show the calculation of the amount of heat involved if 35.6 g of H2S is reacted with excess of O2 to yield sulfur trioxide and water by the following reaction. Report your answer to 4 significant figures
show the calculation of the amount of heat involved if 35.6 g of H2S is reacted...
Hydrogen sulfide (H2S)reacts with oxygen (O2) to produce sulfur dioxide (SO2) and water. How many grams ofSO2will be produced if 100 g of H2Swas reacted with 100 g ofO2? (restrict your answer to 4 significant figures) Type your response
Reaction of aluminum sulfide with water provides aluminum hydroxide and H2S(g). If 20.00 g of aluminum sulfide is combined with 2.00 mL of water (d = 1.000 g/mL), what amount remains of the reagent present in excess? Report your answer to the appropriate number of significant figures. g
Sulfur trioxide is made from the oxidation of sulfur dioxide. 2 SO2 + O2 --> 2 SO3. A 16 g sample of SO2, reacted with excess oxygen, gives 18 g SO3. What is the percent yield?
Consider the reaction 8H2S(g)+4O2(g)→8H2O(g)+S8(g)8H2S(g)+4O2(g)→8H2O(g)+S8(g) Δ[H2S]/ΔtΔ[H2S]/Δt = -0.022 M/sM/s You may want to reference (Pages 587 - 592) Section 14.3 while completing this problem. Part A Find Δ[O2]/ΔtΔ[O2]/Δt. Express your answer to two significant figures and include the appropriate units. Part B Find Δ[H2O]/ΔtΔ[H2O]/Δt. Express your answer to two significant figures and include the appropriate units. Part C Find Δ[S8]/ΔtΔ[S8]/Δt. Express your answer to two significant figures and include the appropriate units. Part D Find the rate of the reaction. Express...
HQ11.44 Homework. Unanswered Using the first equation in HQ11.43, how much heat will be generated if 10.0 g of Hy is reacted with excess O2? Report the answer in kJ and it should be a positive number. Report the answer to four significant figures. Numeric Answer:
Determine the amount of heat involved in a chemical change using. Hess's Law Question 2C(s) + 0,(g) + 2 CO(g) AH = -222 kJ 2 H, (g) + O2(g) + 2H2O(g) AH = -484 kJ H,0(1) H2O(g) AH = +44 kJ Use the thermochemical data above to calculate the change in enthalpy for the reaction below. H,0(1) + C(s) + CO(g) +H, () . Your answer should have three significant figures. Provide your answer below: Activity Details You have viewed...
Show the calculation of the number of moles in the given amount of the following 2 substances. Report your answer to 3 significant figures. 12.0 grams of Ca3(PO4)2
Measuring Heat of Reaction Problems 5. A sample of ethanol (C2H5OH), weighing 6.83 g underwent combustion in a bomb calorimeter by the following reaction: 02 (g) 2 CO2 (g)3 H2O () C2H5OH ()3 If the heat capacity of the calorimeter and contents was 18.1 kJ/°C and the temperature of the calorimeter rose from 25.50 to 36.73, (1) what is the AH of the reaction? Using the definitions at the beginning of the module describe (2) the calorimeter + contents, (3)...
can you please answer all of the parts
d slf Section B: Show all your calculation steps with conversion factors formula of reactants and products, setup with units, calculator value and correct significant figures. Calculation of molar mass should be shown when needed. All atomic mass of elements are up to two decimals as given in the periodic table. Following Reaction is given when zinc reacts with sulfur to form ZnS. 1 Zn (s)+ S(s) ZnS Determine the limiting reactant...
Sulfur dioxide and oxygen react to form sulfur trioxide, like
this: 2SO2(g)+O2(g)→2SO3(g)
Also, a chemist finds that at a certain temperature the
equilibrium mixture of sulfur dioxide, oxygen, and sulfur trioxide
has the following composition:
Calculate the value of the equilibrium constant Kp for this
reaction. Round your answer to 2 significant digits.
compound pressure at equilibrium SO2 58.3 atm 02 84.7 atm SO3 66.3 atm