Q 14 please 11) Calculate the osmotic pressure associated with 90.0 g of an enzyme of molecular weight 98,000 g/mol |dissolved in 2700 mL of benzene at 30.0 °C.A) 5.99 torrB) 1.96 torr4C) 6.43 torrD) 2.48 torr12) The rate constant for the first order reaction A-- B+C is k-4.4 x 103 min¹ at 57 K. What is thehalf-life for this reaction at 57 K?A) 32 minC) 9.1 min.D) 1200 min13) Consider the following reaction:If the half-life for the reaction is 0.610 s, the rate constant is:2 N₂O(g) 2 NO(g) + O2(g); rate = k[N20]A) 1.14 s¹¹B) 0.69 ¹C) 0.86 s¹B) 16 min.D) 0.32 s¹14) The decomposition of N₂Os(g)-NO2(g) + NO(g) proceeds as a first order reaction with a half-life of30.0 seconds at a certain temperature. If the initial concentration [N2Oslo 0.600 M, what is theconcentration after 120 seconds?A) 0.038 MB) 0.100 MC) 0.400 MD) 0.013 M15) Which equation below best gives the concentration of N₂Os versus time in the previous question Q14?A) [N₂0s] =([N₂Oslo)/t12 B) [N₂0s]-[N₂O3]oekC) [N₂O₁]=kt D) 1/[N2Os] = 1/[N2Os]o + kt16) Given: N2(g) + 3 H₂(g) 2NH₂(g)At equilibrium at a certain temperature, the concentration of NH3(g), H₂(g) and N2(g) are 0.49 M, 1.61 M and0.14 M, respectively. Calculate the value of Ke for this reaction.A) 1.26B) 0.612D) 1.96C) 0.41117) Consider the following reaction: 4 PCI(g)- P4(g) + 6 Cl₂(g)If the initial concentration of PCI3(g) is 2.0 M, and "x" is the equilibrium concentration of P4(g), what is thecorrect equilibrium relation?A) Kc = 6x7B) Ke=6x7/(2.0-x)* C) Ke=x²/(2.0-x)*18) Consider the reaction represented by the equation: N₂(g) + 3H2(g) 2NH3(g) Calculate theD) Kc = (x)(6x)/(2.0-4x)"equilibrium pressures at a certain temperature: PNH₁-2.9 x 10 atm, PN2-89x10¹ atm, PH2-2.7x 10 atmA) 4.9 x10B) 2.9x10D) 7.8x104C) 6.3x1045519) Consider the reaction represented by the equation: Fe" (aq) + SCN (aq) →FeSCN²+ (aq)6.00 M Fe³+ (aq) and 10.0 M SCN (aq) are mixed at a certain temperature and at equilibriumthe concentration of FeSCN³+ (aq) is 3 M.A) 250x10¹B) 95 x10320) A particular vinegar solution has a H3O* concentrationA) 17.3B) 12.1C) 143x103D) 303 x10of 0.013 M. What is the pOH of the solution?D) 15.8C) 12.321) What is the pH of 42.0 M aqueous solution of NH3 (ammonia). It's Ks- 1.8 x 10³.A) 12.4B) 0.0104C) 0.77822) The OH concentration in a 0.089M of Ca(OH)2 solution isA) 0.178 MB) 0.108 MD) 1x 10-7 M23) A solution of 9.00 MHCHO2 is 0.77% ionized in water. Calculate the K. value for the acid (HCHO₂).A) 2.3x104B) 5.4x104C) 0.2x10³D) 0.2324) When a weak acid is titrated with a strong base, the pH at the equivalence point is ALWAYSA) 7B)7D)

Question

Q 14 please 11) Calculate the osmotic pressure associated with 90.0 g of an enzyme of molecular weight 98,000 g/mol |dissolved in 2700 mL of benzene at 30.0 °C.A) 5.99 torrB) 1.96 torr4C) 6.43 torrD) 2.48 torr12) The rate constant for the first order reaction A--> B+C is k-4.4 x 103 min¹ at 57 K. What is thehalf-life for this reaction at 57 K?A) 32 minC) 9.1 min.D) 1200 min13) Consider the following reaction:If the half-life for the reaction is 0.610 s, the rate constant is:2 N₂O(g) 2 NO(g) + O2(g); rate = k[N20]A) 1.14 s¹¹B) 0.69 ¹C) 0.86 s¹B) 16 min.D) 0.32 s¹14) The decomposition of N₂Os(g)-NO2(g) + NO(g) proceeds as a first order reaction with a half-life of30.0 seconds at a certain temperature. If the initial concentration [N2Oslo 0.600 M, what is theconcentration after 120 seconds?A) 0.038 MB) 0.100 MC) 0.400 MD) 0.013 M15) Which equation below best gives the concentration of N₂Os versus time in the previous question Q14?A) [N₂0s] =([N₂Oslo)/t12 B) [N₂0s]-[N₂O3]oekC) [N₂O₁]=kt D) 1/[N2Os] = 1/[N2Os]o + kt16) Given: N2(g) + 3 H₂(g) <-> 2NH₂(g)At equilibrium at a certain temperature, the concentration of NH3(g), H₂(g) and N2(g) are 0.49 M, 1.61 M and0.14 M, respectively. Calculate the value of Ke for this reaction.A) 1.26B) 0.612D) 1.96C) 0.41117) Consider the following reaction: 4 PCI(g)-> P4(g) + 6 Cl₂(g)If the initial concentration of PCI3(g) is 2.0 M, and "x" is the equilibrium concentration of P4(g), what is thecorrect equilibrium relation?A) Kc = 6x7B) Ke=6x7/(2.0-x)* C) Ke=x²/(2.0-x)*18) Consider the reaction represented by the equation: N₂(g) + 3H2(g) <-> 2NH3(g) Calculate theD) Kc = (x)(6x)/(2.0-4x)"equilibrium pressures at a certain temperature: PNH₁-2.9 x 10 atm, PN2-89x10¹ atm, PH2-2.7x 10 atmA) 4.9 x10B) 2.9x10D) 7.8x104C) 6.3x1045519) Consider the reaction represented by the equation: Fe" (aq) + SCN (aq) →FeSCN²+ (aq)6.00 M Fe³+ (aq) and 10.0 M SCN (aq) are mixed at a certain temperature and at equilibriumthe concentration of FeSCN³+ (aq) is 3 M.A) 250x10¹B) 95 x10320) A particular vinegar solution has a H3O* concentrationA) 17.3B) 12.1C) 143x103D) 303 x10of 0.013 M. What is the pOH of the solution?D) 15.8C) 12.321) What is the pH of 42.0 M aqueous solution of NH3 (ammonia). It's Ks- 1.8 x 10³.A) 12.4B) 0.0104C) 0.77822) The OH concentration in a 0.089M of Ca(OH)2 solution isA) 0.178 MB) 0.108 MD) 1x 10-7 M23) A solution of 9.00 MHCHO2 is 0.77% ionized in water. Calculate the K. value for the acid (HCHO₂).A) 2.3x104B) 5.4x104C) 0.2x10³D) 0.2324) When a weak acid is titrated with a strong base, the pH at the equivalence point is ALWAYSA) 7B)<7C) >7D) < 1C) 1.3x10-¹2 MD) 12.625) Which one of these statements about strong acid is trueA) Strong acid produce solutions with a higher pH than weak acidsB) All strong acids have H atom bonded to electronegative oxygen atomC) Strong acids are very concentrated acidsD) Strong acids are 100% ionized in water

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