Question

please help me with these three questions! q1. In the coffee cup calorimeter , 0.853 g...

please help me with these three questions!

q1. In the coffee cup calorimeter , 0.853 g of MgO were added to 71.4 ml of diluted aqueous hydrochloric acid. If temperature is increased by 5.9 degrees C, wht is q(rxn) in (KJ)? assume that q (cal) is small enough to be negligible. the specific heat capacity of the solution is similar to water (c=4.184), and the density of dilute hydrochloric acid solution is 1.00 g/ml.


q2.explain how the signs of q(rxn) and initial and final temperature are related to wether a reaction is exothromic or endo thromic?

q2. two seprate coffee cup calorimetric expriment are conducted. one expriment has the calorimeter and all the reagents at room temperature and other has calorimeter and all the reagents at higher temperature. all other experimental conditions are held constant
i) provide one thermochemical values that would be different between the two trials other than T(initial).
ii) provide one thermochemical values that would be consistent between two trails.


0 0
Add a comment Improve this question Transcribed image text
Answer #1

0 ☆ Myo = 0.853 gm (Males Mago 0.853 gm 40 g/mol Il 0.0 3995 * Mgo Ho Mg Colla Malohida tahl + 2 Holoces My clacant (Neutraliof2 2 ② As reaction is exothermic, heat will be released and that heat will be gained by Solution. increase. Temperature of Sol

Add a comment
Know the answer?
Add Answer to:
please help me with these three questions! q1. In the coffee cup calorimeter , 0.853 g...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • 1. A coffee cup calorimeter was used for the neutralization reaction of 100 mL of 1.00...

    1. A coffee cup calorimeter was used for the neutralization reaction of 100 mL of 1.00 M hydrochloric acid with 100 mL of 1.20 M sodium hydroxide. The initial temperature was 22.88 °C and the final temperature was 29.39 °C. Calculate the calorimeter constant for the reaction. HCl (aq) + NaOH (aq) NaCl (aq) + H2O (∆H°rxn = -58.3 kJ/mol) 2. The same calorimeter was used for the dissolution of 8.86 g sample of lithium chloride in 100.0 mL of...

  • In one of the General Chemistry experiments, you used a coffee-cup calorimeter to measure the heat...

    In one of the General Chemistry experiments, you used a coffee-cup calorimeter to measure the heat of neutralization of selected acid-base reactions. The calorimeter consisted of two nested Styrofoam cups with a cardboard lid. A temperature probe was lowered in the solution through a hole in the lid. Is a coffee-cup calorimeter a constant-volume or a constant-pressure device? Is a coffee-cup calorimeter adiabatic? The coffee-cup calorimeter was calibrated by using the neutralization reaction between sodium hydroxide and hydrochloric acid. The...

  • When 0.615 g Mn is combined with enough hydrochloric acid to make 100.0 mL of solution in a coffee-cup calorimeter

    When 0.615 g Mn is combined with enough hydrochloric acid to make 100.0 mL of solution in a coffee-cup calorimeter, all of the Mn reacts, raising the temperature of the solution from 24.0 °C to 29.4°C. Find ΔHrxn for the reaction as written. (Assume that the specific heat capacity of the solution is 4.18 J/g °C and the density is 1.00 g/mL.) Express your answer using three significant figures.

  • Part A In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used....

    Part A In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used. The initial temperature of the calorimeter is 23.0 °C. If 3.10 g of CaCl2 is added to the calorimeter what will be the final temperature of the solution in the calorimeter? The heat of solution AHoln of CaCla is -82.8 kJ/mol Assume that the specific heat of the solution formed in the calorimeter is the same as that for pure water. C, 4.184 J/g...

  • In a coffee-cup calorimeter, 100.0 mL of 1.76 M HNO3 and 100.0 mL of 1.22 M...

    In a coffee-cup calorimeter, 100.0 mL of 1.76 M HNO3 and 100.0 mL of 1.22 M Ca(OH)2 are mixed. Both solutions were originally at 24.6 °C. The maximum temperature observed during the experiment is 36.4 °C. Calculate the enthalpy change for the neutralization reaction that occurs. Assume the mixture in the coffee cup has the same density and specific heat as pure water. *This is from a problem sheet that's for extra practice. It gives me the answer of -112...

  • A 2.490-g sample of cadmium metal completely reacts    when placed in a coffee cup calorimeter that...

    A 2.490-g sample of cadmium metal completely reacts    when placed in a coffee cup calorimeter that contains 75.0 mL of a dilute sulfuric acid solution (aqueous) (density of 1.03 g/mL) to produce hydrogen gas and dissolved cadmium sulfate.  The chemical reaction is exothermic causing the temperature of the resulting aqueous solution to change from 21.5oC to 32.5oC.   Write a balanced chemical equation for the chemical reaction that occurs. Find the enthalpy change, in kJ/mol, for the chemical reaction, assuming the specific...

  • Part 2, find AH°rxn =kJ/mol Two solutions are mixed in a coffee cup calorimeter both are...

    Part 2, find AH°rxn =kJ/mol Two solutions are mixed in a coffee cup calorimeter both are initially at 22.60°C. When a 100.0 mL volume of 1.00 M AgNO3 solution is mixed with a 100.0 mL sample of 0.500 M NaCl solution, the temperature in the calorimeter rises to 28.30°C (assume no heat is lost to the surroundings and the density and heat capacity of the solutions is the same as that of water). Determine the AHºrxn for the reaction as...

  • In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.0 mL of 1.00...

    In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.0 mL of 1.00 M HCl are mixed. Both solutions were originally at 24.6°C. After the reaction, the final temperature is 31.3°C. Given that the density of the NaCl solution is 1.038 g/mL and he specific of NaCl solution is 3.87 J/g-°C, calculate the ΔHneut/mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings. Part A. ) Why are the density...

  • The aluminum cup inside your calorimeter weighs 41.55 g. You add 59.21 g of 1.0 M...

    The aluminum cup inside your calorimeter weighs 41.55 g. You add 59.21 g of 1.0 M acetic acid solution and 50.03 g of 1.0 M sodium hydroxide solution to the calorimeter. Both solutions have an initial temperature of 19.9 °C, and the final temperature after addition is 26.8 °c. What is the molar enthalpy of neutralization, in units of kJ/mol? Assume that: the calorimeter is completely insulated the heat capacity of the empty calorimeter is the heat capacity of the...

  • 6.A 12.8 g sample of ethanol (C,H,OH) is burned in a calorimeter with a heat capacity...

    6.A 12.8 g sample of ethanol (C,H,OH) is burned in a calorimeter with a heat capacity of 5.65 kJ/°C. Assume the heat from the sample is negligible compared to the calorimeter. Determine the initial temperature of the calorimeter if the final temperature is 85.7°C. The molar mass of ethanol is 46.07 g/mol. С-Н,ОН , + 3 О,ее — 2 СОде + 3 Н,0 qrxn -1235 kJ 7. Two solutions, initially at 24.60 °C, are mixed in a coffee cup calorimeter...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT