How do temperature changes lead to solubility changes for salt dissolved in water? High temperatures mean more of the salt will be decreasing solubility. the gas form, causing it to evaporate out of the solution, O High temperatures mean more of the salt will be in the liquid form as it gradually melts, increasing solubility High temperatures mean that sodium and chlorine ions will be moving faster, increasing the odds that they will collide and combine. This reduces solubility. High temperatures mean more kinetic energy, which keeps sodium and chlorine ions from combining, which increases solubility.

How do temperature changes lead to solubility changes for salt dissolved in water? High temperatures mean more of the salt will be decreasing solubility. the gas form, causing it to evaporate out of the solution, O High temperatures mean more of the salt will be in the liquid form as it gradually melts, increasing solubility High temperatures mean that sodium and chlorine ions will be moving faster, increasing the odds that they will collide and combine. This reduces solubility. High temperatures mean more kinetic energy, which keeps sodium and chlorine ions from combining, which increases solubility.

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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Suppose a 500. mL flask is filled with 0.60 mol of CO, 0.30 mol of NO and 1.7 mol of CO,. The following reaction becomes possible: NO,(g) +cO(g) - NO(g) +CO, (g) The equilibrium constant K for this reaction is 0.953 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. ?
Suppose a 250. mL flask is filled with 1.8 mol of H,O, 2.0 mol of CO, and 1.6 mol of H,. The following reaction becomes possible: CO (g) + H,0(g) - CO,(g)+H,(g) The equilibrium constant K for this reaction is 5.86 at the temperature of the flask. Calculate the equilibrium molarity of CO,. Round your answer to two decimal places. OM
Suppose a 500. mL flask is filled with 0.60 mol of NO, 0.90 mol of NO and 0.50 mol of CO,. The following reaction becomes possible: NO, (s) + CO(s) - NO () +co,(e) The equlibrium constant K for this reaction is 0.930 at the temperature of the flask. Calculate the equilibrium molarity of NO,. Round your answer to two decimal places.
While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 75 L tank with 10. mol of ethylene gas and 5.4 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.8 mol of ethylene gas and 2.2 mol of water vapor. The engineer then adds another 1.4 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. |mol x10 O
Suppose a 250. mL flask is filled with 0.70 mol of NO,, 0.40 mol of CO and 2.0 mol of CO ,. The following reaction becomes possible: NO,(3) + CO (g) - No(g)+ CO,(g) The equilibrium constant K for this reaction is 1.04 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 0.30 mol of Cl, and 0.70 mol of HCl. The following reaction becomes possible: H, (g) + Cl, (g)- 2HC1(g) The equilibrium constant K for this reaction is 0.836 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places.
For the reaction... N2 (g) + 3 H2 (g) <−> 2 NH3 (g) If the pressure in the system is increased, which substance will increase in concentration?
Suppose a 250. mL flask is filled with 2.0 mol of NO,, 1.4 mol of CO and 0.40 mol of CO,, The following reaction becomes possible: NO,(g) +CO(g)-NO(g) + CO,(s) The equilibrium constant K for this reaction is 0.676 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 1.8 mol of CO, 1.9 mol of H,0 and 1.6 mol of H,. The following reaction becomes possible: co (g) +H,0(g)– CO,(g) +H2 (g) The equilibrium constant K for this reaction is 0.275 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 0.90 mol of H,O, 1.2 mol of CO, and 1.5 mol of H,. The following reaction becomes possible: CO (g)+ H,O(g)=CO,(g)+H,(g) The equilibrium constant K for this reaction is 5.65 at the temperature of the flask. Calculate the equilibrium molarity of CO,. Round your answer to two decimal places. 2' OM
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 25 L tank with 3.8 mol of carbon monoxide gas and 7.6 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 1.7 mol of carbon monoxide gas, 5.5 mol of water vapor and 2.1 mol of carbon dioxide. The engineer then adds another 1.0 mol of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the moles of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. || mol x10
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