Given Information: NA = 6.022 x1023 w--PAV AE= q +w 9cal = CcalAT q= CAT -grxn- 9cal q= mCgAT M= mol/L milli (m): 1x103 base units kilo (k): 1x10 base units Calculate the molar enthalpy of reaction (AH) in J/mol if 4.75 grams of a substance (formula mass of 150.00 g/mol) is burned in a calorimeter, and the temperature rises by 3.50°C. The heat capacity of the calorimeter is 20.0 1/°c.

Given Information: NA = 6.022 x1023 w--PAV AE= q +w 9cal = CcalAT q= CAT -grxn- 9cal q= mCgAT M= mol/L milli (m): 1x103 base units kilo (k): 1x10 base units Calculate the molar enthalpy of reaction (AH) in J/mol if 4.75 grams of a substance (formula mass of 150.00 g/mol) is burned in a calorimeter, and the temperature rises by 3.50°C. The heat capacity of the calorimeter is 20.0 1/°c.

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

Please solve this question and show all your work, thank you
AT = 2 Calculate the specific heat of a piece of lead if 500 grams of lead absorbs 35,000 Joules of heat, and the temperature changes from 30 °C to 65 °C. AE = m = C = AT =
When a chemist burns ammonia according to the reaction below she finds that the reaction releases heat. (It is exothermic.) 4NH3(g) + 3O2(g) 2N2(g) + 6H2O(g) The enthalpy of the reaction DH = -1267 kJ. What is the enthalpy change (in kJ) when 3 grams of ammonia are burned?
[References) The value for A,H for C3H3(g) is-104.7 kJ/mol. Choose a balanced chemical equation for the formation of one mole of C3Hs (g) from the elements in their standard states. O3 C(s) +4 H2(g) → C,Hs (g) C(s) + H2(g) → C3HS(g) O3 C(g) +4 H2(g) → C3HS (g) O3 C(s) + 8 H2 (g) → 2 C,Hs (g) Submit Answer Try Another Version 10 item attempts remaining
1. a. Calculate the enthalpy change for the reaction below: NO(g) + ½ 0,(g) →NO,(g) Using Hess's law and the following information: NO(g) ½ N,(g) + O2(g) →½ N,(g)+ ½ O,g) →NO,(g) AH°=– 90.33 kJ AH°=+ 33.8 N b. Draw the enthalpy diagram.
In a calorimeter, a 75.0 g piece of metal at 98.6 *C is submerged in 100.0 g of water, that is initially at 21.8 *C. When the metal and water reach thermal equilibrium, the temperature is 26.2 *C. What was the heat capacity of the metal (3 sig figs)?
2 NO(g) N2(g) + O2(g) H = -180.7 kJ 2 NO(g) + O2(g) 2 NO2(g) H = -113.1 kJ 2 N2O(g) 2 N2(g) + O2(g) H = -163.2 kJ Use Hess's law to calculate H for the reaction below.3 NO(g) N2O(g) + NO2(g)H = _____k J
|| Question 15 A calorimeter holds 25 g water at 25.0°C. A sample of hot iron is added to the water, and the final temperature of the water and iron is 30.0°C. What is the change in en- thalpy associated with the change in the water's temperature? Note: The specific heat of water is 4.18 g°c. Use the formula AH = - cm AT %3D Show your work. IUS
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
The combustion of butane produces heat according to the equation2C4H10(g) + 13O2(g) --> 8CO2(g) + 10H2O(l) ΔH = -5,314.0 kJ What is the change in heat if 13.98 g C4H10 (58.12g/mol) reacts?(Answer should have one place after the decimal. Watch the sign)
Methane (CH4) burns in oxygen via the following reaction:CHa(g) + 202(g) > CO2(g) + 2H20(g) ; AH= -890 kJWhat is the enthalpy change for the combustion of 148.2 grams of methane ?
A coffee-cup calorimeter contains 30 mL of water with an initial temperature of 24.8°C. An unknown sample with a mass of 12.618 grams was placed inside making the water temperature rise up to 25.5°C. The initial temperature of the metal was 79.9°C. (Water: density = 1g/mL; specific heat = 4.184 J/g-°C). 1. How much heat (in Joules) was absorbed by the water in the calorimeter?