for the reaction
S(s)+O2(g)=SO2(g)
delta H=-296 kJ per mole of SO2 formed
calculate the quantity of heat released when 2.78g of sulfur is burned in oxygen=
for the reaction S(s)+O2(g)=SO2(g) delta H=-296 kJ per mole of SO2 formed calculate the quantity of...
For the reaction below ΔH = -296 kJ per mole of SO2 formed. S(s) + O2(g) → SO2(g) (a) Calculate the quantity of heat released when 1.05 g of sulfur is burned in oxygen. (b) Calculate the quantity of heat released when 0.584 mol of sulfur is burned in air. (c) What quantity of energy is required to break up exactly 9 mol of SO2(g) into its constituent elements?
Consider the reaction B2H6(g)+O2(g)=B2O3(s)+3H2O(g) delta heat -2035 kJ/mol calculate the amount of heat released when 24.8g of diaborane is burned heat released=
Consider the reaction B_2H_6(g) + 3 O_2(g) rightarrow B_2O_3(s) + 3 H_2O(g) Delta H= -2035 kJ/mol Calculate the amount of heat released when 54.4 g of diborane is burned, heat released = kJ
Calculate heat for the following reaction to produce sulfur dioxide, S(3) + O2(g) = SO2(E) given the thermochemical equations below. 2 S(s) + 3 O2(g) =2 SO3(g) AH° = -791.5 kJ 2 SO2(g) + O2(g) = 2 SO3(g) AH° = -197 9 kJ Show all work and calculate to the correct number of sig figs.
Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO2(g), by the reaction 2 502(g) + O2(g) → 250 (8) The standard enthalpies of formation for SO2(g) and SO2(g) are AH; (SO2(8)) = –296.8 kJ/mol AH (SO2(2)) = –395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 4.46 L of So,(g) is converted to 4.46 L of So, (g) according to this process at a constant pressure and...
A) For the reaction 4HCl(g) + O2(g)---->2H2O(g) + 2Cl2(g) Delta H° = -114.4 kJ and Delta S° = -128.9 J/K The equilibrium constant for this reaction at 306.0 K is _______? Assume that Delta H° and DeltaS° are independent of temperature. B) For the reaction N2(g) + 3H2(g)---->2NH3(g) Delta H° = -92.2 kJ and Delta S° = -198.7 J/K The equilibrium constant for this reaction at 333.0 K is ___? Assume that Delta H° and Delta S° are independent of...
Consider the following data. Mg(s) + S(s) MgS(s) H = -598.0 kJ SO2(g) S(s) + O2(g) H = +296.8 kJ MgS(s) + 2 MgO(s) 3 Mg(s) + SO2(g) H = +1504.6 kJ Use Hess's law to calculate H for the reaction below. 2 Mg(s) + O2(g) 2 MgO(s)
calculate delta H for the reaction 4Cu(s)+O2(g)=2Cu2O(s) given the following hypothetical data 2Cu(s)+O2(g)=2CuO(s) delta H=-312 kJ 2Cu2OtO2(g)=4CuO(s) delta H=-340kJ deltaH=
help The value of H° for the reaction below is -1107 kJ: 2Ba (s) + O2 (g) 2BaO (s) How many kJ of heat are released when 5.75 g of Ba (s) reacts completely with oxygen to form BaO (s)? 23.2 kJ 26.3 kJ 96.3 kJ 46.4 kJ 193 kJ
34. At volcanic sites, sulfur is formed via the following reaction. 2 H2S(g) +SO2(g) = 3S(s) +2 H20(g) a. Calculate the equilibrium constant, K, for this reaction at 25°C. 4 Gº (kJ/mol H2S (8) SO2) H20 (8) -33.0 -300.4 -228.6 s, b. Predict whether sulfur formation becomes more or less favorable as temperature increases. Explain. C Sulfur dioxide is a pollutant released by power plants. Would this reaction be suitable for removing SO2 from power plant waste?