Enter your answer in the provided box. Calculate the work done (in joules) when 50.6 g of tin dissolves in excess acid...
Calculate the work done (in joules) when 58.3 g of tin dissolves in excess acid at 1.07 atm and 28 ° C. Assume ideal gas behavior. Sn(s) + 2H+(aq) → Sn2+(aq) + H2(g)
Calculate the work done (in Joules) when 43.3 g of Tin dissolves in excess acid at 1.05 atm and 23 degree Celsius. Assume ideal gas behavior. Sn(s) + 2H+ (aq) -> Sn2+(aq) + H2 (g)
calculate the work done when 50.0g of tin dissolves in excess acid at 1.00 am and 25defree celcous
Enter your answer in the provided box. Consider the reaction 2Na(s) + 2H2O(1) 2NaOH(aq) + H2) When 2 moles of Na react with water at 25°C and 1 atm, the volume of H2 formed is 24.5 L. Calculate the magnitude of work done in joules when 0.25 g of Na reacts with water under the same conditions. (The conversion factor is 1 L atm = 101.3 J.) J
Calculate the work in Joules if 0.25 moles of Mg metal react with excess hydrochloric acid solution at 13.0°C and 1.00 atm (assume all gases behave ideally) Mg(s) + 2HCl(aq.) + MgCl2(aq.) + H2(e) A.- 450J B. - 594 J C.-750) D. - 500 J
Calculate the work in Joules if 0.5 moles of Al metal reacts with excess hydrochloric acid solution at 25 °C and 1 atm (assume all gases behave ideally): 2Al(s) + 6HCl(aq) + 2AlCl3(aq) +3H2(g) A. 1858.1) B. - 1238.7) C.-1858.1) D.1238.7)
Enter your answer in the provided box. A 5.70 g sample of a salt dissolves in 9.60 g of water to give a saturated solution at 26°C. What is the solubility (in g salt/100 g of H20) of the salt? g salt/100 g
Enter your answer in the provided box. Calculate the vapor pressure of a solution of 43.5 g of glycerol (C3H803) in 500.0 g of water at 25°C. The vapor pressure of water at 25°C is 23.76 torr. (Assume ideal behavior.) I torr
3 attempts left Check my work Enter your answer in the provided box. Calculate the density of helium in a helium balloon at 24.7°C. (Assume that the pressure inside the balloon is 1.01 atm.) g/ml
Enter your answer in the provided box. Consider the reaction H2(g) + Cl2(g) → 2HCl(g) ΔH =-184.6 kJ/mol If 5.0 moles of H2 reacts with 5.0 moles of C12 to form HC1 at 1.0 atm, what is Δ U for this reaction? Assume the reaction goes to completion and Δ V= 0 L (The conversion factor is 1 L·atm = 101.3 J.) kJ