What is the temperature of the high-temperature reservoir of a process that has an efficiency of 44.0% (0.440) and a low-temperature reservoir at 150°C?
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What is the temperature of the high-temperature reservoir of a process that has an efficiency of 44.0% (0.440) and a low-temperature reservoir at 150°C?
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- Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.Using the data below, calculate ∆Hrxn for: HCl(aq) + NH3(aq) ® NH4Cl(aq) The reaction of 50.0 mL of 1.00 M HCl with 50.0 mL of 1.00 M NH3 causes a temperature rise of 6.4 ̊C in the resulting 100.0 mL of solution. The NH4Cl solution has density 1.005 g/mL and specific heat capacity 3.97 J/g ̊C. Pay careful attention to sig figs in this problem.A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 4.70 kg of water at 37.5C. During the reaction 92.8kJ of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. Heat capacity of water is 4.18J.g-1.K-1. Round your answer to 3
- One kilogram of boiling water is poured into an empty thermos whose mass is 1kg and whose temperature is 25oC. No heat is lost from the thermos. The specific heats of water and the thermos are 1 and 0.5 kcal/kg-oC, respectively. Their final temperature is?The following reaction: 2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l)was studied in a coffee cup calorimeter. In the experiment, 100. mL portions each of 1.00 M aqueous NaOH and H2SO4, each at 24.0°C were mixed. The maximum temperature achieved was 30.6°C. Neglect the heat capacity of the cup and the thermometer, and assume the solution of products has a density of 1.00 g/mL and a specific heat capacity of 4.18 J/g K.What is the heat of reaction, (Delta)Hrxn, for the reaction as written in kJ?a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) Show your working below:
- A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 68.5 mL water (where X is a hypothetical metal): X + 2 HCI ---> XCI2 + H2 In this process, the water temperature rose from 25.0 °C to 33.3 °C. If 0.00629 mol of "X" was consumed during the reaction, what is ?rH of this reaction in kJ mol^-1with respect to "X"? The specific heat of water is 4.184 J g-¹ °C-¹NH4NO3 + H2O -> NH4NO DeltaH = +25.7kJ What is the final temperature in an activated cold pack that contains 50.0g of NH4NO3 dissolved in 125mL of water? Assume a specific heat of 4.184J/g.C for the solution, an initial temperature of 25.0C and no heat transfer between the cold pack and the environment.Under a constant pressure of 1.00 atm, at 25.00oC, the combustion of 1.136 g of C6H12O3(l) raises the temperature of 2.000 kg of water by 2.617 degrees Celsius. Combustion is the reaction of a substance with O2(g) to give CO2(g) and H2O(l). The specific heat capacity of water is 4.184 J K-1 g-1. Ignore the heat capacities of any containers.With the help of the data above, find the values of ΔH, ΔU, Q, and W for the combustion of 1.000 mol of C6H12O3(l) in a steel container of constant volume at 25.00oC.
- The n-butane is converted into isobutane in an isomerization reactor, which operates isothermally at 149°C. Suppose that the reactor is fed with a mixture containing 93% mole of n-butane, 5% isobutane and 2% HCl at 149°C and that a 40% conversion of n-butane is achieved. How much heat in KJ/m3 (STP) of the feed, should be supplied or extracted from the reactor?A quantitity of 100mL of 0.500 MHCl was mixed with 50 mL of 0.500M NaOH in a constant pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and NaOH solutions was the same, 20ºC, and the final temperature of the mixed solution was 22.3ºC. Calculate the heat change for neutralization reaction on a molar baisis.In constant pressure calorimeter 75.0 ml is mixed with 1.25 M Hydrocloric acid solution is mixed with 75.0 ml of 1.25 M Sodium hydroxide solution. the density of the final solution is 1.00g/ml and the the solution both initially 21.45c, reach a maximum temperature of 28.32c when mixed. based on this information, and estimating the solution's heat capacity as 4.18Jg-1c-1, what is the amount of heat in Kilojoules, transferred in this reaction?