2 K(s) + 2 H2O(l) → 2 KOH(aq) + H2(g) AH-393 kJ/molræn When 3.9 g of K(s) is added to 200. mL of water at 25°C in a calorimeter, all the K(s) reacts with the water as represented by the equation above. Which of the following is true about the pH of the water after the reaction is complete? (A) pH <7 B pH = 7 pH > 7 The pH of the water cannot be determined without additional information.

2 K(s) + 2 H2O(l) → 2 KOH(aq) + H2(g) AH-393 kJ/molræn When 3.9 g of K(s) is added to 200. mL of water at 25°C in a calorimeter, all the K(s) reacts with the water as represented by the equation above. Which of the following is true about the pH of the water after the reaction is complete? (A) pH <7 B pH = 7 pH > 7 The pH of the water cannot be determined without additional information.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A chemist measures the enthalpy change AH during the following reaction: 2 HNO3(1) + Mg(s)→Mg(NO3),(s) + H2(g) ДН--443. kJ '2 Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ x10 Mg(NO,), (s) + H, (8) → 2HNO,(1) + Mg(s) hno,() + Ma() -- Me(No,),C) + H, G) 1 - Mg(s) 2 Mg(NO,) (s) + ,H, (g) kJ 3. 3 Mg(NO,), (s) + 3H, (g) - 6HNO, (1) + 3Mg(s) ||kJ
50.0 mL of 2.03 M NaOH(aq) is mixed with 50.0 mL of 2.20 M HCl in a Styrofoam calorimeter. Calculate the moles of NaOH(s) added to the calorimeter. The molar mass of NaOH is 40.00 g/mol, H2O is 18.016 g/mol, an HCl is 36.458 g/mol. Report your value to the correct number of significant figures.
6A + 2C 6D Determine the enthalpy(AH) in kJ of the above reaction using the reactions below: 6B -> 2C AH = 438.3 kJ A + B D AH =-133.1 kJ
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Consider the following thermochemical equations (Note: HA is a weak acid)H+(aq) + OH-(aq) → H2O(l) ΔH1HA(aq) → H+(aq) + A-(aq) ΔH2HA(aq) + OH-(aq) → A-(aq) + H2O(l) ΔH3Choose the equation that shows the correct relationship between their enthalpy changes. A.) ΔH1 = ΔH3 - ΔH2 B.) ΔH2 = ΔH1 + ΔH3
A chemist measures the enthalpy change AH during the following reaction: 2 Al(OH)3(s)→Al,03(s) + 3 H,0(1) AH=41. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ x10 2 Al,0, (s) + H,0(1) Al(OH), (s) kJ 3 3 Al, O, (s) + 3H,0(1) → 2A1(OH), (s) kJ 3 Al(OH), (s) → Al, 0, (s) + H,0() |kJ 3
2 (a) In this investigation, you will use a polystyrene-cup calorimter to determine the amount of heat released during acid-base neutralization reactions. Find information in your textbook, an encyclopedia, or a web site about calorimetry. Sketch the apparatus for a polystrene-cup calorimeter. (b) For more precise heat of reaction measurnments, chemists use a device called bomb calorimeter. How is a bomb calorimeter similar to and different from a polystyrene-cup calorimeter?
Use the standard enthalpy of formation data to find the ΔHo for the following reaction: Cr2O3 (s) + 3 CO (g) →→ 2 Cr (s) + 3 CO2 (g) Substance or Ion ΔHfo (kJ/mol) Cr (s) 0 Cr2+ (aq) -138.9 Cr3+ (aq) -1971 Cr2O3 (s) -1128.4 CrO42- (aq) -863.2 Cr2O72- (aq) -1461 C (graphite) 0 C (diamond) 1.896 C (g) 715.0 CO (g) -110.5 CO2 (g) -393.5 CO2 (aq) -412.9 CO32-(aq) -676.26 +846 kJ -846 kJ -279 kJ -1632 kJ +1632 kJ +279 kJ -2641 kJ