URGENT If you take four gas samples with the following pressures: 12.3 atm, 56.7 atm, 1.09 atm, and 32.6 atm. What is the total pressure of your samples? *
24,782 atm
74.9 atm
0.035 atm
102.69 atm

The total pressure of gas samples are 102.69 atmosphere, if the gas samples have pressure of 12.3 atmosphere, 56.7 atmosphere, 1.09 atmosphere, and 32.6 atmosphere.

Explanation:

The given is,

                 Gas samples pressure are,

                 12.3 atmosphere, 56.7 atmosphere, 1.09 atmosphere, and 32.6 atmosphere

Step:1

              From the  Dalton’s Law of Partial Pressure,

              The total pressure of a mixture of gases can be defined as the sum of the pressures of each individual gas,

                                    .........................(1)

              Where, ., etc. are the pressure of gas sample respectively 1,2,3.,etc.

Step:2

               From the given,

                                  = 12.3 atmosphere    

                                  = 56.7 atmosphere

                                  = 1.09 atmosphere

                                  = 32.6 atmosphere

                Equation (1) becomes,

                                       = 12.3 + 56.7 + 1.09 + 32.6

                                       = 102.69 atmosphere

                Total pressure of gas samples are = 102.69 atmosphere

Result:

              The total pressure of gas samples are 102.69 atmosphere, if gas samples have pressure of 12.3 atmosphere, 56.7 atmosphere, 1.09 atmosphere, and 32.6 atmosphere.

i'm assuming that the correct answer is indeed the first one/ "a"..

1. a)c-14 has two more protons

2. d)they have different numbers of protons, neutrons, and valence electrons; they are all gases at room temperature.

3. c) iron and nickel.