Base your answers to questions 59 through 60 on the information below and on your knowledge of chemistry. At 1023 K and I atm, a 3.00-gram sample of SnO2(s) (gram-formula mass = 151 g/mol) reacts with hydrogen gas to produce tin and water, as shown in the balanced equation below. SnO2(s) + 2H2(g) ==>Sn(L) + 2H2O(g) 59 Show a numerical setu for calculating the number of moles of Sn02(s) in the 3.00-gram sample. [I] Answer--> ( 3.00g)/(151g/mol) no units needed for credit |
60 Determine the number of moles of Sn(L) produced when 4.0 moles of H2(g) is completely consumed. [1] on to Questions 61-62 |