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need help with a chem problem QUESTION 2 Consider the following reactions. At constant pressure, in...
Consider each of the following systems at constant pressure. Mark each system where work is done by the surroundings on the system. (Select all that apply.) 1. CaCO3(s) → CaO(s) + CO2(g) 2. CO2(s) → CO2(g) 3. 2 SO2(g) + O2(g) → 2 SO3(g) 4. H2O(g) → H2O(l) 5. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)
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Predict if the following reactions are exothermic or endothermic a) 2 H2(g) + O2(g/> 2 H2O(g) ΔΗ -484 kJ b) 2 Al(s) + Fe2O3(s) → 2 Fe(s) + Al2O3(s)AH =-852 kJ c) 2 H2O(g) 2 H2(g) + O2(g)AH :484 kJ d) 2 NH3(g) → N2(g) + 3 H2(g)AH = 92.2 kJ e) H2O(g) H2O(l) ΔΗ--44 kJ
37. Which of the following equilibria would not be affected by pressure changes at constant temperature? a. CO2(g) + H2(g) = CO(g) + H2O(g) b.CO(g) + 302(g) =CO2(8) c. 2Hg(1) + O2(g) = 2HgO(s) d. 2H2(g) + O2(g) = 2H2O(1) e. CaCO3(s) CaO(s) + CO2(g)
Consider the reaction: H2(g) + (1/2)O2(g) -------> H2O(l) ΔH° = -286 kJ Which of the following is true? (Select all that apply) the reaction is endothermic heat is given off by the surroundings the reaction is exothermic heat is absorbed by the system the enthalpy of the products is less than the that of the reactants
For which of the following reactions is ?H?rxn equal to ?H?f of the product(s)? You do not need to look up any values to answer this question. Check all that apply. H2O2(g)?12O2(g)+H2O(g) Na(s)+12F2(l)?NaF(s) 2H2(g)+O2(g)?2H2O(g) 2Na(s)+F2(g)?2NaF(s) H2(g)+12O2(g)?H2O(g) Na(s)+12F2(g)?NaF(s)
At constant pressure for which of the reactions shown below should ΔH° be greater than ΔE° ? I. 2 SO2(g) + O2(g) → 2 SO3(g) II. C23H48(g) + 35 O2(g) → 23 CO2(g) + 24 H2O(l) III. H2(g) + Cl2(g) → 2 HCl(g) IV. N2O4(g) → 2 NO2(g)
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Chem. If an ideal gas has a pressure of 2.13 atm, a temperature of 309 K, and has a volume of 59.73 L, how many moles of gas are in the sample A 6.8 increased its volume to 34.4 L. What was the initial volume of the balloon? s mol sample of freon gas was placed in a balloon. Adding 3.50 mol of freon gas to the balloon A hot air balloon...
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Consider the following reaction at equilibrium. What effect will decreasing the temperature have on the system? CO2(g) + 2 H20(I) = CH4(g) + 2 - AH° - +890 kJ O2(g) No effect will be observed. The reaction will shift to the right in the direction of products. The equilibrium constant will increase. The reaction will shift to the left in the direction of reactants.
The enthalpy change, ΔH, for a reaction at constant pressure is defined as: ΔH = ΔE + PΔV. For which of the following reactions will ΔH be approximately equal to ΔE? Select all that apply. Group of answer choices 2 NO2(g) -> N2(g) + 2 O2(g) Ca(OH)2(aq) + H2SO4(aq) -> 2 H2O(l) + CaSO4(s) C(s) + O2(g) -> CO2(g) None of the above
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Problem 4 (1) Use first law to directly prove that work done by an ideal gas during an adiabatic process is CV (Ti -Tf), where T1 and Tf are the initial and final temperatures of the system. (2) Show that the heat transferred to an ideal gas system during an infinitesimal reversible process can be written as where c and ?,, are specific heat capacities under constant volume and pressure, respectively. Use this...