You mix 5 moles of H2 at 300 K with 5 moles of He at 360...

Question

Question

You mix 5 moles of H2 at 300 K with 5 moles of He at 360 K in a perfectly insulated calorimeter. Is the final temperature higher or lower than 330 K?

Answer 1

Answer #1

Answer 2

Similar Homework Help Questions

If you mix 2.00 moles of H2, 1.00 moles of N2 and 2.00 moles of NH3...

If you mix 2.00 moles of H2, 1.00 moles of N2 and 2.00 moles of NH3 in a one liter vessel at 472 C. Will H2 and N2 react to form NH3?
a cylinder contains 10 moles of an ideal gas at a temperature of 300 K. The...

a cylinder contains 10 moles of an ideal gas at a temperature of 300 K. The gas is compressed at constant pressure until the final volume equals 0.77 times the initial volume. The molar heat capacity at constant volume of the gas is 24.0 j/mol. What is the heat absorbed by the gas in kJ
7. A 0.2 moles of diatomic gas are contained in a cylinder at 300 K and atmospheric pressure 1*10...

7. A 0.2 moles of diatomic gas are contained in a cylinder at 300 K and atmospheric pressure 1*10^5 Pa. The gas receives 1000 J of heat in an ideal adiabatic transformation. Calculate the change of internal energy, the work done on the gas and the final volume and temperature of the gas.

For an isolated system of one mole of He initially at 300 K and a pressure...

For an isolated system of one mole of He initially at 300 K and a pressure of 15 atm expands to a final pressure of 1 atm, and the final temperature of 188 K. During this process, the expansition work is 1.40x103 J. Calculate q, w, ΔE and ΔH
Two moles of an ideal monoatomic gas is initially at 300 K and 1 bar of...

Two moles of an ideal monoatomic gas is initially at 300 K and 1 bar of pressure inside a cylinder with a frictionless piston. a) Calculatethekineticenergyforthissystemat300K. b) Calculate the heat capacity at constant volume. c) How much heat is required to increase the temperature by 10°C. d) What is the final pressure after heating, if there is no change in volume.
A gaseous mixture is composed of 2 moles of Ne, 3 moles of He, and 5...

A gaseous mixture is composed of 2 moles of Ne, 3 moles of He, and 5 moles of N2. The mixture is contained with a 10-liter vessel. If the partial pressure of the N2 is 10atm, what is the temperature of the mixture? R= 0.0821 L × atm/mol × °K

1. If 2.6 moles of Mg were mixed with HCl, how many moles of H2 gas would you expect to be produced? NG 3 2. If th...

1. If 2.6 moles of Mg were mixed with HCl, how many moles of H2 gas would you expect to be produced? NG 3 2. If the ambient pressure is 1.009 atm and the temperature is 298 K, what volume (in liters) would moles of H, occupy? NG| 3
5. A student determined AH for the reaction below using the procedure you used in this...

5. A student determined AH for the reaction below using the procedure you used in this lab but the student made mistakes. For each of the following mistakes, state whether the magnitude of the student's AH would be higher, lower, or no different from the correct AH value. Explain each answer. Mg(s) + 2HCl(aq) + MgCl2(aq) + H2(g) a. The student dropped some Mg on the lab bench while transferring it to the calorimeter after weighing it. b. The student...
a) A helium-filled weather balloon has a volume of 521 L at 17.9°C and 758 mmHg....

a) A helium-filled weather balloon has a volume of 521 L at 17.9°C and 758 mmHg. It is released and rises to an altitude of 5.22 km, where the pressure is 472 mmHg and the temperature is –14.1°C. The volume of the balloon at this altitude is ______L b) A sample of krypton gas occupies a volume of 6.19 L at 56.0°C and 382 torr. If the volume of the gas sample is decreased to 4.90 L, while its temperature...

Five moles of an ideal gas expands isothermally at 300 K from an initial volume of...

Five moles of an ideal gas expands isothermally at 300 K from an initial volume of 100 L to a final volume of 500 L. Calculate: (a) the maximum work the gas can deliver, (b) the heat accompanying the process, (c) ∆S for the gas. (Please explain why did you use the equation, what conditions did you see from the question, etc)