After transfer of 1.50 kJ of thermal energy to a 0.499-kg block of copper the temperature is 47.0 °C. The specific heat capacity of copper is 0.385 Jg-1 °C-1. Calculate the initial temperature of the copper.

The table provides molar heat capacities (Cm) of selected metals with the units of joules per mole-kelvin. Heat capacity is also frequently given as specific heat capacity (C₂) with the units joules per gram-degree Celsius. Using the values provided in the table, convert the molar heat capacity (Cm) of zinc to the specific heat capacity (C₂) of zinc. C₁ = J/(g. °C) Molar heat capacity (Cm) of selected metals at 25 °C Element aluminum copper iron lead magnesium nickel titanium zinc Cm (J/(mol-K)) 24.20 24.44 25.10 26.84 24.87 26.07 25.06 25.39

Calcium acetate, Ca(CH3COO)2 has a molar mass of 158.17 g/mol. In a constant pressure calorimeter, 44.2 g of Ca(CH3COO)2 is dissolved in 861g of water at 25.00 °C. The heat produced by the solution was determined to be 15kJ. What is the final temperature of the solution? q= - msAT SH20 = 4.184 29.0 °C O 18.4 °C O 64.6 °C O 33.8 °C O 3.96 °C O 21.0 °C

A 100.0-mL sample of 1.0 M NaOH is mixed with 50.0 mL of 1.0 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which a calibrated thermometer passes. The temperature of both solutions before mixing is 22.3 °C. After the NaOH solution is added to the coffee cup and the mixed solutions are stirred with the thermometer, the maximum temperature measured is 31.4 °C. Assume that the density of the mixed solution is 1.00 g/mL, the specific heat of the mixed solutions is 4.18 J/g•°C, and no heat is lost to the surroundings.(a) Write a balanced chemical equation for the reaction that takes place.(b) Is there any unreacted NaOH or H2SO4 remaining after the reaction?(c) Calculate the enthalpy change per mole of H2SO4 in the reaction.

A 110.2 mL sample of 1.00 M NaOH is mixed with 55.1  mL of 1.00 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 21.85 °C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 31.30 °C. Assume that the density of the mixed solutions is 1.00 g/mL, that the specific heat of the mixed solutions is 4.18 J/(g·°C), and that no heat is lost to the surroundings.   a. Write a balanced chemical equation for the reaction that takes place in the Styrofoam cup. Remember to include phases in the balanced chemical equation.   b. Is any NaOH or H2SO4 left in the Styrofoam cup when the reaction is over?A.   No B.   Yes  c. Calculate the enthalpy change per mole of H2SO4 in the reaction.     kJ/mol

In this experiment you will place a sample of your salt in water in a constant pressure calorimeter with a heat capacity of 29.4 J/℃. You will determine the enthalpy change for the dissociation of your salt, delta Hdiss or rxn.  A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃ and the final temperature was 27.086365℃. What is the total mass of the solution in sig figs?    mass  = 4.368 g + 35.5 g = 39.868 g   a. 39.8 g b. 40 g c. 39 g d. 39.868 g e. 4.0 x 10^1 g f. 39.87 g g. 39.86 g h. 39.9 g i. none of these

Use the thermochemical equations shown below to determine the enthalpy for the reaction: C3H8(g) + 502(g) +3CO 2 + 4H2O(1) CO2 C(graphite) + 02 HE = 221.6KJ H2(g) + 1/2O2(g) H2O(1) HE= -160.3KJ 3 C(graphite) + 4 H2(g) C3H8(g) HE= -58.5KJ

CH,,0, (s) + 60, (g) → 6CO, (g) + 6H,0(g) 12 The combustion of glucose was performed in a bomb calorimeter. Qwater= 14.52kJ. The heat capacity of the bomb is Ca = 2.273 kJ/C and the change in temperature was 28.49C. If 0.03255 moles of glucose was used in the bomb calorimeter, then what is AHmy in kJ/mol? a. ´cal rnx

The reaction between hydrogen and oxygen to yield water vapor has AH" = -1843 2H₂(g) + O₂(g) 2H₂O(g)AH <=-484kJ Part A What is the enthalpy change in kilojoules when 0.70 mol of H₂ reacts with 0.35 mol of O, to produce 0.70 mol of H₂ at constant pressure of 1.00 atm? Express your answer as a whole number. AH = Submit Part B W= Submit 1957 ΑΣΦ How much PV work is done in kilojoules for this reaction at constant pressure of 1.00 atm if the volume change is-9-2 L? Express your answer using two significant figures. 100 ΑΣΦΑ Part C Request Answer Request Answer kJ What is the value of AE for this reaction in kilojoules?

The standard heat of formation, AH;, is defined as the enthalpy change for the formation of one mole of Part B substance from its constituent elements in their standard states. Thus, elements in their standard states have AH: = 0. Heat of formation values can be used The combustion of ethene, C2H4, occurs via the reaction to calculate the enthalpy change of any reaction. C2H4 (g) + 302 (g)→2CO2(g) + 2H20(g) Consider, for example, the reaction with heat of formation values given by the following table: 2NΟ (5) + Ο, (s) 2ΝO, (g) ΔΗρ (kJ/mol) Substance with heat of formation values given by the following table: C2H4 (g) 52.47 CO2 (g) -393.5 Substance (kJ/mol) H2O(g) -241.8 NO(g) 90.2 Calculate the enthalpy for the combustion of ethene. 02 (g) Express your answer to four significant figures and include the appropriate units. NO2(g) 33.2 • View Available Hint(s) Then the heat of formation for the overall reaction is ΔΗ ΔΗ (products) -ΔΗ; (reactants ) [2(90.2) + 0] HA ? 2(33.2) -114 kJ/mol…