2. Calculate the amount of heat required to raise the temperature of 950.0 mL of a solution from 22.5 °C to 38.0 °C if thesolution has a density of 1.04 g mL-l and a heat capacity of 4.08 J K-l g.3. This reaction: CH4(g) + 202(g) → CO2(g) + 2H2O(1) produces 56.0 kJ of heat when 1.00 g of methane is burned. Whatis the molar heat of combustion for CH4?4. In thermodynamics heat is represented by the letter 'q' and q is negative for processes which lose heat to the surroundings(i.e. exothermic processes). What is q for burning one mole of methane?5. What mass of methane would need to be burned in order to generate the heat required to raise the temperature of thesolution in question 2? (Hint: look at question 3 for some relevant data)6. In this lab class you will measure the enthalpy change for hydrochloric acid reacting with sodium hydroxide. What effect,if any, would using nitric acid instead of hydrochloric acid have on the enthalpy changes measured in this experiment?Why? (Hint: what is the actual reaction you are measuring the enthalpy change for?)

Since you have asked multiple question, we will solve the first question for you. If you want any…

2. Calculate the amount of heat required to raise the temperature of 950.0 mL of a solution from 22.5 °C to 38.0 °C if the solution has a density of 1.04 g mLl and a heat capacity of 4.08 J K-l g-l.

2. Calculate the amount of heat required to raise the temperature of 950.0 mL of a solution from 22.5 °C to 38.0 °C if the solution has a density of 1.04 g mLl and a heat capacity of 4.08 J K-l g-l.

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...

See similar textbooks

Similar questions

A certain chemical reaction releases 368.kJ of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 4.09J of heat energy to raise the temperature of this calorimeter by 1°C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 14.6°C. How would you calculate the number of moles of reactant that were consumed? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols.
1. A certain two-step process involves transfer of heat and work between the system and the surroundings. In the first step, the internal energy, AE, of the system increases by 115.4 J when 95.1 J of work is done on the system. In the second step, the internal energy of the system decreases by 32.2 J when 15.6 J of work is done on the surroundings. In the first step of the two-step process, how much heat, in Joules, was absorbed or released? b. How much heat, in Joules, was absorbed or released in the whole two-step process? a.
In parts 2, 3 and 4 of this lab, you will be conducting calorimetry experiments on neutralization reactions in solution. Two solutions (each of volume 2.5 mL) will be mixed together to initiate the reaction. What mass of water should be used in the calculation of the heat energy absorbed by the calorimeter? 2.5 g 5.0 g (since the two solutions are mixed together, the volumes and hence their masses are added together).
A 77.5g piece of brass is heated so that its temperature is 98.7◦C. Next,it is quickly placed in a calorimeter containing 102.76 g of water at 18.5◦C.Knowing that the final temperature is 23.5◦C, what is the specific heat of this alloy?Note: Brass is an alloy of copper and zinc. From 98.7 to 23.5◦C, this alloy does not changeno phase, it remains in solid form.
2. A calorimeter contains 100.0 g of water at 39.8 °C. A 12.78 g object at 100.0 ºC is placed inside the calorimeter. When equilibrium has been reached, the new temperature of the water and metal object is 40.6 °C. What is the specific heat of the metal?
Please don't provide handwritten solution ....
A 29.00 g sample of metal alloy is heated to 92.6 °C; then placed in 55.23 g of water in an insulated calorimeter at 21.3 °C. If the final temperature of the system is 43.9 °C, what is the specific heat of the metal alloy? Assume that the calorimeter absorbs a negligible amount of heat.
4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
During an experiment, a student adds 1.05 g of calcium metal to 200.0 mL of 0.75 M HCI. The student observes a temperature increase of 17.0 °C for the solution. Assuming the solution's final volume is 200.0 mL, the density is 1.00 g/mL, and the specific heat is 4.184 J/(g.°C), calculate the heat of the reaction, AHrxn - Ca(s) + 2 H*(aq) → Ca+(aq) + H, (g) %3D kJ/mol
THe G.R.A.S.P. method
A certain chemical reaction releases 269. kJ of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 3.21 J of heat energy to raise the temperature of this calorimeter by 1 °C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 5.0 °C. How would you calculate the number of moles of reactant that were consumed? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols. moles consumed = x10 010 X Ś
An ideal gas in a cylinder fitted with a piston expands at constant temperature from a pressure of 9 atm and a volume of 4.,0 L to a final volume of 13 L against a constant opposing pressure of 1.4 atm. How much heat does the gas absorb, expressed in units of L atm (liter x atm)? Latm