
QUESTION 8 The density of a gas is 1.2 g/L at STP. What is its molar...
QUESTION 3 What volume of 2 M HCl is required to prepare 150 mL of 0.2 M HCl? a. 0.015mL b. 30 ml c. 15 ml O d. 1.09 x 103 ml 04.1.5 103 mL QUESTION 4 What is the oxidation half-reaction for the reaction of zinc with hydrochloric acid? Zn(s) + 2H+ (aq) + 2C1"(aq) -- Zn2+ (aq) + 2Cl(aq) + H2(g) a. 2H +(aq) + 2e (aq) → H2(g) + 2C1_(aq) b.2H +(aq) + 2e - → H2(g)...
Calculate and use the molar volume of a gas under ndard temperature and pressure conditions Question The Periodic Table of Elements He Rn Fr Ho Er Tm Md No Zinc will react with hydrochloric acid to produce hydrogen gas. Zn(s)+2 HCl(aq) ZnCl2(aq)H2 (g) What is the volume of H2 gas produced if 2.00 g of zinc is used with an excess of hydrochloric acid in the reaction above at STP? Round to 3 significant figures. Provide your answer below: Oal-...
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Determine the voltage (V) of the following cell at 25°C: Zn(s) | Zn2+(aq, 0.37 M) || Cl-laq, 0.75 M) C12(g, 0.750 atm)| Pt Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Hg2Cl2(s) + 2e --> 2Hg(l) + 2Cl(aq); E° = +0.27 V AgCl(s) + e --> Ag(s) + Cl (aq); E° = +0.22 V Ni2+(aq) + 2e --> Ni(s); E° =...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
The zinc within a copper-plated penny will dissolve in hydrochloric acid if the copper coating is filed down in several spots (so that the hydrochloric acid can get to the zinc). The reaction between the acid and the zinc is 2H+(aq)+Zn(s)→H2(g)+Zn2+(aq)2H+(aq)+Zn(s)→H2(g)+Zn2+(aq). When the zinc in a certain penny dissolves, the total volume of gas collected over water at 25 ∘C∘C was 0.961 L L at a total pressure of 0.995 bar bar . What mass of hydrogen gas was collected? The vapour...
The density of a gas is 1.25 g/L at STP. What is its molar mass? A) 22.4 g/mol B) 17.9 g/mol C) 28.0 g/mol D) 37.6 g/mol E) 41.6 g/mol please show work
The density of a gas is 0.803 g/L at STP. What is its molar mass? PICK ONE A 22.4 g/mol B 27.9 g/mol C 18.0 g/mol D 24.1 g/mol E 26.7 g/mol
If the density of an unknown gas is 1.95 g/L at STP what is the molar mass of the gas? (R = 0.0821 atmL/molek) A) 11.4 g/mol B) 22.4 g/mol C) 23.8 g/mol D) 43.7 g/mol E) 139 g/mol
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
7) At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) → 키.4x10-7. Calculate AG)for this reaction at 1500°C A) 105 kJ/mol B)-105 kJmol C)1.07 kJ/molD) CH,011(g) has the value K, D)255 8) Determine the equilibriurn constant K, at 25°C for the reaction Nag) + 3H2(g) → 2NHO 3 kJ/mol A) 1.52 x 106 B) 6.60 x 10 9) Predict the sign of AS for the reaction 02(g) → 20(g). C) 828 x 10D) 2.60 A) Negative B) zero...