When 0.2235g of strontium reacted with 25.00ml of 1.168 m hcl, 63.18g

When 0.2235g of strontium reacted with 25.00mL of 1.168 M HCl, 63.18g of H20 (water) was displaced by the H2 gas produced. The temperature in the reaction flask was 27.0 degrees C and the barometric pressure was 777 Torr. The molar mass of strontium is 87.62g/mol. At 27.0 degrees C the vapor pressure of water is 27.0 Torr and its density is 0.9965g/mL. When the final reaction mixture was titrated with 0.6137M NaOH, the endpoint was reached when 39.25mL of base were added. 

a. From the volume of water displaced, calculate the volume of gas collected during the reaction. Recall that v=m/d 

b. Calculate the number of moles of gas collected during the reaction. Recall that PV = nRT and R = 8.21×10^-2. 

c. Calculate the number of moles of HCl used as a reactant. 

d. Calculate the number of moles or unreacted HCl left in the reaction mixture. 

e. Calculate the number of moles of HCl that reacted with the strontium. 

f. Calculate the number of moles of strontium used as a reactant. 

g. Calculate the ratio of the number of moles of HCl that reacted witht the strontium to the number of moles of strontium used. 

 

h. Calculate the ration of the number of moles of gas collected to the number of moles of strontium used.