what mass of water (in grams) is necessary to convert 225 g SiF4 to SiO2? SiF4 + 2 H2O → 4HF + SIO2
Calculate delta H rxn for each of the following: (a) SiO2(s) + 4HF(g) > SiF4(g) + 2H2O(l) (b) C2H6(g) + O2(g) > CO2(g) + H2O(g) [unbalanced] 6.54 Calculate AHºrxn for each of the following: (a) SiO2(s) + 4HF(g) → SiF4(g) + 2H20(1) (b) CH6(g) + O2(g) → CO2(g) + H2O(g) [unbalanced]
Consider the following: SiF4 (g) + 2H2O (g) < ---> SiO2 (s) + 4HF (g) Kp=7.44 x 10-3 at 2000 K a) Write the equilibrium expression b) Calculate Kc for the above reaction. Will the reaction go to the right, the left, or is it at equilibrium under the following initial conditions? [HF] = 0.100M Given the above information, calculate the value of Kp for the following reaction at 2000 K: 1/2 SiO2 (s) + 2HF (g) <- ->...
Hess's Law Practice Find AH° for the following equation: SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(g) Using the following equations: Si(s) + O2(g) → SiO2(s) Si(s) + 2F2(g) → SiF4(g) H2(g) + F2(g) → 2HF(g) H2(g) + 4202(g) → H2O(g) AH = -910.9 kJ/mol rxn AH = -1651 kJ/mol rxn AH = -542 kJ/mol rxn AH = -241.8 kJ/mol rxn
1. What is the theoretical yield in grams of SiF4 (104.08 g/mol) if 37.1 g of SiO2 (60.08 g/mol) are allowed to react with 106.9 g of hydrogen fluoride? SiO2 + 4HF---> SiF4 + 2H2O 2. What is the theoretical yield in grams of Fe2O3 if 54.9 g of iron are allowed to react with 13.5 g of molecular oxygen? 4Fe + 3O2 ---> 2 Fe2O3
654 Calculate ΔΗ'm for each of the following: (a) SiO2(s)+4HF(g) -SiF4(g) + 2H:O() (b) CHo(8)+0(g) CO2(g)+H20(g) (unbalanced]
Determine which of the following chemical equations are correctly balanced. Fe2O3(s)+CO(g)→2Fe(s)+CO2(g) Al2S3(s)+H2O(l)→2Al(OH)3(s)+3H2S(g) 2Cr(s)+3O2(g)→Cr2O3(s) SiO2(s)+4HF(aq)→SiF4(g)+2H2O(l)
Hydrofluoric acid dissolves glass by reacting with silica as shown in this balanced chemical equation. SiO2 + 4 HF → SiF4 + 2 H2O If 15.75 g SiO2 (molar mass = 60.08 g/mol) and 18.25 g HF (molar mass = 20.01 g/mol) are combined, how many grams of SiF4 (molar mass = 104.1 g/mol) could be produced? How many grams of SiO2 AND how many grams of HF will remain when the reaction is complete? If 16.39 g SiF4 were...
According to the following thermochemical equation, what mass of H2O (in g) must form in order to produce 975 kJ of energy? SiO2(s) + 4 HF(g) → SiF4(g) + 2 H2O(l) ΔH°rxn = -184 kJ 54.1 g 95.5 g 102 g 68.0 g 191 g
Consider the unbalanced chemical equation below. CaSiO3(-) + HF (@)-CaF2(aq) + SiF4(g) + H2O(1) Suppose a 34.3 g sample of CaSiO3 is reacted with 31.3 L of HF at 27.0 °C and 1,00 atm. Assuming the reaction goes to completion calculate the mass (in grams) of the SiF4 and H2O produced in the reaction. mass SiF4 = mass H2O Submit Hide Hints
Question 1. Consider the reaction SiC14(g) + 2H2O(g) → SiO2(g) + 4 HCl(g) You may need the data below. Compound AHac(kJ/mal) SiCl4(g) SiF4(g) H2O(g) SiQ2(s) HCl(9) -1599.3 -2386.5 -926.3 -1864.9 -431.6 a) Find enthalpy of reaction AH for this reaction. [3 Marks] b) How do the strengths of the bonds in the products compare to those of the reactants? Explain your answer. [2 marks] c) How would you expect AH for the above reaction to compare to AH for the...