1. Experimental Data Identity of the salt, a. Mass of salt [g] NaCl Trial 1 Trial 2 21.07 21.07 b. Molar Mass of salt [g/mol] 58.44 58.44 c. Moles of salt [mol] 0.3605 0.3605 d. Mass of water [g] 174.3 175.2 e. Initial temperature of water ['C] 20.9 21.1 f. Final temperature of mixture from graph ["C] 47,4 47.0 Show calculations for moles of salt. Report the results with correct number of significant figures. i.

1. Experimental Data Identity of the salt, a. Mass of salt [g] NaCl Trial 1 Trial 2 21.07 21.07 b. Molar Mass of salt [g/mol] 58.44 58.44 c. Moles of salt [mol] 0.3605 0.3605 d. Mass of water [g] 174.3 175.2 e. Initial temperature of water ['C] 20.9 21.1 f. Final temperature of mixture from graph ["C] 47,4 47.0 Show calculations for moles of salt. Report the results with correct number of significant figures. i.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.83PAE: 9.83 A student performing a calorimetry experiment combined 100.0 mL of 0.50 M HCl and 100.0 mL of...

See similar textbooks

Similar questions

One statement of the second law of thermodynamics is that heat cannot be turned completely into work. Another is that the entropy of the universe always increases. How are these two statements related?
Given the following information at 25C, calculate G at 25C for the reaction 2A(g)+B(g)3C(g) Substance Hf(kJ/mol) S(J/molK) A(g) 191 244 B(g) 70.8 300 C(g) 197 164 a 956 kJ b 956 kJ c 346 kJ d 346 kJ e 1.03 103 kJ
When vapors from hydrochloric acid and aqueous ammonia come in contact, they react, producing a white cloud of solid NH4C1 (Figure 18.9). HCI(g) + NH3(g) NH4Cl(s) Defining the reactants and products as the system under study: (a) Predict whether S(system), S(surroundings), S(universe), rH, and rG (at 298 K) are greater than zero, equal to zero, or less than zero; and explain your prediction. Verify your predictions by calculating values for each of these quantities. (b) Calculate the value of Kp for this reaction at 298 K.
The reaction between magnesium metal and water (l) produces solid magnesium hydroxide and hydrogen gas. Calculate G for the formation of one mole of Mg(OH)2 at 27C and at 39C.
9.83 A student performing a calorimetry experiment combined 100.0 mL of 0.50 M HCl and 100.0 mL of 0.50 M NaOH in a coffee cup calorimeter. Both solutions were initially at 20.0°C, but when the two were mixed, the temperature rose to 23.2°C. (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCl and 100.0 mL of 1.00 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why?
Hesss law is really just another statement of the first law of thermodynamics. Explain.
Given the thermochemical expression CaO(s) + 3C(s) CaC2(s) + CO(g) rH = 464.8 kJ/mol calculate the quantity of energy transferred when (a) 34.8 mol CO(g) is formed by this reaction. (b) A metric ton (1000 kg) of CaC2(s) is manufactured. (c) 0.432 mol carbon reacts with CaO(s).
Natural gas is mostly CH4. When it burns, the chemical reaction is CH4 g 2O2 g CO2 g 2H2O g The H of combustion of one mole of CH4 at 25.0 C is -890.9 kJ. Calculate q, w, and U under these conditions, assuming an external pressure of 1.07 atm.
9.20 State the first law of thermodynamics briefly in your own words.
Explain in your own words what is meant by the term entropy. Explain how both matter spread and energy spread are related to the concept of entropy.
What are the two ways that a final chemical state of a system can be more probable than its initial state?
With regard to exercise 2.50, how accurate do you think your answer is, and why?