PV/RT = (756/760)*(0.215) / (0.0821*298)
= 0.00874 mol
No of mol of M = 0.00874 mol
Molarmass of M = 0.554/0.00874 = 63.4 g/mol
2. q required = m*s*DT + n*DHfus + m*s*DT + n*DHvap + m*s*DT
= 83*2.087*(0+10)+83*(333.6) + 83*4.184*(100-0)+(83/18)*(40.7*10^3)+83*2.01*(175-100)
= 264.332 kj/mol
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