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if the same amount of heat is added to 1.00 g of each
substances which substance...
Q 1. a. A process in which heat is given off is said to be _____________________...
Q 1. a. A process in which heat is given off is said to be _____________________ (endothermic or exothermic) b. DH is negative for an ___________________ (endothermic or exothermic) reaction c. If a reaction is carried out in solution, and the solution gets cooler as the reaction occurrs, the reaction must be ___________________ (endothermic or exothermic) d. A hot penny is dropped in water, and 25.2 J is tranferred from the penny to the water. q for the water =...
35. Consider the following specific heats of metals. Metal Specific Heat Copper 0.385 J/(g. °C) Cobalt0.418...
35. Consider the following specific heats of metals. Metal Specific Heat Copper 0.385 J/(g. °C) Cobalt0.418 J/(g °C) Chromium 0.447 J/(g. °C) Gold Silver0.237 J/(g. °C) 0.129 J/(g.°C) If the same amount of heat is added to 100-g samples of each of the metals, which are all at the same temperature, which metal will reach the lowest temperature? a. copper b. cobalt c chromium d. gold e. silver x 36. The sign of AH for the process 12(s)- 12(3) is...
B. Heat of Solution Solid unknown number Mass of water (Mw) Mass of solid (Ms) Original temperatu...
B. Heat of Solution Solid unknown number Mass of water (Mw) Mass of solid (Ms) Original temperature (T1) Final temperature (T2) 9 Show Calculations aw = Mw x (TI . T2) x (1.00 cal/goC) Qs = Ms x (Ti . T2) x (0.2 cal/goc). Q = Qw + Qs = heat flow into solution cal The quantity you have just calculated is approximately equal to the heat of solution, AH, of your sample. Note that if T1>T2. the reaction is...
When 0.0700 mol of a substance is added to 150.0 grams of an aqueous solution in...
When 0.0700 mol of a substance is added to 150.0 grams of an aqueous solution in a Styrofoam cup calorimeter, a chemical reaction occurs that causes the temperature of the solution to increase from 25.3 to 38.3 °C. Assume that the specific heat of the solution is 4.18 J/(g°C) and that the heat capacity of the calorimeter is negligible. Use this data to calculate the enthalpy change (in kJ/mol substance) for the chemical reaction +116 kJ/mol +3.80 kJ/mol -571 kJ/mol...
The table lists the specific heat capacities of select substances. Substance Specific heat capacity (J/g °C)...
The table lists the specific heat capacities of select substances. Substance Specific heat capacity (J/g °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 water 4.184 An unknown substance has a mass of 13.3 g. The temperature of the substance increases by 16.7 °C when 52.2 J of heat is added to the substance. What is the most likely identity of the substance? O lead O aluminum iron O copper water O silver
Fill in the Blanks Let's use calorimetry to measure heats of reaction. Suppose you mix 25.0...
Fill in the Blanks Let's use calorimetry to measure heats of reaction. Suppose you mix 25.0 mL of 0.08M cesium hydroxide with 25.0 mL of 0.08M hydrochloric acid. Assume both solutions are at 28.0°C. The temperature of the solution after the reaction is 30.2°C. Because the temperature of the solution went up, the reaction is (endothermic/exothermic). Now compute the heat of the reaction assuming the heat capacities of the solutions are equal to pure water (4.18 J/g°C). Report the Q...
A calorimeter contains 29.0 mL of water at 14.0 ∘C . When 1.30 g of X (a substance with a molar mass of 61.0 g/mol ) is...
A calorimeter contains 29.0 mL of water at 14.0 ∘C . When 1.30 g of X (a substance with a molar mass of 61.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 27.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...
Which of the following 10.0 gram substances will increase in temperature by the greatest amount when 100 J of hea...
Which of the following 10.0 gram substances will increase in temperature by the greatest amount when 100 J of heat is added to each? Substance D, specific heat 1.67 J/(g°C) Substance C, specific heat 1.22 J/(g°C) Substance A, specific heat 1.06 J/(g°C) Substance B, specific heat 0.892 J/(g°C) Given that the enthalpy of formation, AH, of gaseous nitrogen dioxide is +33.84 kJ/mol, what is the enthalpy change for the following reaction? 2NO2(g) N2(g)202(g) AH= ? -33.84 kJ +67,68 kJ -67.68...
Lab 14 Heat of Reaction Objective: To experimentally determine the heat of reaction for two exothermic...
Lab 14 Heat of Reaction Objective: To experimentally determine the heat of reaction for two exothermic reactions. Consider the following equations. (1) Mg(s) + 2HCI → MgCl2(aq) + H2(g) Hz(8) AH = ? (2) MgO(s) + 2HCl(aq) → MgCl(aq) + HOH (1) AH2 = ? The reactions represented by equations (1) and (2) will be our experimental work for today. Background: The heat given off or gained in a reaction is commonly called the heat of reaction. A reaction that...
disregard the answers I put. please answer all parts of the question. 3. In Part A...
disregard the answers I put. please answer all parts of the
question.
3. In Part A you dissolved CaCl2 in water. a. What happened to the temperature? Here we wten we added cache b. That means the calorimeter (circle one) ABSORBED/RELEASED heat. C. As a result, the reaction dissolving the CaCl2 (circle one) ABSORBED RELEASED heat. d. That means that dissolving CaCl2 is (circle one) ENDOTHERMIC/EXOTHERMIC, and e. AH for dissolving CaCl2 will be (circle one) POSITIVE/NEGATIVE. nplete the following...
35. Consider the following specific heats of metals. Metal Specific Heat Copper 0.385 J/(g. °C) Cobalt0.418 J/(g °C) Chromium 0.447 J/(g. °C) Gold Silver0.237 J/(g. °C) 0.129 J/(g.°C) If the same amount of heat is added to 100-g samples of each of the metals, which are all at the same temperature, which metal will reach the lowest temperature? a. copper b. cobalt c chromium d. gold e. silver x 36. The sign of AH for the process 12(s)- 12(3) is...
B. Heat of Solution Solid unknown number Mass of water (Mw) Mass of solid (Ms) Original temperature (T1) Final temperature (T2) 9 Show Calculations aw = Mw x (TI . T2) x (1.00 cal/goC) Qs = Ms x (Ti . T2) x (0.2 cal/goc). Q = Qw + Qs = heat flow into solution cal The quantity you have just calculated is approximately equal to the heat of solution, AH, of your sample. Note that if T1>T2. the reaction is...
When 0.0700 mol of a substance is added to 150.0 grams of an aqueous solution in a Styrofoam cup calorimeter, a chemical reaction occurs that causes the temperature of the solution to increase from 25.3 to 38.3 °C. Assume that the specific heat of the solution is 4.18 J/(g°C) and that the heat capacity of the calorimeter is negligible. Use this data to calculate the enthalpy change (in kJ/mol substance) for the chemical reaction +116 kJ/mol +3.80 kJ/mol -571 kJ/mol...
The table lists the specific heat capacities of select substances. Substance Specific heat capacity (J/g °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 water 4.184 An unknown substance has a mass of 13.3 g. The temperature of the substance increases by 16.7 °C when 52.2 J of heat is added to the substance. What is the most likely identity of the substance? O lead O aluminum iron O copper water O silver
Fill in the Blanks Let's use calorimetry to measure heats of reaction. Suppose you mix 25.0 mL of 0.08M cesium hydroxide with 25.0 mL of 0.08M hydrochloric acid. Assume both solutions are at 28.0°C. The temperature of the solution after the reaction is 30.2°C. Because the temperature of the solution went up, the reaction is (endothermic/exothermic). Now compute the heat of the reaction assuming the heat capacities of the solutions are equal to pure water (4.18 J/g°C). Report the Q...
Which of the following 10.0 gram substances will increase in temperature by the greatest amount when 100 J of heat is added to each? Substance D, specific heat 1.67 J/(g°C) Substance C, specific heat 1.22 J/(g°C) Substance A, specific heat 1.06 J/(g°C) Substance B, specific heat 0.892 J/(g°C) Given that the enthalpy of formation, AH, of gaseous nitrogen dioxide is +33.84 kJ/mol, what is the enthalpy change for the following reaction? 2NO2(g) N2(g)202(g) AH= ? -33.84 kJ +67,68 kJ -67.68...
Lab 14 Heat of Reaction Objective: To experimentally determine the heat of reaction for two exothermic reactions. Consider the following equations. (1) Mg(s) + 2HCI → MgCl2(aq) + H2(g) Hz(8) AH = ? (2) MgO(s) + 2HCl(aq) → MgCl(aq) + HOH (1) AH2 = ? The reactions represented by equations (1) and (2) will be our experimental work for today. Background: The heat given off or gained in a reaction is commonly called the heat of reaction. A reaction that...
disregard the answers I put. please answer all parts of the
question.
3. In Part A you dissolved CaCl2 in water. a. What happened to the temperature? Here we wten we added cache b. That means the calorimeter (circle one) ABSORBED/RELEASED heat. C. As a result, the reaction dissolving the CaCl2 (circle one) ABSORBED RELEASED heat. d. That means that dissolving CaCl2 is (circle one) ENDOTHERMIC/EXOTHERMIC, and e. AH for dissolving CaCl2 will be (circle one) POSITIVE/NEGATIVE. nplete the following...
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