From the data above, calculate the molar mass of the vapor. If 16.0 g of O_2 and

Question

From the data above, calculate the molar mass of the vapor. If 16.0 g of O_2 and 4.40 g of CO_2 are placed in a 5.00 L container at 21.0 degree C, what is the pressure of this mixture of gases? A metal that weighs 6.25 g is at 50.0 degree C. When placed into a calorimeter with 30.00 ml of water at 23.0 degree C the temperature of the water rose to 27.0 degree C. The specific heat of water is 4.184 J/K·g. What is the specific heat of the metal? When a 10.00 g sample of NaOH was dissolved in a calorimeter with 100.0 g of water, the temperature rose from 23.9 degree C to 33.0 degree C. Calculate Delta H (in kJ/mol) for the solution process: NaOH (s) rightarrow Na+ (aq) + OH- (aq) Assume it's a perfect calorimeter and that the specific heat of the solution is the same as that of pure water.

Explanation / Answer

5)
It is contunation. can't be answered without previous parts

6)
number of moles of O2 = mass of O2 / molar mass of O2
= 16.0/32
= 0 .5 mol

number of moles of CO2 = mass of CO2 / molar mass of CO2
= 4.40/44
= 0 .1 mol

total number of moles,
n = 0.1+ 0.5 mol = 0.6 mol

P = ?
V = 5.00 L
T = 21.0 oC = (21 + 273) K = 294 K

use:
P*V = n*R*T
P*5.00 = 0.6*0.0821*294
P = 2.90 atm

Answer: 2.90 atm

I am allowed to answer only 1 question at a time

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