balance the reactions x x He → d. SO2(g) + O2(g) → s0(8) Part 2 (1.3...
06 Question (1 point) Balance the following reactions that occur among volcanic gases. Part 1 (0.3 point) X X. He → o. SO2(g) + O2(g) → Soz(8) Part 2 (0.3 point) x x. He → o. HS(g) + O2(g) → SO2(g) + H20(3) Part 3 (0.3 point) X X. He → o. H,S(g)+ S02(g) — Sg(s) + H2O(g)
balance the equations
He → 12 112s(g) + E1 2 H2O(g) 3 O SO2(g) + 02 (g) -→ 2 Part 3 (1 point) HS(g) + SO2(g) → S(s)+ H,0(8)
12. The equilibrium constant for the reaction: SO2(g) + O2(g)so,(g) is Kc # 1.3 x 10, What is the equilibrium constant for the reaction: 2S0,(g)O,(g)+ 2S02(g) 13. For the following reaction, Kc (@ 500 K) 1.0 x 10 2 SO-(g) + 02(g) 2 SO,(g). What is the value of Kp for this reaction at 500 K? (3 Pts.)
Given these equilibrium reactions: 1. % Sa(s) + 2O2te) <---------- → 2 SO2 Ka = 1.86 x 10105 2. 1/8 Ses) + 3/2 O2(e) <--------→ SO3(e) ka = 1.77 x 1053 Calculate the equilibrium constant ka for the reaction below, which is important in the formation of acid-rain air pollution. 2 SO2(g) + O2(g) ------ --→2 SO3(g) [SO] Klz- 30g] 7 [0]
Given the following reactions: 2 S (s) + 3 O2 (g) ⟶ 2 SO3 (g) ΔH1= LaTeX: -− 790 kJ S (s) + O2 (g) ⟶ SO2 (g) ΔH2= LaTeX: -−297 kJ What is the enthalpy change of the following reaction? 2 SO3 (g) ⟶ 2 SO2 (g) + O2 (g) ΔH3=?
plesae ASAP
The contact process for producing sulfuric acid is: Sg(s) + 8 O2(g) — 2 SO2(g) + O2(g) SO3(g) + H2O(l) 8 SO2(g) +2 SO3(g) H2SO4(aq) each step has a percent yield of 77.1%, how many grams of Sg are needed to produce 1.50 kg sulfuric acid? 637 g 1.07*10^3 g 378 9 2.25*10^3 g 0 212 g
Please give explanations
B 3) Given: H2S(g) + 02(g) - H20 (liq) + SO2(g) AH = -562.3 kJ 1/8 Sg(s) + O2(g) - SO2(g) AH° = -297.0 kJ H2(g)+102 - H20 (liq) AH -266.9 kJ Compute AHⓇ for H2(g) + 1/8 S8 (s) - H2S(g) in kJ. A) 20.5 kJ (B) 562.3 kJ C) 276.6 kJ D) 265.3 kJ E) -1.6 kJ
Balance the following equations (stoichiometric reactions):
C8H18 + 12.5 ( O2 + 3.76 N2 ) = CO2 + N2 + H2O
C12H26 + 18.5 ( O2 + 3.76 N2 ) = CO2 + N2 + H2O
C2H4 (OH)2 + O2 = CO2 + H2O
1. Balance the following equations (stoichiometrical reactions): a). C3H18 (8) + 12.5 (02 + 3.76 N2) (8) → CO2 (8) + N2 (9) + H2O (8). b). C12H26 (g) + 18.5 (02 +3.76 N2) (8) +...
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2. Balance the following chemical reactions: a. CO + O2 →CO b. KNO: →KNO2 + O2 C. 03 > d. Cr(OH)3 + HCIO. Cr(ClO4)3 + H20 From the reaction: B2H6 +0, HBO, + H2O a. What mass of O, will be needed to burn 36.1 g of BH6? b. How many moles of water are produced from 19.2 g of B2 H.?!
1).From the following enthalpy changes, S (s) +3/2 O2 (g) 2 SO2 (g) SO3 (g) O2 (g)2 SO3 (g) AH =-395.2 kJ AHo 198.2 kJ Calculate the value of AHo for the reaction by using Hess's law of Heat Summation S(s) O2 (g) SO2 (g) 2) Oxyacetylene torches are fueled by the combustion of acetylene, C2H2. 4 CO2 (g) +2 H20 (g) 2 C2H2 + 5 O2 (g) If the enthalpy change for the reaction is -2511.14 kJ/mol, a) How...